?Solution \(A\) has a \(pH\) of \(4.5\), and solution \(B\) has a \(pH\) of \(6.7\)

Indicate whether each of the following statements is characteristic of an acid, a base, or both: a. has a sour taste b. neutralizes bases c. produces H+ ions in water d. is named barium hydroxide e. is an electrolyte

Indicate whether each of the following statements is characteristic of an acid, a base, or both: a. neutralizes acids b. produces OH- ions in water c. has a slippery feel d. conducts an electrical current in solution e. turns litmus red

Name each of the following acids or bases: a. \(\mathrm{HCl}\) b. \(\mathrm{Ca}(\mathrm{OH})_{2}\) c. \(\mathrm{HClO}_{4}\) d. \(\mathrm{Sr}(\mathrm{OH})_{2}\) e. \(\mathrm{H}_{2} \mathrm{SO}_{3}\) f. \(\mathrm{HBrO}_{2}\) Equation Transcription: HCl Ca(OH)2 HCIO4 Sr(OH)2 H2SO3 HBrO2 Text Transcription: HCl Ca(OH)_2 HCIO_4 Sr(OH)_2 H_2SO_3 HBrO_2

Name each of the following acids or bases: a. \(\mathrm{Al}(\mathrm{OH})_{3}\) b. \(\mathrm{HBr}\) c. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) d. \(\mathrm{KOH}\) e. \(\mathrm{HNO}_{2}\) f. \(\mathrm{HClO}_{2}\) Equation Transcription: Al(OH)3 HBr H2SO4 KOH HNO2 HClO2 Text Transcription: Al(OH)_3 HBr H_2SO_4 KOH HNO_2 HClO_2

Write formulas for each of the following acids and bases: a. rubidium hydroxide b. hydrofluoric acid c. phosphoric acid d. lithium hydroxide e. ammonium hydroxide f. periodic acid

Write formulas for each of the following acids and bases: a. barium hydroxide b. hydroiodic acid c. nitric acid d. strontium hydroxide e. acetic acid f. hypochlorous acid

Identify the reactant that is a Br?nsted-Lowry acid and the reactant that is a Br?nsted-Lowry base in each of the following: a. \(\mathrm{HI}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{l}^{\prime}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) b. \(\mathrm{F}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \leftrightarrows \mathrm{HF}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})\) c. \(\mathrm{H}_{2} \mathrm{~S}(\mathrm{aq})+\mathrm{C}_{2} \mathrm{H}_{5}-\mathrm{NH}_{2}(\mathrm{aq}) \leftrightarrows \mathrm{HS}^{\prime}(\mathrm{aq})+\mathrm{C}_{2} \mathrm{H}_{5}-\mathrm{NH}_{2}{ }^{+}(\mathrm{aq})\) Equation Transcription: Hl(aq) + H2O(l) ? I-(aq) + H3O+(aq) F-(aq) + H2O(l) ? HF(aq) + OH-(aq) H2S(aq) + C2H5 ? NH2(aq) ? HS-(aq) + C2H5 ? NH3+(aq) Text Transcription: Hl(aq) + H_2O(l) right arrow I^-(aq) + H_3O^+(aq) F^-(aq) + H_2O(l) left right arrow HF(aq) + OH^-(aq) H_2S(aq) + C_2H_5 ? NH2(aq) left right arrow HS^-(aq) + C_2H_5 ? NH_3^+(aq)

Identify the reactant that is a Br?nsted-Lowry acid and the reactant that is a Br?nsted-Lowry base in each of the following: a. \(\mathrm{CO}_{3}{ }^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{HCO}_{3} \cdot(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) c. \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{\cdot}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \leftrightarrows \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) Equation Transcription: CO32-(aq) + H2O(l) ? HCO3-(aq) + OH-(aq) H2SO4(aq) + H2O(l) ? HSO4-(aq) + H3O+(aq) C2H3O2-(aq) + H3O+(aq) ? HC2H3O2(aq) + H2O(l) Text Transcription: CO_3^2-(aq) + H_2O(l) left right arrow HCO_3^-(aq) + OH^-(aq) H_2SO_4(aq) + H_2O(l) left right arrow HSO_4^-(aq) + H_3O^+(aq) C_2H_3O_2^-(aq) + H_3O^+(aq) left right arrow HC_2H_3O_2(aq) + H_2O(l)

Write the formula for the conjugate base for each of the following acids: a. \(\mathrm{HF}\) b. \(\mathrm{H}_{2} \mathrm{O}\) c. \(\mathrm{H}_{2} \mathrm{PO}_{3}^{-}\) d. \(\mathrm{HSO}_{4}^{-}\) e. \(\mathrm{HClO}_{2}\) Equation Transcription: HF H2O H2PO3- HSO4- HCIO2 Text Transcription: HF H_2O H_2PO_3^- HSO_4^- HCIO_2

Write the formula for the conjugate base for each of the following acids: a. \(\mathrm{HCO}_{3}^{-}\) b. \(\mathrm{CH}_{3}-\mathrm{NH}_{3}{ }^{+}\) c. \(\mathrm{HPO}_{4}{ }^{2-}\) d. \(\mathrm{HNO}_{2}\) e. \(\text { HBrO }\) Equation Transcription: HCO3- CH3 ? NH3+ HPO42- HNO2 HBrO Text Transcription: HCO_3^- CH_3 ? NH_3^+ HPO_4^2- HNO_2 HBrO

Write the formula for the conjugate acid for each of the following bases: a. \(\mathrm{CO}_{3}^{2-}\) b. \(\mathrm{H}_{2} \mathrm{O}\) c. \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) d. \(\text { Br }\) e. \(\mathrm{ClO}_{4}^{-}\) Equation Transcription: CO32- H2O H2PO4- Br- CIO4- Text Transcription: CO_3^2- H_2O H_2PO_4^- Br^- CIO_4^-

Write the formula for the conjugate acid for each of the following bases: a. \(\mathrm{SO}_{4}^{2-}\) b. \(\mathrm{CN}^{-}\) c. \(\mathrm{NH}_{3}\) d. \(\mathrm{ClO}_{2}^{-}\) e. \(\mathrm{HS}^{-}\) Equation Transcription: SO42- CN- NH3 CIO2- HS- Text Transcription: SO_4^2- CN^- NH_3 CIO_2^- HS^-

Identify the Brønsted-Lowry acid-base pairs in each of the following equations: a. \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{HCO}_{3}{ }^{-}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) b. \(\mathrm{HCN}(\mathrm{aq})+\mathrm{NO}_{2}^{-}(\mathrm{aq}) \leftrightarrows \mathrm{CN}(\mathrm{aq})+\mathrm{HNO}_{2}(\mathrm{aq})\) c. \(\mathrm{CHO}_{2}^{\prime}(\mathrm{aq})+\mathrm{HF}(\mathrm{aq}) \leftrightarrows \mathrm{HCHO}_{2}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq})\) Equation Transcription: H2CO3(aq) + H2O(l) ? HCO3-(aq) + H3O+(aq) HCN(aq) + NO2-(aq) ? CN-(aq) + HNO2(aq) CHO2-(aq) + HF(aq) ? HCHO2(aq) + F-(aq) Text Transcription: H_2CO_3(aq) + H_2O(l) left right arrow HCO_3^-(aq) + H_3O^+(aq) HCN(aq) + NO_2^-(aq) left right arrow CN^-(aq) + HNO_2(aq) CHO_2^-(aq) + HF(aq) left right arrow HCHO_2(aq) + F-(aq)

Identify the Brønsted-Lowry acid-base pairs in each of the following equations: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \leftrightarrows \mathrm{H}_{2} \mathrm{PO}_{4}^{-}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) b. \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \leftrightarrows \mathrm{H}_{2} \mathrm{PO}_{4}^{-}(\mathrm{aq})+\mathrm{NH}_{4}^{+}(\mathrm{aq})\) c. \(\mathrm{HNO}_{2}(\mathrm{aq})+\mathrm{C}_{2} \mathrm{H}_{5}-\mathrm{NH}_{2}(\mathrm{aq}) \leftrightarrows \mathrm{C}_{2} \mathrm{H}_{5}-\mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{NO}_{2}^{-}(\mathrm{aq})\) Equation Transcription: H3PO4(aq) + H2O(l) ? H2PO4-(aq) + H3O+(aq) H3PO4(aq) + NH3(aq) ? H2PO4-(aq) + NH4+(aq) HNO2(aq) + C2H5 ? NH2(aq) ? C2H5 ? NH3+(aq) + NO2-(aq) Text Transcription: H_3PO_4(aq) + H_2O(l) left right arrow H_2PO_4^-(aq) + H_3O^+(aq) H_3PO_4(aq) + NH_3(aq) left right arrow H_2PO_4^-(aq) + NH_4^+(aq) HNO_2(aq) + C_2H_5 ? NH_2(aq) left right arrow C_2H_5 ? NH_3^+(aq) + NO_2^-(aq)

When ammonium chloride dissolves in water, the ammonium ion, \(\mathrm{NH}_{4}{ }^{+}\), acts as an acid. Write a balanced equation for the reaction of the ammonium ion with water. Equation Transcription: NH4+ Text Transcription: NH_4^+

When sodium carbonate dissolves in water, the carbonate ion, \(\mathrm{CO}_{3}^{2-}\), acts as a base. Write a balanced equation of the carbonate ion with water. Equation Transcription: CO32- Text Transcription: CO_3^2-

What is meant by the phrase "A strong acid has a weak conjugate base"?

What is meant by the phrase "A weak acid has a strong conjugate base"?

Identify the stronger acid in each of the following pairs: a. \(\mathrm{HBr} \text { or } \mathrm{HNO}_{2}\) b. \(\mathrm{H}_{3} \mathrm{PO}_{4} \text { or } \mathrm{HSO}_{4}^{-}\) c. \(\mathrm{HCN} \text { or } \mathrm{H}_{2} \mathrm{CO}_{3}\) Equation Transcription: HBr or HNO2 H3PO4 or HSO4- HCN or H2CO3 Text Transcription: HBr or HNO_2 H_3PO_4 or HSO_4^- HCN or H_2CO_3

Identify the stronger acid in each of the following pairs: a. \(\mathrm{NH}_{4}{ }^{+} \text {or } \mathrm{H}_{3} \mathrm{O}^{+}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4} \text { or } \mathrm{HCl}\) c. \(\mathrm{H}_{2} \mathrm{O} \text { or } \mathrm{H}_{2} \mathrm{CO}_{3}\) Equation Transcription: NH4+ or H3O+ H2SO4 or HCI H2O or H2CO3 Text Transcription: NH_4^+ or H_3O^+ H_2SO_4 or HCI H_2O or H_2CO_3

Identify the weaker acid in each of the following pairs: a. \(\mathrm{HCl} \text { or } \mathrm{HSO}_{4}^{\circ}\) b. \(\mathrm{HNO}_{2} \text { or HF }\) c. \(\mathrm{HCO}_{3}^{-} \text {or } \mathrm{NH}_{4}^{+}\) Equation Transcription: HCI or HSO4- HNO2 or HF HCO3- or NH4+ Text Transcription: HCI or HSO_4^- HNO_2 or HF HCO_3^- or NH_4^+

Identify the weaker acid in each of the following pairs: a. \(\mathrm{HNO}_{3} \text { or } \mathrm{HCO}_{3}^{-}\) b. \(\mathrm{HSO}_{4}^{-} \text {or } \mathrm{H}_{2} \mathrm{O}\) c. \(\mathrm{H}_{2} \mathrm{SO}_{4} \text { or } \mathrm{H}_{2} \mathrm{CO}_{3}\) Equation Transcription: HNO3 or HCO3- HSO4- or H2O H2SO4 or H2CO3 Text Transcription: HNO_3 or HCO_3^- HSO_4^- or H_2O H_2SO_4 or H_2CO_3

Predict whether each of the following reactions contains mostly reactants or products at equilibrium: a. \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{HCO}_{3}{ }^{-}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) b. \(\mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{NH}_{3}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) c. \(\mathrm{HNO}_{2}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \leftrightarrows \mathrm{NO}_{2} \cdot(\mathrm{aq})+\mathrm{NH}_{4}{ }^{+}(\mathrm{aq})\) Equation Transcription: H2CO3(aq) + H2O(l) ? HCO3-(aq) + H3O+(aq) NH4+(aq) + H2O(l) ? NH3(aq) + H3O+(aq) HNO2(aq) + NH3(aq) ? NO2-(aq) + NH4+(aq) Text Transcription: H_2CO_3(aq) + H_2O(l) left right arrow HCO_3^-(aq) + H_3O^+(aq) NH_4^+(aq) + H_2O(l) left right arrow NH_3(aq) + H_3O^+(aq) HNO_2(aq) + NH_3(aq) left right arrow NO_2^-(aq) + NH_4^+(aq)

Predict whether each of the following reactions contains mostly reactants or products at equilibrium: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{PO}_{4}{ }^{-}(\mathrm{aq})\) b. \(\mathrm{CO}_{3}{ }^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \leftrightarrows \mathrm{OH}^{-}(\mathrm{aq})+\mathrm{HCO}_{3}{ }^{\circ}(\mathrm{aq})\) c. \(\mathrm{HS}^{-}(\mathrm{aq})+\mathrm{F}^{\cdot}(\mathrm{aq}) \leftrightarrows \mathrm{HF}(\mathrm{aq})+\mathrm{S}^{2-}(\mathrm{aq})\) Equation Transcription: H3PO4(aq) + H2O(l) ? H3O+(aq) + H2PO4-(aq) CO32-(aq) + H2O(l) ? OH-(aq) + HCO3-(aq) HS-(aq) + F-(aq) ? HF(aq) + S2-(aq) Text Transcription: H_3PO_4(aq) + H_2O(l) left right arrow H_3O+(aq) + H_2PO_4-(aq) CO_3^2-(aq) + H_2O(l) left right arrow OH-(aq) + HCO_3-(aq) HS^-(aq) + F^-(aq) left right arrow HF(aq) + S^2-(aq)

Write an equation for the acid-base reaction between ammonium ion and sulfate ion. Why does the equilibrium mixture contain mostly reactants?

Write an equation for the acid-base reaction between nitrous acid and hydroxide ion. Why does the equilibrium mixture contain mostly products?

Answer True or False for each of the following: A strong acid a. is completely dissociated in aqueous solution b. has a small value of \(\mathrm{K}_{\mathrm{a}}\). c. has a strong conjugate base d. has a weak conjugate base e. is slightly dissociated in aqueous solution Equation Transcription: Ka Text Transcription: K_a

Answer True or False for each of the following: A weak acid a. is completely dissociated in aqueous solution b. has a small value of \(\mathrm{K}_{\mathrm{a}}\). c. has a strong conjugate base d. has a weak conjugate base e. is slightly dissociated in aqueous solution Equation Transcription: Ka Text Transcription: K_a

Consider the following acids and their dissociation constants: \(\mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2}(O)(I) \leftrightarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HSO}_{3}^{-}(a q) \quad K_{a}=1.2 \times 10^{-2}\) \(H S^{-}(a q)+H_{2}(O)(I) \leftrightarrows H_{3} O^{+}(a q)+S^{2-}(a q) \quad K_{a}=1.3 \times 10^{-19}\) a. Which is the stronger acid, \(\mathrm{H}_{2} \mathrm{SO}_{3} \text { or HS }\)? b. What is the conjugate base of \(\mathrm{H}_{2} \mathrm{SO}_{3}\)? c. Which acid has the weaker conjugate base? d. Which acid has the stronger conjugate base? e. Which acid produces more ions? Equation Transcription: ? ? Text Transcription: H_2 SO_3 (aq) + H_2 (O)(I) left right arrow H_3 O^+ (aq) + HSO_3 ^- (aq) K_a =1.2 times 10^-2 HS^- (aq) + H_2 (O)(I) left right arrow H_3 O^+ (aq) + S^2- (aq) K_a =1.3 times 10^-19 H_2 SO_3 or HS^- H_2 SO_3

Consider the following acids and their dissociation constants: \(\mathrm{HPO}_{4}{ }^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(I) \leftrightarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{PO}_{4}{ }^{3-}(a q) \quad K_{a}=2.2 \times 10^{-13}\) \(\mathrm{HCHO}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \leftrightarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CHO}_{2}^{-}(a q) \quad K_{a}=1.8 \times 10^{-4}\) a. Which is the weaker acid, \(\mathrm{HPO}_{4}{ }^{2-} \text { or } \mathrm{HCHO}_{2}\)? b. What is the conjugate base of \(\mathrm{HPO}_{4}^{2-}\)? c. Which acid has the weaker conjugate base? d. Which acid has the stronger conjugate base? e. Which acid produces more ions? Equation Transcription: ? ? Text Transcription: HPO_4 ^2- (aq) + H_2 O(I) left right arrow H_3 O^+ (aq) + PO_4 ^3- (aq) K_a =2.2 times 10^-13 HCHO_2 (aq) + H_2 O(I) left right arrow H_3 O^+ (aq) + CHO_2 ^- (aq) K_a =1.8 times 10^-4 HPO_4 ^2- or HCHO_2 HPO_4 ^2-

Phosphoric acid dissociates to form hydronium ion and dihydrogen phosphate. Phosphoric acid has a \(K_{a} \text { of } 7.5 \times 10^{-3}\). Write the equation for the reaction and the acid dissociation expression for phosphoric acid. Equation Transcription: Text Transcription: K_a of 7.5 times 10^-3

Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5}-\mathrm{NH}_{2}\), a weak base with a \(K_{b} \text { of } 4.0 \times 10^{-10}\), reacts with water to form \(\mathrm{C}_{6} \mathrm{H}_{5}-\mathrm{NH}_{3}^{+}\) and hydroxide ion. Write the equation for the reaction and the base dissociation expression for aniline. Equation Transcription: Text Transcription: C_6 H_5 - NH_2 K_b of 4.0 times 10^-10 C_6 H_5 - NH_3 ^+

Why are the concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+} \text {and } \mathrm{OH}^{-}\) equal in pure water? Equation Transcription: Text Transcription: H_3 O^+ and OH^-

What is the meaning and value of \(K_{w} \text { at } 25^{\circ} \mathrm{C}\)? Equation Transcription: ° Text Transcription: K_w at 25 degrees celsius

ln an acidic solution, how does the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) compare to the concentration of \(\mathrm{OH}^{-}\)? Equation Transcription: Text Transcription: H_3 O^+ OH^-

If a base is added to pure water, why does the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) decrease? Equation Transcription: Text Transcription: [H_3 O^+ ]

Indicate whether each of the following solutions is acidic, basic, or neutral: a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.0 \times 10^{-5} \mathrm{M}\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.4 \times 10^{-9} \mathrm{M}\) c. \(\left[O H^{-}\right]=8.0 \times 10^{-3} M\) d. \(\left[\mathrm{OH}^{-}\right]=3.5 \times 10^{-10} \mathrm{M}\) Equation Transcription: Text Transcription: [H_3 O^+ ]=2.0 times 10^-5 M [H_3 O^+ ]=1.4 times 10^-9 M [OH^- ]=8.0 times 10^-3 M [OH^- ]=3.5 times 10^-10 M

Indicate whether each of the following solutions is acidic, basic, or neutral: a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=6.0 \times 10^{-12} \mathrm{M}\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.4 \times 10^{-4} \mathrm{M}\) c. \(\left[O H^{-}\right]=5.0 \times 10^{-12} M\) d. \(\left[\mathrm{OH}^{-}\right]=4.5 \times 10^{-2} \mathrm{M}\) Equation Transcription: Text Transcription: [H_3 O^+ ]=6.0 times 10^-12 M [H_3 O^+ ]=1.4 times 10^-4 M [OH^- ]=5.0 times 10^-12 M [OH^- ]=4.5 times 10^-2 M

Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of each aqueous solution with the following \(\left[\mathrm{OH}^{-}\right]\): a. coffee, \(1.0 \times 10^{-9} M\) b. soap, \(1.0 \times 10^{-6} M\) c. cleanser, \(2.0 \times 10^{-5} M\) d. lemon juice, \(4.0 \times 10^{-13} M\) Equation Transcription: Text Transcription: [H_3 O^+ ] [OH^- ] 1.0 times 10^-9 M 1.0 times 10^-5 M 2.0 times 10^-5 M 4.0 times 10^-13 M

Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of each aqueous solution with the following \(\left[\mathrm{OH}^{-}\right]\): a. NaOH solution, \(1.0 \times 10^{-2} M\) b. milk of magnesia, \(1.0 \times 10^{-5} M\) c. aspirin, \(1.8 \times 10^{-11} M\) d. seawater, \(2.5 \times 10^{-6} M\) Equation Transcription: Text Transcription: [H_3 O^+ ] [OH^- ] 1.0 times 10^-2 M 1.0 times 10^-5 M 1.8 times 10^-11 M 2.5 times 10^-6 M

Calculate the \(\left[O H^{-}\right]\) of each aqueous solution with the following \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\): a. stomach acid, \(4.0 \times 10^{-2} M\) b. urine, \(5.0 \times 10^{-6} M\) c. orange juice, \(2.0 \times 10^{-4} M\) d. bile, \(7.9 \times 10^{-19} M\) Equation Transcription: Text Transcription: [OH^- ] [H_3 O^+ ] 4.0 times 10^-2 M 5.0 times 10^-6 M 2.0 times 10^-4 M 7.9 times 10^-9 M

Calculate the \(\left[\mathrm{OH}^{-}\right]\) of each aqueous solution with the following \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\): a. baking soda, \(1.0 \times 10^{-8} M\) b. blood, \(4.2 \times 10^{-8} M\) c. milk, \(5.0 \times 10^{-7} M\) d. pancreatic juice, \(4.0 \times 10^{-9} M\) Equation Transcription: Text Transcription: [OH^- ] [H_3 O^+ ] 1.0 times 10^-8 M 4.2 times 10^-8 M 5.0 times 10^-7 M 4.0 times 10^-9 M

Why does a neutral solution have a \(p H \text { of } 7.0\)? Equation Transcription: Text Transcription: pH of 7.0

If the \(\left[\mathrm{OH}^{-}\right]\) of a solution is greater than the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\), is the solution acidic or basic? Equation Transcription: Text Transcription: [OH^- ] [H_3 O^+ ]

State whether each of the following solutions is acidic, basic, or neutral: a. blood plasma, \(p H\ 7.38\) b. vinegar, \(p H\ 2.8\) c. coffee, \(p H\ 5.52\) d. tomatoes, \(p H\ 4.2\) e. chocolate cake, \(p H\ 7.6\) Equation Transcription: Text Transcription: pH 7.38 pH 2.8 pH 5.52 pH 4.2 pH 7.6

State whether each of the following solutions is acidic, basic, or neutral: a. soda, \(p H\ 3.22\) b. shampoo, \(p H\ 5.7\) c. rain, \(p H\ 5.8\) d. honey, \(p H\ 3.9\) e. cheese, \(p H\ 5.2\) Equation Transcription: Text Transcription: pH 3.22 pH 5.7 pH 5.8 pH 3.9 pH 5.2

A solution with a \(p H \text { of } 3\) is 10 times more acidic than a solution with \(p H\ 4\). Explain. Equation Transcription: Text Transcription: pH of 3 pH 4

A solution with a \(p H \text { of } 10\) is 100 times more basic than a solution with \(p H\ 8\). Explain. Equation Transcription: Text Transcription: pH of 10 pH 8

Calculate the pH of each solution given the following: a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1 \times 10^{-4} \mathrm{M}\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=3 \times 10^{-8} \mathrm{M}\) c. \(\left[\mathrm{OH}^{-}\right]=1 \times 10^{-5} \mathrm{M}\) d. \(\left[\mathrm{OH}^{-}\right]=2.5 \times 10^{-11} \mathrm{M}\) e. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=6.7 \times 10^{-8} \mathrm{M}\) f. \(\left[\mathrm{OH}^{-}\right]=8.2 \times 10^{-4} \mathrm{M}\) Equation Transcription: Text Transcription: [H_3 O^+] = 1x10^-4 M [H_3 O^+]= 3x10^-8 M [OH^-] = 1x10^-5 M [OH^-] = 2.5x10^-11M [H_3 O^+]= 6.7x10^-8 M [OH^-]= 8.2x10^-4 M

Calculate the pH of each solution given the following: a. \(\left[H_{3} O^{+}\right]=1 \times 10^{-8} M\) b. \(\left[H_{3} O^{+}\right]=5 \times 10^{-6} M\) c. \(\left[O H^{-}\right]=1 \times 10^{-2} M\) d. \(\left[\mathrm{OH}^{-}\right]=8.0 \times 10^{-3} M\) e. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=4.7 \times 10^{-2} \mathrm{M}\) f. \(\left[O H^{-}\right]=3.9 \times 10^{-6} M\) Equation Transcription: Text Transcription: [H_3 O^+ ]=1 times 10^-8 M [H_3 O^+ ]=5 times 10^-6 M [OH^- ]=1 times 10^-2 M [OH^- ]=8.0 times 10^-3 M [H_3 O^+ ]=4.7 times 10^-2 M [OH^- ]=3.9 times 10^-6 M

Complete the following table for a selection of foods:

Complete the following table for a selection of foods:

A patient with severe metabolic acidosis has a blood plasma pH of \(p H \text { of } 6.92\). What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of the blood plasma? Equation Transcription: Text Transcription: pH of 6.92 [H_3 O^+ ]

A patient with respiratory alkalosis has a blood plasma \(\text { pH of } 7.58\). What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of the blood plasma? Equation Transcription: Text Transcription: pH of 7.58 [H_3 O^+ ]

Complete and balance the equation for each of the following reactions: a. \(\operatorname{HBr}(a q)+\mathrm{ZnCO}_{3}(s) \rightarrow\) b. \(H C I(a q)+Z n(s) \rightarrow\) c. \(H C I(a q)+N a H C O_{3}(s) \rightarrow\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s}) \rightarrow\) Equation Transcription: Text Transcription: HBr(aq) + ZnCO_3 (s) right arrow HCI(aq) + Zn(s) right arrow HCI(aq) + NaHCO_3 (s) right arrow H_2 SO_4 (aq) + Mg(OH)_2 (s) right arrow

Complete and balance the equation for each of the following reactions: a. \(\mathrm{HBr}(a q)+\mathrm{KHCO}_{3}(s) \rightarrow\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}(\mathrm{s}) \rightarrow\) c. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{~s}) \rightarrow\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(s) \rightarrow\) Equation Transcription: Text Transcription: HBr(aq) + KHCO_3 (s) right arrow H_2 SO_4 (aq) + Ca(s) right arrow H_2 SO_4 (aq) + Ca(OH)_2 (s) right arrow H_2 SO_4 (aq) + Na_2 CO_3 (s) right arrow

Balance each of the following neutralization reactions: a. \(\mathrm{HCI}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{MgCl}_{2}(\mathrm{aq})\) b. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{LiOH}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{Li}_{3} \mathrm{PO}_{4}(a q)\) Equation Transcription: Text Transcription: HCI(aq) + Mg(OH)_2 (s) right arrow H_2 O(I) + MgCl_2 (aq) H_3 PO_4 (aq) + LiOH(aq) right arrow H_2 O(I) + Li_3 PO_4 (aq)

Balance each of the following neutralization reactions: a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(s) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)\) Equation Transcription: Text Transcription: HNO_3 (aq) + Ba(OH)_2 (s) right arrow H_2 O(I) + Ba(NO_3 )_2 (aq) H_2 SO_4 (aq) + Al(OH)_3 (s) right arrow H_2 O(I) + Al_2 (SO_4)_3 (aq)

Write a balanced equation for the neutralization of each of the following: a. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \text { and } \mathrm{NaOH}(a q)\) b. \(H C I(a q) \text { and } F e(O H)_{3}(s)\) c. \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \text { and } \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})\) Equation Transcription: Text Transcription: H_2 SO_4 (aq) and NaOH(aq) HCI(aq) and Fe(OH)_3 (s) H_2 CO_3 (aq) and Mg(OH)_2 (s)

Write a balanced equation for the neutralization of each of the following: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \text { and } \mathrm{NaOH}(a q)\) b. \(\text { HI }(a q) \text { and } L i O H(a q)\) c. \(\mathrm{HNO}_{3}(a q) \text { and } \mathrm{Ca}(\mathrm{OH})_{2}(s)\) Equation Transcription: Text Transcription: H_3 PO_4 (aq) and NaOH(aq) HI(aq) and LiOH(aq) HNO_3 (aq) and Ca(OH)_2 (s)

What is the molarity of a solution of \(\text { HCI if } 5.00 \mathrm{~mL}\) of the \(\mathrm{HCI}\) solution is titrated with \(28.6 \mathrm{~mL}\) of a \(0.145 \mathrm{NaOH}\) solution? \(\mathrm{HCI}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(I)+\mathrm{NaCl}(a q)\) Equation Transcription: Text Transcription: HCI if 5.00 mL HCI 28.6 mL 0.145 NaOH HCI(aq) + NaOH(aq) right arrow H_2 O(I) + NaCl(aq)

What is the molarity of the acetic acid solution if \(29.7 \mathrm{~mL}\) of a \(0.205 M K O H\) solution is required to titrate \(25.0 \mathrm{~mL}\) of a solution of \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)? \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) Equation Transcription: Text Transcription: 29.7 mL 0.205 M KOH 25.0 mL HC_2 H_3 O_2 HC_2 H_3 O_2 (aq) + KOH(aq) right arrow H_2 O(I) + KC_2 H_3 O_2 (aq)

If \(38.2 \mathrm{~mL}\) of a \(0.163 \mathrm{M\ KOH}\) solution is required to titrate \(25.0 \mathrm{~mL}\) of a \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution, what is the molarity of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution? \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{KOH}(a q) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(I)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)\) Equation Transcription: Text Transcription: 38.2 mL 0.163 M KOH 25.0 mL H_2 SO_4 H_2 SO_4 (aq) + 2KOH(aq) right arrow 2H_2 O(I) + K_2 SO_4 (aq)

If \(32.8 m L\) of a \(0.162 \mathrm{\ M\ NaOH}\) solution is required to titrate \(25.0 m L\) of a solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\), what is the molarity of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution? \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaOH}(a q) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) Equation Transcription: Text Transcription: 32.8 mL 0.162 M NaOH 25.0 mL H_2 SO_4 H_2 SO_4 (aq) + 2NaOH (aq) right arrow 2H_2 O(I) + Na_2 SO_4 (aq)

A solution of \(0.204 \mathrm{\ M\ NaOH}\) is used to titrate \(50.0 m L\) of a \(0.0224 \mathrm{\ M\ H}_{3} \mathrm{PO}_{4}\) solution. What volume, in milliliters, of the \(\mathrm{NaOH}\) solution is required? \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{NaOH}(a q) \rightarrow 3 \mathrm{H}_{2} \mathrm{O}(I)+\mathrm{Na}_{3} \mathrm{PO}_{4}(a q)\) Equation Transcription: Text Transcription: 0.204 M NaOH 50.0 mL 0.0224 M H_3 PO_4 NaOH H_3 PO_4 (aq) + 3NaOH(aq) right arrow 3H_2 O(I) + Na_3 PO_4 (aq)

A solution of \(0.312 \mathrm{\ M\ KOH}\) is used to titrate \(15.0 \mathrm{~mL}\) of a \(0.186 \mathrm{\ M\ H}_{3} \mathrm{PO}_{4}\) solution. What volume, in milliliters, of the \(\mathrm{KOH}\) solution is required? \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+3 \mathrm{KOH}(\mathrm{aq}) \rightarrow 3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{K}_{3} \mathrm{PO}_{4}(\mathrm{aq})\) Equation Transcription: Text Transcription: 0.312 M KOH 15.0 mL 0.186 M H_3 PO_4 KOH H_3 PO_4 (aq) + 3KOH(aq) right arrow 3H_2 O(I) + K_3 PO_4 (aq)

Which of the following represents a buffer system? Explain. a. \(\mathrm{NaOH} \text { and } \mathrm{NaCl}\) b. \(\mathrm{H}_{2} \mathrm{CO}_{3} \text { and } \mathrm{NaHCO}_{3}\) c. \(H F \text { and } K F\) d. \(\mathrm{KCI} \text { and } \mathrm{NaCl}\) Equation Transcription: Text Transcription: NaOH and NaCl H_2 CO_3 and NaHCO_3 HF and KF KCI and NaCl

Which of the following represents a buffer system? Explain. a. \(\mathrm{HCIO}_{2}\) b. \(\mathrm{NaNO}_{3}\) c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \text { and } \mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. \(H C I \text { and } N a O H\) Equation Transcription: Text Transcription: HCIO_2 NaNO_3 HC_2 H_3 O_2 and NaC_2 H_3 O_2 HCI and NaOH

Consider the buffer system of hydrofluoric acid, HF, and its salt, NaF. \(H F(a q)+H_{2} O(I) \leftrightarrows H_{3} O^{+}(a q)+F^{-}(a q)\) a. The purpose of this buffer system is to: 1. maintain \([H F]\) 2. maintain \(\left[F^{-}\right]\) 3. maintain \(p H\) b. The salt of the weak acid is needed to: 1. provide the conjugate base 2. neutralize added \(\mathrm{H}_{3} \mathrm{O}^{+}\) 3. provide the conjugate acid c. If \(\mathrm{OH}^{-}\) is added, it is neutralized by: 1. the salt 2. \(\mathrm{H}_{2} \mathrm{O}\) 3. \(\mathrm{H}_{3} \mathrm{O}^{+}\) d. When \(\mathrm{H}_{3} \mathrm{O}^{+}\) is added, the equilibrium shifts in the direction of the: 1. reactants 2. products 3. does not change Equation Transcription: ? Text Transcription: HF(aq) + H_2 O(I) left right arrow H_3 O^+ (aq) + F^- (aq) [HF] [F^-] pH H_3 O^+ OH^- H_2 O H_3 O^+

Consider the buffer system of nitrous acid, \(\mathrm{HNO}_{2}\), and its salt, \(\mathrm{NaNO}_{2}\). \(\mathrm{HNO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \leftrightarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q)\) a. The purpose of this buffer system is to: 1. maintain \(\left[\mathrm{HNO}_{2}\right]\) 2. maintain \(\left[\mathrm{NO}_{2}^{-}\right]\) 3. maintain \(p H\) b. The weak acid is needed to: 1. provide the conjugate base 2. neutralize added \(\mathrm{OH}^{-}\) 3. provide the conjugate acid c. If \(\mathrm{H}_{3} \mathrm{O}^{-}\) is added, it is neutralized by: 1. the salt 2. \(\mathrm{H}_{2} \mathrm{O}\) 3. \(\mathrm{OH}^{-}\) d. When \(\mathrm{OH}^{-}\) is added, the equilibrium shifts in the direction of the: 1. reactants 2. products 3. does not change Equation Transcription: ? Text Transcription: HNO_2 NaNO_2 HNO_2 (aq) + H_2 O(I) left right arrow H_3 O^+ (aq) + NO_2 ^- (aq) NO_2 ^- pH OH^- H_3 O^- H_2 O

Nitrous acid has a \(K_{a} \text { of } 4.5 \times 10^{-4}\). What is the \(p H\) of a buffer solution containing \(0.10 \mathrm{\ M\ HNO}_{2} \text { and } 0.10 \mathrm{\ M\ NO}_{2}^{-}\)? Equation Transcription: Text Transcription: K_a of 4.5 times 10^-4 pH 0.10 M HNO_2 and 0.10 M NO_2 ^-

Acetic acid has a \(K_{a} \text { of } 1.8 \times 10^{-5}\). What is the \(p H\) of a buffer solution containing \(0.15 \mathrm{\ M\ HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \text { and } 0.15 \mathrm{\ M\ C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\)? Equation Transcription: Text Transcription: K_a of 1.8 times 10^-5 pH 0.15 M HC_2 H_3 O_2 and 0.15 M C_2 H_3 O_2 ^-

Using Table 11.4 for \(K_{a}\) values, compare the \(p H\) of a \(H F\) buffer that contains \(0.10 \mathrm{\ M\ HF} \text { and } 0.10 \mathrm{\ M\ NaF}\) with another HF buffer that contains \(0.060 \mathrm{\ M\ HF} \text { and } 0.120 \mathrm{\ M\ NaF}\). Equation Transcription: Text Transcription: K_a pH HF 0.1 0 M HF and 0.10 M NaF 0.060 M HF and 0.120 M NaF

Using Table 11.4 for \(K_{a}\) values, compare the \(p H\) of a \(\mathrm{H}_{2} \mathrm{CO}_{3}\) buffer that contains \(0.10 \mathrm{\ M\ H}_{2} \mathrm{CO}_{3} \text { and } 0.10 \mathrm{\ M\ NaHCO}_{3}\) with another \(\mathrm{H}_{2} \mathrm{CO}_{3}\) buffer that contains \(0.15 \mathrm{\ M\ H}_{2} \mathrm{CO}_{3} \text { and } 0.050 \mathrm{\ M\ NaHCO}_{3}\). Equation Transcription: Text Transcription: K_a pH H_2 CO_3 0.10 M H_2 CO_3 and 0.10 M NaHCO_3 0.15 M H_2 CO_3 and 0.050 M NaHCO_3

Why would the \(p H\) of your blood plasma increase if you breathe fast? Equation Transcription: Text Transcription: pH

Why would the \(p H\) of your blood plasma decrease if you hold your breath? Equation Transcription: Text Transcription: pH

Someone with kidney failure excretes urine with large amounts of \(\mathrm{HCO}_{3}^{-}\). How would this loss of \(\mathrm{HCO}_{3}^{-}\) affect the \(p H\) of the blood plasma? Equation Transcription: Text Transcription: HCO_3 ^- pH

Someone with severe diabetes obtains energy by the breakdown of fats, which produce large amounts of acidic substances. How would this affect the \(p H\) of the blood plasma? Equation Transcription: Text Transcription: pH

At rest, the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of the stomach fluid is \(2.0 \times 10^{-4} M\). What is the \(p H\) of the stomach fluid? Equation Transcription: Text Transcription: [H_3 O^+ ] 2.0 times 10^-4 M pH

When food enters the stomach, \(\text { HCI }\) is released and the \(\left[H_{3} O^{+}\right]\) of the stomach fluid rises to \(4.2 \times 10^{-2} M\). What is the \(p H\) of the stomach fluid while eating? Equation Transcription: Text Transcription: HCI [H_3 O^+ ] 4.2 times 10^-2 M pH

In Larry's esophageal pH test, a \(p H\) value of \(3.60\) was recorded in the esophagus. What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in his esophagus? Equation Transcription: Text Transcription: pH 3.60 [H_3 O^+ ]

After Larry had taken Nexium for 4 weeks, the \(p H\) in his stomach was raised to \(4.52\). What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in his stomach? Equation Transcription: Text Transcription: pH 4.52 [H_3 O^+ ]

Write the balanced chemical equation for the neutralization reaction of stomach acid \(H C I\) with \(\mathrm{CaCO}_{3}\), an ingredient in some antacids. Equation Transcription: Text Transcription: HCI CaCO_3

Write the balanced chemical equation for the neutralization reaction of stomach acid \(H C I\) with \(A l(O H)_{3}\), an ingredient in some antacids. Equation Transcription: Text Transcription: HCI Al(OH)_3

How many grams of \(\mathrm{CaCO}_{3}\) are required to neutralize \(100 \mathrm{~mL}\) of stomach acid \(\mathrm{HCI}\), which is \(0.0400 \mathrm{\ M\ } \mathrm{HCI}\)? Equation Transcription: Text Transcription: CaCO_3 100 mL HCI 0.0400 M HCI

How many grams of \(\mathrm{Al}(\mathrm{OH})_{3}\) are required to neutralize \(150 \mathrm{~mL}\) of stomach acid \(H C I\) with a \(\text { pH of } 1.50\)? Equation Transcription: Text Transcription: Al(OH)_3 150 mL HCI pH of 1.50

Determine if each of the following diagrams represents a strong acid or a weak acid. The acid has the formula \(H X .(11.3)\) Equation Transcription: Text Transcription: HX. (11. 3)

Adding a few drops of a strong acid to water will lower the \(p H\) appreciably. However, adding the same number of drops to a buffer does not appreciably alter the \(p H\). Why? (11.8) Equation Transcription: Text Transcription: pH

Identify each of the following as an acid or a base: (11.1) a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) b. \(\mathrm{RbOH}\) c. \(\mathrm{Ca}(\mathrm{OH})_{2}\) d. \(H I\) Equation Transcription: Text Transcription: H_2 SO_4 RbOH Ca(OH)_2 HI

Identify each of the following as an acid or a base: (11.1) a. \(\mathrm{Sr}(\mathrm{OH})_{2}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{3}\) c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. \(\mathrm{CsOH}\) Equation Transcription: Text Transcription: Sr(OH)_2 H_2 SO_3 HC_2 H_3 O_2 CsOH

Complete the following table: (11.2)

Complete the following table: (11.2)

Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting. (11.8) a. What changes occur in the blood \(p H\) during hyperventilation? b. How does breathing into a paper bag help return blood \(p H\) to normal? Equation Transcription: Text Transcription: pH

In the blood plasma, \(p H\) is maintained by the carbonic acid-bicarbonate buffer system. (11.8) a. How is \(p H\) maintained when acid is added to the buffer system? b. How is \(p H\) maintained when base is added to the buffer system? Equation Transcription: Text Transcription: pH

State whether each of the following solutions is acidic, basic, or neutral: (11.5) a. sweat, \(p H\ 5.2\) b. tears, \(p H\ 7.5\) c. bile, \(p H\ 8.1\) d. stomach acid, \(p H\ 2.5\) Equation Transcription: Text Transcription: pH 5.2 pH 7.5 pH 8.1 pH 2.5

State whether each of the following solutions is acidic, basic, or neutral: (11.5) a. saliva, \(p H\ 6.8\) b. urine, \(p H\ 5.9\) c. pancreatic juice, \(p H\ 8.0\) d. blood, \(p H\ 7.45\) Equation Transcription: Text Transcription: pH 6.8 pH 5.9 pH 8.0 pH 7.45

Identify each of the following as an acid, base, or salt, and give its name: (11.1) a. \(\mathrm{HBrO}_{2}\) b. \(\mathrm{CsOH}\) c. \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) d. \(\mathrm{HCIO}_{4}\) Equation Transcription: Text Transcription: HBrO_2 CsOH Mg(NO_3 )_2 HCIO_4

Identify each of the following as an acid, base, or salt, and give its name: (11.1) a. \(\mathrm{HNO}_{2}\) b. \(M g B r_{2}\) c. \(\mathrm{NH}_{3}\) d. \(\mathrm{Li}_{2} \mathrm{SO}_{3}\) Equation Transcription: Text Transcription: HNO_2 MgBr_2 NH_3 Li_2 SO_3

Complete the following table: (11.2)

Complete the following table: (11.2)

Using Table 11.3, identify the stronger acid in each of the following pairs: (11.3) a. \(\text { HF or HCN }\) b. \(\mathrm{H}_{3} \mathrm{O}^{+} \text {or } \mathrm{H}_{2} \mathrm{~S}\) c. \(\mathrm{HNO}_{2} \text { or } \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. \(\mathrm{H}_{2} \mathrm{O} \text { or } \mathrm{HCO}_{3}^{-}\) Equation Transcription: Text Transcription: HF or HCN H_3 O^+ or H_2 S HNO_2 or HC_2 H_3 O_2 H_2 O or HCO_3 ^-

Using Table 11.3, identify the stronger base in each of the following pairs: (11.3) a. \(\mathrm{H}_{2} \mathrm{O} \text { or } \mathrm{Cl}^{-}\) b. \(\mathrm{OH}^{-} \text {or } \mathrm{NH}_{3}\) c. \(\mathrm{SO}_{4}^{2-} \text { or } \mathrm{NO}_{2}^{-}\) d. \(\mathrm{CO}_{3}{ }^{2-} \text { or } \mathrm{H}_{2} \mathrm{O}\) Equation Transcription: Text Transcription: H_2 O or Cl^- OH^- or NH_3 SO_4 ^2- or NO_2 ^- CO_3 ^2- or H_2 O

Determine the pH for each of the following solutions: (11.6) a. \(\left[H_{3} O^{+}\right]=2.0 \times 10^{-8} M\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=5.0 \times 10^{-2} \mathrm{M}\) c. \(\left[\mathrm{OH}^{-}\right]=3.5 \times 10^{-4} \mathrm{M}\) d. \(\left[O H^{-}\right]=0.0054 M\) Equation Transcription: Text Transcription: [H_3 O^+ ] = 2.0 times 10^-8 M [H_3 O^+ ] = 5.0 times 10^-2 M [OH^- ] = 3.5 times 10^-4 M [OH^- ] = 0.0054 M

Determine the pH for each of the following solutions: (11.6) a. \(\left[O H^{-}\right]=1.0 \times 10^{-7} M\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=4.2 \times 10^{-3} \mathrm{M}\) c. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=0.0001 \mathrm{M}\) d. \(\left[O H^{-}\right]=8.5 \times 10^{-9} \mathrm{M}\) Equation Transcription: Text Transcription: [OH^- ] = 1.0 times 10^-7 M [H_3 O^+ ] = 4.2 times 10^-3 M [H_3 O^+ ] = 0.0001 M [OH^- ] = 8.5 times 10^-9 M

Are the solutions in problem 11.103 acidic, basic, or neutral? (11.6) a. \(\left[H_{3} O^{+}\right]=2.0 \times 10^{-8} M\) b. \(\left[H_{3} O^{+}\right]=5.0 \times 10^{-2} M\) c. \(\left[O H^{-}\right]=3.5 \times 10^{-4} M\) d. \(\left[O H^{-}\right]=0.0054 M\) Equation Transcription: Text Transcription: [H_3 O^+ ] = 2.0 times 10^-8 M [H_2 O^+ ] = 5.0 times 10^-2 M [OH^- ] = 3.5 times 10^-4 M [OH^- ] = 0.0054 M

Are the solutions in problem 11.104 acidic, basic, or neutral? (11.6) a. \(\left[\mathrm{OH}^{-}\right]=1.0 \times 10^{-7} \mathrm{M}\) b. \(\left[H_{3} O^{+}\right]=4.2 \times 10^{-3} M\) c. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=0.0001 \mathrm{M}\) d. \(\left[O H^{-}\right]=8.5 \times 10^{-9} M\) Equation Transcription: Text Transcription: [OH^- ] = 1.0 times 10^-7 M [H_3 O^+ ] = 4.2 times 10^-3 M [H_3 O^+ ] = 0.0001 M [OH^- ] = 8.5 times 10^-9 M

Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right] \text {and }\left[\mathrm{OH}^{-}\right]\) for a solution with each of the following pH values: (11.6) a. \(3.00\) b. \(6.2\) c. \(8.85\) d. \(11.00\) Equation Transcription: Text Transcription: [H_3 O^+ ] and [OH^- ] 3.00 6.2 8.85 11.00

Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right] \text {and }\left[\mathrm{OH}^{-}\right]\) for a solution with each of the following pH values: (11.6) a. \(10.00\) b. \(5.0\) c. \(6.54\) d. \(1.82\) Equation Transcription: Text Transcription: [H_3 O^+ ] and [OH^- ] 10.00 5.0 6.54 1.82

Solution \(A\) has a \(pH\) of \(4.5\), and solution \(B\) has a \(pH\) of \(6.7\). \((11.6)\) a . Which solution is more acidic? b. What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in each? c. What is the \(\left[\mathrm{OH}^{=}\right]\) in each? Equation Transcription: Text Transcription:

Solution \(X\) has a \(\mathrm{pH}\) of \(9.5\), and solution \(Y\) has a \(\mathrm{pH}\) of \(7.5\). \((11.6)\) a. Which solution is more acidic? b. What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in each? c. What is the \(\left[\mathrm{OH}^{-}\right]\) in each? Equation Transcription: X pH 9.5 Y 7.5 (11.6) Text Transcription: X pH 9.5 Y 7.5 (11.6) [H_3 O^+] [OH^-]

What is the \(\left[\mathrm{OH}^{-}\right]\) in a solution that contains \(0.225 \ g\) of \(\mathrm{NaOH}\) in \(0.250 \ L\) of solution? \((11.7)\) Equation Transcription: 0.225 g NaOH 0.250 L (11.7) Text Transcription: [OH^-] 0.225 g NaOH 0.250 L (11.7)

What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a solution that contains \(1.54 \ g\) of \(\mathrm{HNO}_{3}\) in \(0.500 \ L\) of solution? \((11.7)\) Equation Transcription: 1.54 g 0.500 L (11.7) Text Transcription: [H_3 O^+] 1.54 g HNO_3 0.500 L (11.7)

What is the \(\mathrm{pH}\) of a solution prepared by dissolving \(2.5 \ g\) of \(\mathrm{HCI}\) in water to make \(425 \ mL\) of solution? \((11.6)\) Equation Transcription: pH 2.5 g HCI 425 mL (11.6) Text Transcription: pH 2.5 g HCI 425 mL (11.6)

What is the \(\mathrm{pH}\) of a solution prepared by dissolving \(1.0 \ g\) of \(\mathrm{Ca(OH)}_{2}\) in water to make \(875 \ mL\) of solution? \((11.6)\) Equation Transcription: pH 1.0 g 875 mL (11.6) Text Transcription: pH 1.0 g ca(OH)_2 875 mL (11.6)

For each of the following: \((11.2, 11.3)\) 1. \(\mathrm{H}_{2} \mathrm{S}\) 2. \(\mathrm{H}_{3} \mathrm{PO}_{4}\) a. Write the formula for the conjugate base. b. Write the \(K_{\mathrm{a}}\) expression. c. Which is the weaker acid? Equation Transcription: (11.2, 11.3) Text Transcription: (11.2, 11.3) H_2 S H_3 PO_4 K_a

For each of the following: \((11.2, 11.3)\) 1. \(\mathrm{HCO}_{3}^{-}\) 2. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) a. Write the formula for the conjugate base. b. Write the \(K_{\mathrm{a}}\) expression. c. Which is the stronger acid? Equation Transcription: (11.2, 11.3) Text Transcription: (11.2, 11.3) HCO_3 ^- HC_2 H_3 O_2 K_a

Using Table \(11.3\), identify the conjugate acid-base pairs in each of the following equations and whether the equilibrium mixture contains mostly products or mostly reactants: \((11.2 , 11.3)\) a. \(\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{HNO}_{3}(\mathrm{aq}) \leftrightarrows \mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})\) b. \(\mathrm{HBr}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \leftrightarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})\) Equation Transcription: Text Transcription: 11.3 11.12, 11.13 NH_3(aq) + HNO_3(aq) left right arrows NH_4 ^+ (aq) + NO_3 ^- (aq) HBr(aq) + H_2O(l) left right arrows H_3 O^+ (aq) + Br ^- (aq)

Using Table \(11.3\), identify the conjugate acid-base pairs in each of the following equations and whether the equilibrium mixture contains mostly products or mostly reactants: \((11.2, 11.3)\) a. \(\mathrm{HNO}_{2}(\mathrm{aq})+\mathrm{HS}(\mathrm{aq}) \leftrightarrows \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})+\mathrm{NO}_{2}^{-}(\mathrm{aq})\) b. \(\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \leftrightarrows \mathrm{OH}^{-}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq})\) Equation Transcription: Text Transcription: 11.3 (11.2, 11.3) HNO_2 (aq) + HS^- (aq) left right arrow H_2 S(g) + NO_2 ^- (aq) Cl^- (aq) + H_2O(l) left right arrow OH^- (aq) + HCI(aq)

Complete and balance each of the following: \((11.7)\) a. \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{ZnCO}_{3}(\mathrm{~s}) \rightarrow\) b. \(\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{Al}(\mathrm{s}) \rightarrow\) Equation Transcription: Text Transcription: 11.7 H_2 SO_4 (aq) + ZnCO_3 (s) right arrow HNO_3 (aq) + AI(s) right arrow

Complete and balance each of the following: \((11.7)\) a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{~s}) \rightarrow\) b. \(\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{KHCO}_{3}(\mathrm{~s}) \rightarrow\) Equation Transcription: Text Transcription: 11.7 H_3 PO_4(aq) + Ca(OH)_2 (s) right arrow HNO_3 (aq) + KHCO_3 (s) right arrow

Determine each of the following for a \(0.050 M KOH\) solution: \((11.6, 11.7)\) a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) b. \(pH\) c. the balanced equation for the reaction with \(\mathrm{H}_{2} \mathrm{SO}_{4}\) d. milliliters of \(KOH\) solution required to neutralize \(40.0 mL\) of a \(0.035 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution Equation Transcription: Text Transcription: 0.050 M KOH (11.6, 11.7) [H_3 O^+] pH H_2 SO_4 KOH 40.0 mL 0.035 M H_2 SO_4

Determine each of the following for a \(0.10 M HBr\) solution: \((11.6, 11.7)\) a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) b. \(pH\) c. the balanced equation for the reaction with \(LiOH\) d. milliliters of \(HBr\) solution required to neutralize \(36.0 mL\) of a \(0.25 M LiOH\) solution Equation Transcription: Text Transcription: 0.10 M HBr (11.6, 11.7) [H_3 O^+] pH LiOH HBr 36.0 mL 0.25 M LiOH

Calculate the volume, in milliliters, of a \(0.150 M NaOH\) solution that will completely neutralize each of the following: \((11.7)\) a. \(25.0 mL\) of a \(0.288 M HCI\) solution b. \(10.0 mL\) of a \(0.560 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution Equation Transcription: Text Transcription: 0.150 M NaOH (11.7) 25.0 mL 0.288 M HCI 10.0 mL 0.560 M H_2 SO_4

Calculate the volume, in milliliters, of a \(0.215 M NaOH\) solution that will completely neutralize each of the following: \((11.7)\) a. \(3.80 mL\) of a \(1.25 \mathrm{M} \mathrm{HNO}_{3}\) solution b. \(8.50 mL\) of a \(0.825 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) solution Equation Transcription: Text Transcription: 0.215 M NaOH (11.7) 3.80 mL 1.25 M HNO_3 8.50 mL 0.825 M H_3 PO_4

A solution of \(0.205 M NaOH\) is used to titrate \(20.0 mL\) of a \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution. If \(45.6 mL\) of the \(NaOH\) solution is required to reach the endpoint, what is the molarity of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution? \((11.7)\) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{NaOH}(\mathrm{aq}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})\) Equation Transcription: Text Transcription: 0.205 M NaOH 20.0 mL H_2 SO_4 45.6 mL NaOH (11.7) H_2 SO_4(aq) + 2NaOH(aq) right arrow 2H_2 O(I) + Na_2 SO_4(aq)

A \(10.0-mL\) sample of vinegar, which is an aqueous solution of acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), requires \(16.5 mL\) of a \(0.500 M NaOH\) solution to reach the endpoint in a titration. What is the molarity of the acetic acid solution? \((11.7)\) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) Equation Transcription: Text Transcription: 10.0-mL HC_2 H_3 O_2 16.5 mL 0.500 M NaOH (11.7) HC_2 H_3 O_2(aq) + NaOH(aq) right arrow H_2 O(l) + NaC_2 H_3 O_2(aq)

A buffer solution is made by dissolving \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{NaH}_{2} \mathrm{PO}_{4}\) in water. \((11.8)\) a. Write an equation that shows how this buffer neutralizes added acid. b. Write an equation that shows how this buffer neutralizes added base. c. Calculate the pH of this buffer if it contains \(0.50 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) and \(0.20 \mathrm{M} \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\). The \(\mathrm{K}_{\mathrm{a}}\) for \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is \(7.5 \times 10^{-3}\). Equation Transcription: Text Transcription: H_3 PO_4 NaH_2 PO_4 (11.8) 0.50 M H_3 PO_4 0.20 M H_2 PO_4 ^- K_a 7.5 times 10^-3

A buffer solution is made by dissolving \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and \(\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) in water. \((11.8)\) a. Write an equation that shows how this buffer neutralizes added acid. b. Write an equation that shows how this buffer neutralizes added base. c. Calculate the \(pH\) of this buffer if it contains \(0.20 \mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and \(0.40 \mathrm{M} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\). The \(\mathrm{K}_{\mathrm{a}}\) for \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) is \(1.8 \times 10^{-5}\). Equation Transcription: Text Transcription: HC_2 H_3 O_2 NaC_2 H_3 O_2 (11.8) pH 0.20 M HC_2 H_3 O_2 0.40 M C_2 H_3 O_2 ^- K_a 1.8 times 10^-5

One of the most acidic lakes in the United States is Little Echo Pond in the Adirondacks in New York. Recently, this lake had a \(pH\) of \(4.2\), well below the recommended \(pH\) of \(6.5\). \((11.6, 11.7)\) a. What are the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) of Little Echo Pond? b. What are the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) of a lake that has a \(pH\) of \(6.5\)? c. One way to raise the pH of an acidic lake (and restore aquatic life) is to add limestone \(\left(\mathrm{CaCO}_{3}\right)\). How many grams of \(\mathrm{CaCO}_{3}\) are needed to neutralize \(1.0 kL\) of the acidic water from the lake if the acid is sulfuric acid? \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}\mathrm{O}(\mathrm{I})+\mathrm{CaSO}_{4}(\mathrm{aq})\) Equation Transcription: Text Transcription: pH 4.2 6.5 (11.6, 11.7) [H_3 O^+] [OH^-] (CaCO_3) 1.0 kL H_2 SO_4(aq) + CaCO_3(s) right arrow CO_2(g) + H_2O(I) + CaSO_4(aq)

The daily output of stomach acid (gastric juice) is \(1000 mL\) to \(2000 mL\). Prior to a meal, stomach acid \((HCI)\) typically has a \(pH\) of \(1.42\). \((11.6, 11.7)\) a. What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of the stomach acid? b. One chewable tablet of the antacid Maalox contains \(600. Mg\) of \(\mathrm{CaCO}_{3}\). Write the neutralization equation, and calculate the milliliters of stomach acid neutralized by two tablets of Maalox. c. The antacid milk of magnesia contains \(400. mg\) of \(\mathrm{Mg}(\mathrm{OH})_{2}\) per teaspoon. Write the neutralization equation, and calculate the number of milliliters of stomach acid that are neutralized by \(1\) tablespoon of milk of magnesia \(\text { (1 tablespoon = } 3 \text { teaspoons) }\). Equation Transcription: Text Transcription: 1000 mL 2000 mL HCI pH 1.42 (11.6, 11.7) [H3O^+] 600 Mg CaCO_3 400 mg Mg(OH)_2 1 1 tablespoon=3 teaspoons