A strong acid has a weak bond to its acidic proton,

The molecular scene depicts the relative concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+}\) (purple) and \(\mathrm{OH}^{-}\) (green) in an aqueous solution at \(25^{\circ} \mathrm{C}\). (Counter ions and solvent molecules are omitted for clarity.) (a) Calculate the pH. (b) How many \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions would you have to draw for every \(\mathrm{OH}^{-}\) ion to depict a solution of pH 4? Equation Transcription: H3O+ OH- 25°C Text Transcription: H_3O^+ OH^- 25°C

Problem 114P Polymers are not very soluble in water, but their solubility increases if they have charged groups. (a) Casein, a milk protein, contains many —COO– groups on its side chains. How does the solubility of casein vary with pH? ________________ (b) Histones are proteins essential to the function of DNA. They are weakly basic due to the presence of side chains with —NH2 and =NH groups. How does the solubility of a histone vary with pH?

Problem 118P A site in Pennsylvania receives a total annual deposition of 2.688 g/m2 of sulfate from fertilizer and acid rain. The ratio by mass of ammonium sulfate/ammonium bisulfate/sulfuric acid is 3.0/5.5/1.0. (a) How much acid, expressed as kg of sulfuric acid, is deposited over an area of 10. km2? (b) How many pounds of CaCO3 are needed to neutralize this acid? (c) If 10. km2 is the area of an unpolluted lake 3 m deep and there is no loss of acid, what pH would be attained in the year? (Assume constant volume.)

Problem 115P Hemoglobin (Hb) transports oxygen in the blood: HbH+(aq)+O2(aq)+H2O(l)?HbO2(aq)+H3O+(aq) In blood, [H3O+] is held nearly constant at 4×10-8M. (a) How does the equilibrium position change in the lungs? ________________ (b) How does it change in O2-delicient cells? ________________ (c) Excessive vomiting may lead to metabolic alkalosis, in which [H3O+] in blood decreases. How does this condition affect the ability of Hb to transport O2? ________________ (d) Diabetes mellitus may lead to metabolic acidosis, in which [H3O+] in blood increases. How does this condition affect the ability of Hb to transport O2?

Problem 5P Which of the following are Arrhenius acids? (a) H2O ________________ (b) Ca(OH)2 ________________ (c) H3PO3 ________________ (d) HI

Problem 1P What is the role of water in the Arrhenius acid-base definition?

Problem 8P Write the Ka expression for each of the following in water: (a)H2PO4- ________________ (b) H3PO2 ________________ (c) HSO4-

Problem 4P What do “strong” and “weak” mean for acids and bases?Ka values of weak acids vary over more than 10 orders of magnitude. What do the acids have in common that makes them “weak”?

Problem 9P Use Appendix C to rank the following in order of increasing acid strength: HIO3, HI, CH3COOH, HF.

Problem 10P Use Appendix C to rank the following in order of decreasing acid strength: HClO, HCl, HCN, HNO2.

Problem 7P Write the Ka expression for each of the following in water: (a) HNO2 ________________ (b) CH3COOH ________________ (c) HBrO2

Problem 11P Classify each as a strong or weak acid or base: (a) H3AsO4 ________________ (b) Sr(OH)2 ________________ (c) HIO ________________ (d) HClO4

Problem 13P What is an autoionization reaction? Write equations for the autoionization reactions of H2O and of H2SO4.

Problem 17P (a) What is the pH of 0.0333 M HNO3? Is the solution neutral, acidic, or basic? (b) What is the pOH of 0.0347 M KOH? Is the solution neutral, acidic, or basic?

Problem 14P (a) What is the change in pH when [OH-] increases by a factor of 10? (b) What is the change in [H3O+] when the pH decreases by 3 units?

Problem 15P Which solution has the higher pH? Explain. (a) A 0.1M solution of an acid with Ka = 1×10-4 or one with Ka = 4×10 -5 ________________ (b) A 0.1M solution of an acid with pKa = 3.0 or one with pKa = 3.5 ________________ (c) A 0.1 M solution or a 0.01M solution of a weak acid ________________ (d) A 0.1 M solution of a weak acid or a 0.1M solution of a strong acid ________________ (e) A 0.1 M solution of an acid or a 0.01 M solution of a base ________________ (f) A solution of pOH 6.0 or one of pOH 8.0

Problem 12P Classify each as a strong or weak acid or base: (a) CH3NH2 ________________ (b) K2O ________________ (c) HI ________________ (d) HCOOH

Problem 16P (a) What is the pH of 0.0111 M NaOH? Is the solution neutral, acidic, or basic? ________________ (b) What is the pOH of 1.35 × 10 -3M HCl? Is the solution neutral, acidic, or basic?

Problem 18P (a) What are [H3O+], [OH?], and pOH in a solution with a pH of 9.85? (b) What are [H3O+], [OH?], and pH in a solution with a pOH of 9.43?

Problem 19P (a) What are [H3O+], [OH?], and pOH in a solution with a pH of 4.77? (b) What are [H3O+], [OH?], and pH in a solution with a pOH of 5.65?

Problem 20P How many moles of H3O+ or OH ? must you add to 5.6 L of HA solution to adjust its pH from 4.52 to 5.25? Assume a negligible volume change.

Problem 21P How many moles of H3O+ or OH ? must you add to 87.5 mL of HA solution to adjust its pH from 8.92 to 6.33? Assume a negligible volume change.

Problem 25P How are the Arrhenius and Brønsted-Lowry acid-base definitions different? How are they similar? Name two Bronsted- Lowry bases that are not Arrhenius bases. Can you do the same for acids? Explain.

Problem 26P What is a conjugate acid-base pair? What is the relationship between the two members of the pair?

The two molecular scenes below depict the relative concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+}\) (purple) in solutions of the same volume (with counter ions and solvent molecules omitted for clarity). If the pH in scene A is 4.8, what is the pH in scene B? Equation Transcription: H3O+ Text Transcription: H_3O^+

Problem 29P What is an amphiprotic species? Name one and write balanced equations that show why it is amphiprotic.

Problem 24P Like any equilibrium constant,Kw changes with temperature. (a) Given that autoionization is endothermic, how does Kw change with rising T? Explain with a reaction that includes heat as reactant or product, (b) In many medical applications, the value of Kw at 37°C (body temperature) may be more appropriate than the value at 25°C, 1.0×10-14. The pH of pure water at 37°C is 6.80. Calculate Kw, pOH, and [OH?] at this temperature.

Problem 32P Give the formula of the conjugate acid: (a) NH3 (b) NH2- (c) nicotine, C10H14N2

Problem 30P Give the formula of the conjugate base: (a) HCl ________________ (b) H2CO3 ________________ (c) H2O

Problem 31P Give the formula of the conjugate base: (a) HPO42 - ________________ (b) NH4+ ________________ (c) HS-

Write balanced net ionic equations for the following reactions, and label the conjugate acid-base pairs: (a) \(\mathrm{HNO}_{3}(a q)+\mathrm{Li}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{LiNO}_{3}(a q)+\mathrm{LiHCO}_{3}(a q)\) (b) \(2 \mathrm{NH}_{4} \mathrm{Cl}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{BaCl}_{2}(a q)+2 \mathrm{NH}_{3}(a q)\) Equation Transcription: Text Transcription: HNO_3(aq) + Li_2CO_3(aq) ? LiNO_3(aq) + LiHCO_3(aq) 2NH_4Cl(aq) + Ba(OH)_2(aq) ? 2H_2O(l) + BaCl_2(aq) + 2NH_3(aq)

Problem 38P The following aqueous species constitute two conjugate acid-base pairs. Use them to write one acid-base reaction with Kc > 1 and another with Kc< 1: HS-, Cl-, HCl, H2S.

Problem 33P Give the formula of the conjugate acid: (a) O2- ________________ (b) SO42- ________________ (c) H20

In each equation, label the acids, bases, and conjugate acid-base pairs: (a) \(\mathrm{NH}_{3}+\mathrm{H}_{3} \mathrm{PO}_{4} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (b) \(\mathrm{CH}_{3} \mathrm{O}^{-}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}+\mathrm{NH}_{2}^{-}\) (c) \(\mathrm{HPO}_{4}{ }^{2-}+\mathrm{HSO}_{4} \rightleftharpoons \mathrm{H}_{2} \mathrm{PO}_{4}{ }^{-}+\mathrm{SO}_{4}{ }^{2-}\) Equation Transcription: Text Transcription: NH_3 + H_3PO_4 ? NH_4+ + H_2PO_4? CH_3O ? + NH_3 ? CH_3OH + NH_2? HPO_4^2? + HSO_4 ? H_2PO_4? + SO_4^2 ?

Problem 42P In each of the following cases, is the concentration of acid before and after dissociation nearly the same or very different? Explain your reasoning: (a) a concentrated solution of a strong acid; (b) a concentrated solution of a weak acid; (c) a dilute solution of a weak acid; (d) a dilute solution of a strong acid.

Problem 39P The following aqueous species constitute two conjugate acid-base pairs. Use them to write one acid-base reaction with Kc > 1 and another with Kc< 1: NO3–,, F–, HF, HNO3.

Use Figure 18.9 to determine whether \(\mathrm{Kc}>1\) for (a) \(\mathrm{HCl}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{NH}_{4}{ }^{+}+\mathrm{Cl}^{-}\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{3}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{HSO}_{3}-+\mathrm{NH}_{4}^{+}\) Equation Transcription: Kc > 1 HCl + NH3 ? NH4+ + Cl ? H2SO3 + NH3 ? HSO3 ? + NH4+ Text Transcription: K_c > 1 HCl + NH_3 ? NH_4^+ + Cl ? H_2SO_3 + NH_3 ? HSO_3 ? + NH_4^+

Write balanced net ionic equations for the following reactions, and label the conjugate acid-base pairs: (a) \(\mathrm{NaOH}(a q)+\mathrm{NaH}_{2} \mathrm{PO}_{4}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Na}_{2} \mathrm{HPO}_{4}(a q)\) (b) \(\mathrm{KHSO}_{4}(a q)+\mathrm{K}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{KHCO}_{3}(a q)\) Equation Transcription: Text Transcription: NaOH(aq) + NaH_2PO_4(aq) ? H_2O(l) + Na_2HPO_4(aq) KHSO_4(aq) + K_2CO_3(aq) ? K_2SO_4(aq) + KHCO_3(aq)

Use Figure 18.9 to determine whether \(K_{c}<1\) for (a) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{F}^{-} \rightleftharpoons \mathrm{HPO}_{4}^{2}-+\mathrm{HF}\) (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{HSO}_{4}^{-} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+\mathrm{SO}_{4}^{2-} \text {. }\) Equation Transcription: Kc < 1 . Text Transcription: K_c < 1 H_2PO_4? + F ? ? HPO_4^2 ? + HF CH_3COO ? + HSO_4? ? CH_3COOH + SO_4^2 ?.

Problem 43P In which of the following solutions will [H3O+] be approximately equal to [CH3COO–]: (a) 0.1M CH3COOH; ________________ (b) 1×10-7M CH3COOH; ________________ (c) a solution containing both 0.1M CH3COOH and 0.1M CH3COONa? Explain.

Problem 44P Why do successive Ka's decrease for all polyprotic acids?

Problem 45P A 0.15 M solution of butanoic acid, CH3CH2CH2COOH, contains 1.51×10-3M H3O+. What is the Ka of butanoic acid?

Problem 46P A 0.035 M solution of a weak acid (HA) has a pH of 4.88. What is the Ka of the acid?

Problem 48P Hydrofluoric acid, HF, has a Ka of 6.8×10?4. What are [H3O+], [F?], and [OH?] in 0.75 M HF?

Nitrous acid, HNO2, has a Ka of 7 x 104. What are [H3O?], [NO2], and [OH?] in 0.60 M HNO2?

Problem 49P Chloroacetic acid, ClCH2COOH, has a pKa of 2.87. What are [H3O+], pH, [ClCH2COO?], and [ClCH2COOH] in 1.25 M ClCH2COOH?

Problem 50P Hypochlorous acid, HClO, has a p Ka, of 7.54. What are [H3O+], pH, [ClO?], and [HClO] in 0.115M HClO?

Problem 51P In a 0.20 M solution, a weak acid is 3.0% dissociated. (a) Calculate the [H3O+], pH, [OH?], and pOH of the solution. ________________ (b) Calculate Ka of the acid.

Problem 57P What is the key structural feature of all Bronsted-Lowry bases? How does this feature function in an acid-base reaction?

Problem 53P The weak acid HZ has a Ka of 2.55 × 10-4. Calculate the pH of 0.075M HZ. Calculate the pOH of 0.045 M HZ.

Problem 52P In a 0.735M solution, a weak acid is 12.5% dissociated. (a) Calculate the [H3O+], pH, [OH?], and pOH of the solution. ________________ (b) Calculate Kaof the acid.

Problem 55P Acetylsalicylic acid (aspirin), HC9H7O4, is the most widely used pain reliever and fever reducer. Find the pH of 0.018 M aqueous aspirin at body temperature (Ka at 37°C = 3.6 × 10-4).

Problem 58P Why are most anions basic in H2O? Give formulas of four anions that are not basic.

Problem 54P The weak acid HQ has a p Ka, of 4.89. (a) Calculate the [H3O+] of 3.5× 10-2M HQ. (b) Calculate the [OH?] of 0.65M HQ.

Problem 60P Write balanced equations and Kb expressions for these Bronsted-Lowry bases in water: (a) Pyridine, C5H5N ________________ (b) CO32-

Problem 63P What is the pH of 0.12 M diethylamine?

Problem 64P (a) What is the pKb of ClO2-? ________________ (b) What is the pKa of the dimethylammonium ion, (CH3)2NH2+?

Problem 61P Write balanced equations and Kb expressions for these Brønsted-Lowry bases in water: (a) Benzoate ion, C6H5COO? ________________ (b) (CH3)3N

Problem 62P what is the pH of 0.070M dimethylamine?

Problem 59P Except for the Na+ spectator ion, aqueous solutions of CH3COOH and CH3COONa contain the same species. (a) What are the species (other than H2O)? (b) Why is 0.1M CH3COOH acidic and 0.1M CH3COONa basic?

Problem 65P (a) What is the p Kbof NO2-? ________________ (b) What is the p Ka of the hydrazinium ion, H2N—NH3+(Kb of hydrazine = 8.5×10-7)?

Problem 70P Across a period, how does the electronegativity of a nonmetal affect the acidity of its binary hydride?

Sodium hypochlorite solution, sold as "chlorine bleach," is potentially dangerous because of the basicity of ClO, the active bleaching ingredient. What is [OH?] in an aqueous solution that is 6.5% NaClO by mass? What is the pH of the solution? (Assume d of solution = 1.0g/mL.

Problem 67P (a) What is the pH of 0.100 M sodium phenolate, C6H5ONa, the sodium salt of phenol? ________________ (b) What is the pH of 0.15M methyl ammonium bromide, CH3NH3Br (Kb of CH3NH2 = 4.4 × 10-4)?

Codeine (C18H21NO3) is a narcotic pain reliever that forms a salt with HCl. What is the pH of 0.050 M codeine hydrochloride (pKb of codeine = 5.80)?

Problem 66P (a) What is the pH of 0.150 M KCN? ________________ (b) What is the pH of 0.40 M triethylammonium chloride, (CH3CH2)3NHCl?

Problem 72P A strong acid has a weak bond to its acidic proton, whereas a weak acid has a strong bond to its acidic proton. Explain.

Problem 71P How does the atomic size of a nonmetal affect the acidity of its binary hydride?

Problem 75P Choose the weaker acid in each of the following pairs: (a) HI or HBr ________________ (b) H3AsO4 or H2SeO4 ________________ (c) HNO3 or HNO2

Problem 74P Choose the stronger acid in each of the following pairs: (a) H2Se or H3As ________________ (b) B(OH)3 or Al(OH)3 ________________ (c) HBrO2 or HBrO

Problem 73P Perchloric acid, HClO4, is the strongest of the halogen oxoacids, and hypoiodous acid, HIO, is the weakest. What two factors govern this difference in acid strength?

Problem 76P Use Appendix C to choose the solution with the lower pH: (a)0.5 M CuSO4 or 0.25 M Al2(SO4)3 ________________ (b)0.3 M ZnCl2 or 0.3 M PbCl2

Problem 79P Why is aqueous NaF basic but aqueous NaCl neutral?

Problem 77P Use Appendix C to choose the solution with the higher pH: (a)0.1M NiCl2 or 0.1 M NaCl ________________ (b) 0.1M Sn(NO3)2 or 0.1M Co(NO3)2

Problem 78P What determines whether an aqueous solution of a salt will be acidic, basic, or neutral? Give an example of each type of salt.

Problem 81P Explain with equations and calculations, when necessary, whether an aqueous solution of each of these salts is acidic, basic, or neutral: (a) KBr; (b)NH4I; (c) KCN.

Problem 82P Explain with equations and calculations, when necessary, whether an aqueous solution of each of these salts is acidic, basic, or neutral: (a) Cr(NO3)3; (b) NaHS; (c) Zn(CH3COO)2.

Problem 80P The NH4+ ion forms acidic solutions, and the CH3COO? ion forms basic solutions. However, a solution of ammonium acetate is almost neutral. Do all of the ammonium salts of weak acids form neutral solutions? Explain your answer.

Problem 83P Rank the following salts in order of increasing pH of their 0.1M aqueous solutions: (a) KNO3, K2SO3, K2S, Fe(NO3)2 (b) NH4NO3, NaHSO4, NaHCO3, Na2CO3

Problem 85P What feature must a molecule or ion have for it to act as a Lewis base? A Lewis acid? Explain the roles of these features.

(a) Is a weak Brønsted-Lowry base necessarily a weak Lewis base? Explain with an example. (b) Identify the Lewis bases in the following reaction: \(\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}{ }^{2+}(a q)+4 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Cu}(\mathrm{CN})_{4}{ }^{2-}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l)\) (c) Given that \(K_{c}>1\) for the reaction in part (b), which Lewis base is stronger? Equation Transcription: Kc > 1 Text Transcription: Cu(H_2O)_4^2+(aq) + 4CN ? (aq) ? Cu(CN)_4^2-(aq) + 4H_2O(l) Kc > 1

Problem 86P How do Lewis acids differ from Bronsted-Lowry acids? How are they similar? Do Lewis bases differ from Bronsted- Lowry bases? Explain.

Problem 88P In which of the three acid-base concepts can water be a product of an acid-base reaction? In which is it the only product?

Problem 89P (a) Give an example of a substance that is a base in two of the three acid-base definitions, but not in the third. ________________ (b) Give an example of a substance that is an acid in one of the three acid-base definitions, but not in the other two.

Problem 90P Which are Lewis acids and which are Lewis bases? (a) Cu2+ (b)Cl? (c) SnCl2 (d) OF2

Identify the Lewis acid and Lewis base in each equation: (a) \(\mathrm{Na}^{+}+6 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Na}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{+}\) (b) \(\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}\) (c) \(F^{-}+B F_{3} \rightleftharpoons B F_{4}^{-}\) Equation Transcription: Text Transcription: Na^+ + 6H_2O ? Na(H_2O)_6^+ CO_2 + H_2O ? H_2CO_3 F ? + BF_3 ? BF_4?

Problem 96P In humans, blood pH is maintained within a narrow range: acidosis occurs if the blood pH is below 7.35, and alkalosis occurs if the pH is above 7.45. Given that the pKw of blood is 13.63 at 37°C (body temperature), what is the normal range of [H3O+] and of [OH?] in blood?

Classify the following as Arrhenius, Brønsted-Lowry, or Lewis acid-base reactions. A reaction may fit all, two, one, or none of the categories: (a) \(\mathrm{Ag}^{+}+2 \mathrm{NH}_{3} \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{HSO}_{4}^{-}+\mathrm{NH}_{4}^{+}\) (c) \(2 \mathrm{HCl} \rightleftharpoons \mathrm{H}_{2}+\mathrm{Cl}_{2}\) (d) \(\mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \rightleftharpoons \mathrm{AlCl}_{4}^{-}\) Equation Transcription: Text Transcription: Ag^+ + 2NH_3 ? Ag(NH_3)_2^+ H_2SO_4 + NH_3 ? HSO_4? + NH_4^+ 2HCl ? H_2 + Cl_2 AlCl_3 + Cl ? ? AlCl_4?

Identify the Lewis acid and Lewis base in each equation: (a) \(\mathrm{Fe}^{3+}+2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{FeOH}^{2+}+\mathrm{H}_{3} \mathrm{O}^{+}\) (b) \(\mathrm{H}_{2} \mathrm{O}+\mathrm{H}^{-} \rightleftharpoons \mathrm{OH}^{-}+\mathrm{H}_{2}\) (c) \(4 C O+N i \rightleftharpoons N i(C O)_{4}\) Equation Transcription: Text Transcription: Fe^3 + + 2H_2O ? FeOH^2 + + H_3O ^+ H_2O + H ? ? OH ? + H_2 4CO + Ni ? Ni(CO)_4

When carbon dioxide dissolves in water, it undergoes a multistep equilibrium process, with \(K_{\text {overal }} 4.5 \times 10^{-7}\), which is simplified to the following: \(\begin{array}{l} \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \\ \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \end{array} \) (a) Classify each step as a Lewis or a Brønsted-Lowry reaction. (b) What is the pH of nonpolluted rainwater in equilibrium with clean air ( \(\mathrm{P}_{\mathrm{CO} 2}\) in clean air \(3.2 \times 10^{-4} \mathrm{~atm}\); Henry’s law constant for \(\mathrm{CO}_{2}\) at \(25^{\circ} \mathrm{C}\) is 0.033 mol/Latm)? (c) What is \(\left[\mathrm{CO}_{3}{ }^{2-}\right]\) in rainwater (\(\mathrm{K}_{\mathrm{a}} \text { of } \mathrm{HCO}_{3}{ }^{-}=4.7 \times 10^{-11}\))? (d) If the partial pressure of \(\mathrm{CO}_{2}\) in clean air doubles in the next few decades, what will the pH of rainwater become? Equation Transcription: Koverall 4.5x10-7 PCO2 3.2x10-4 atm CO2 25°C \(0.033 \mathrm{~mol} / \mathrm{L} \cdot \mathrm{atm}\) [CO32 ? ] Ka of HCO3? = 4.7x10-11 CO2 Text Transcription: K_overall 4.5x10^-7 CO_2(g) + H_2O(l) ? H_2CO_3(aq) H_2CO_3(aq) + H_2O(l) ? HCO_3? (aq) +H_3O + (aq) P_CO2 3.2x10^-4 atm CO_2 25°C 0.033 mol/L times atm [CO_3^2 ? ] K_a of HCO_3? = 4.7x10^-11 CO_2

Classify the following as Arrhenius, Brønsted-Lowry, or Lewis acid-base reactions. A reaction may fit all, two, one, or none of the categories: (a) \(\mathrm{Cu}^{2+}+4 \mathrm{Cl}^{-} \rightleftharpoons \mathrm{CuCl}_{4}{ }^{2-}\) (b) \(\mathrm{Al}(\mathrm{OH})_{3}+3 \mathrm{HNO}_{3} \rightleftharpoons \mathrm{Al}^{3+}+3 \mathrm{H}_{2} \mathrm{O}+3 \mathrm{NO}_{3}-\) (c) \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\) (d) \(\mathrm{CN}^{-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HCN}+\mathrm{OH}^{-}\) Equation Transcription: Text Transcription: Cu2 + + 4Cl ? ? CuCl42? Al(OH)3 + 3HNO3 ? Al3 + + 3H2O + 3NO3? N2 + 3H2 ? 2NH3 CN ? +H2O ? HCN + OH ?

Many molecules with central atoms from Period \(3\) or higher take part in Lewis acid-base reactions in which the central atom expands its valence shell. \(\mathrm{SnCl}_{4}\) reacts with \(\left(\mathrm{CH}_{3}\right)_{3}\)N as follows: (a) Identify the Lewis acid and the Lewis base in the reaction. (b) Give the nl designation of the sublevel of the central atom in the acid that accepts the lone pair. Equation Transcription: SnCl4 (CH3)3 Text Transcription: 3 SnCl_4 (CH_3)_3

Problem 103P Thiamine hydrochloride (C12H18ON4SCl2) is a watersoluble form of thiamine (vitamin B1; Ka = 3.37×10-7). How many grams of the hydrochloride must he dissolved in 10.00 mL of water to give a pH of 3.50?

Esters, \(RCOOR\) ' , are formed by the reaction of carboxylic acids, \(RCOOH\), and alcohols, R'OH, where R and R' are hydrocarbon groups. Many esters are responsible for the odors of fruit and, thus, have important uses in the food and cosmetics industries. The first two steps in the mechanism of ester formation are Identify the Lewis acids and Lewis bases in these two steps. Equation Transcription: Text Transcription: RCOOR RCOOH

Problem 100P A chemist makes four successive 1:10 dilutions of 1.0× 10-5 M HCl. Calculate the pH of the original solution and of each diluted solution (through 1.0× 10-9 M HCl).

Problem 101P Hydrogen peroxide, H2O2 (pKa = 11.75), is a bleaching agent and antiseptic. It is sold as 3% H2O2 by mass and contains 0.001% H3PO4 by mass to stabilize the solution. Which contributes more H3O+ to the solution, the H2O2 or the H3PO4?

The beakers shown contain \(0.300 L\) of aqueous solutions of a moderately weak acid HY. Each particle represents \(0.010 mol\); solvent molecules are omitted for clarity. (a) The reaction in beaker A is at equilibrium. Calculate for B, C, and D to determine which, if any, is also at equilibrium. (b) For any not at equilibrium, in which direction does the reaction proceed? (c) Does dilution affect the extent of dissociation of a weak acid? Explain. Equation Transcription: Text Transcription: 0.300 L 0.010 mol

Problem 105P When Fe3+ salts are dissolved in water, the solution becomes acidic due to formation of Fe(H2O)5OH2+ and H3O+. The overall process involves both Lewis and Bronsted-Lowry acid-base reactions. Write the equations for the process.

Problem 106P At 50°C and 1 atm,Kw = 5.19×10-14. At these conditions, find (a) [H3O+] in pure water, (b) [H3O+] in 0.010 M NaOH, and (c) [OH-] in 0.0010 M HClO4. (d) Find [H3O+] in 0.0100 M KOH at 100°C and 1000 atm (Kw = 1.10× 10-12). (e) Find the pH of pure water at 100°C and 1000 atm.

Problem 107P A 1.000 m solution of chloroacetic acid (ClCH2COOH) freezes at ?1.93°C. Find the K.a of chloroacetic acid. (Assume the molarities equal the molalities.)

Problem 109P Calcium propionate [Ca(CH3CH2COO)2; calcium propanoate] is a mold inhibitor used in food, tobacco, and pharmaceuticals. (a) Use balanced equations to show whether aqueous calcium propionate is acidic, basic, or neutral, (b) Use Appendix C to find the resulting pH when 8.75 g of Ca(CH3CH2COO)2 dissolves in enough water to give 0.500 L of solution.

Problem 111P (a) If Kw = 1.139×10-15at 0°C and 5.474X 10-14 at 50°C, find [H3O+] and pH of water at 0°C and 50°C. ________________ (b)The autoionization constant for heavy water (deuterium oxide, D2O) is 3.64×10-2 at 0°C and 7.89×10-15 at 50°C. Find [D3O+] and pD of heavy water at 0°C and 50°C. ________________ (c)Suggest a reason for these differences.

Problem 112P HX (? = 150. g/mol) and HY (? = 50.0 g/mol) are weak acids. A solution of 12.0 g/L of HX has the same pH as one containing 6.00 g/L of HY. Which is the stronger acid? Why?

Problem 113P Nitrogen is discharged from wastewater treatment facilities into rivers and streams, usually as NH3 and NH4+: NH3(aq)+H2O(l)?NH4+(aq)+OH? (aq) Kb = 1.76×10?5 One strategy for removing it is to raise the pH and “strip” the NH3 from solution by bubbling air through the water, (a) At pH 7.00, what fraction of the total nitrogen in solution is NH3, defined as [NH3]/([NH3] + [NH4+])? ________________ (b) What is the fraction at pH 10.00? (c) Explain the basis of ammonia stripping.

In each equation, label the acids, bases, and conjugate acid-base pairs: (a) \(\mathrm{NH}_{4}^{+}+\mathrm{CN}^{-} \rightleftharpoons \mathrm{NH}_{3}+\mathrm{HCN}\) (b) \(\mathrm{H}_{2} \mathrm{O}+\mathrm{HS}^{-} \rightleftharpoons \mathrm{OH}^{-}+\mathrm{H}_{2} \mathrm{~S}\) (c) \(\mathrm{HSO}_{3}^{-}+\mathrm{CH}_{3} \mathrm{NH}_{2} \rightleftharpoons \mathrm{SO}_{3}^{2-}+\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) Equation Transcription: Text Transcription: NH_4^+ + CN ? ? NH_3 + HCN H_2O + HS ? ? OH ? +H_2S HSO_3? + CH_3NH_2 ? SO_3^2 - + CH_3NH_3^+

Drinking water is often disinfected with chlorine gas, which hydrolyzes to form hypochlorous acid \((\mathrm{HClO})\), a weak acid but powerful disinfectant: \(\mathrm{Cl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HClO}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{Cl}^{-}(a q)\) The fraction of $\mathrm{HClO}$ in solution is defined as \(\frac{[\mathrm{HClO}]}{[\mathrm{HClO}]+\left[\mathrm{ClO}^{-}\right]}\) (a) What is the fraction of \(\mathrm{HClO}\) at \(\mathrm{pH} 7.00\left(K_{\mathrm{a}}\right.\) of \(\mathrm{HClO}=\) \(2.9 \times 10^{-8}\) )? (b) What is the fraction at \(\mathrm{pH} 10.00\) ? Equation Transcription: Text Transcription: Cl2(aq) + 2H2O(l) ? HClO(aq) + H3O+(aq) + Cl?(aq) HClOHClO + ClO ? pH 7.00 (Ka of HClO = 2.9x10-8)