Write formulas for each of the following acids and

Problem 1QP Indicate each of the following statements as a characteristic of an acid, base, or both: a. has a sour taste b. neutralizes bases c. produces H+ ions in water d. is named potassium hydroxide e. is an electrolyte

Problem 1SC a. Identify as an acid or base and give the name for HClO3. b. Write the formula for iron(III) hydroxide.

Problem 2QP Indicate each of the following statements as a characteristic of an acid, base, or both: a. neutralizes acids b. produces OH? ions in water c. has a slippery feel d. conducts an electrical current e. turns litmus red

Problem 2SC When HNO3 reacts with water, water acts as a Brønsted–Lowry base. Write the equation for the reaction.

Problem 3QP Name each of the following acids and bases: a. HCl b. Ca(OH)2 c. H2CO3 d. HNO3 e. H2SO3 f. Fe(OH)2

Problem 3SC In the following reaction, identify the conjugate acid–base pairs: HNO2(aq) + SO42?(aq) ? NO2?(aq) + HSO4?(aq)

Problem 4QP Name each of the following acids and bases: a. Al(OH)3 b. HBr c. H2SO4 d. KOH e. HNO2 f. HBrO2

Problem 5QP Write formulas for each of the following acids and bases: a. magnesium hydroxide b. hydrofluoric acid c. phosphorus acid d. lithium hydroxide e. copper(II) hydroxide

Problem 4SC Using Table 10.4, determine whether nitrous acid or carbonic acid is the stronger acid. Explain your answer. TABLE 10.4 Ka Values for Selected Weak Acids Acid Formula Ka >Phosphoric acid H3PO4 7.5 × 10?3 Hydrofluoric acid HF 7.2 × 10?4 Nitrous acid HNO2 4.5 × 10?4 Formic acid HCHO2 1.8 × 10?4 Acetic acid HC2H3O2 1.8 × 10?5 Carbonic acid H2CO3 4.3 × 10?7 Hydrosulfuric acid H2S 9.1 × 10?8 Dihydrogen phosphate H2PO4? 6.2 × 10?8 Bicarbonate HCO3? 5.6 × 10?11 Hydrogen phosphate HPO42? 2.2 × 10?13

Problem 5SC What is the [H3O+] of an ammonia cleaning solution with [OH?] = 4.0 × 10?4 M? Is the solution acidic, basic, or neutral?

Problem 6QP Write formulas for each of the following acids and bases: a. barium hydroxide b. hydroiodic acid c. nitric acid d. strontium hydroxide e. sodium hydroxide

Problem 6SC What is the pH of bleach with [H3O+] = 4.2 × 10?12 M?

Problem 7QP Identify the reactant that is a Brønsted–Lowry acid and the reactant that is a Brønsted–Lowry base in each of the following: a. HI(aq) + H2O(l) ? H3O+(aq) + I?(aq) b. F?(aq) + H2O(l) ? HF(aq) + OH?(aq)

Problem 7SC Calculate the pH of a sample of acid rain that has [OH?] = 2 × 10?10 M.

Problem 8QP Identify the reactant that is a Brønsted–Lowry acid and the reactant that is a Brønsted–Lowry base in each of the following: a. CO32?(aq) + H2O(l) ? HCO3?(aq) + OH?(aq) b. H2SO4(aq) + H2O(l) ? H3O+(aq) + HSO4?(aq)

Problem 8SC What are the [H3O+] and [OH?] of a beer that has a pH of 4.7?

Problem 9QP Write the formula and name of the conjugate base for each of the following: a. HF b. H2O c. H2CO3 d. HSO4?

Problem 9SC Write the balanced equation for the reaction between H2SO4 and LiOH.

Problem 10QP Write the formula and name of the conjugate base for each of the following: a. HCO3? b. H3O+ c. HPO42? d. HNO2

Problem 10SC What is the molarity of an HCl solution if 28.6 mL of a 0.175 M NaOH solution is needed to neutralize a 25.0-mL sample of the HCl solution?

Problem 11QP Write the formula and name of the conjugate acid for each of the following: a. CO32? b. H2O c. H2PO4? d. SO32?

Problem 11SC The acid–base pair in a buffer is H2PO4?/HPO42?, which has a Ka of 6.2 × 10?8. What is the pH of a buffer that is made of 0.10 M H2PO4? and 0.50 M HPO42??

Problem 12QP Write the formula and name of the conjugate acid for each of the following: a. SO42? b. BrO2? c. OH? d. ClO?

Problem 13QP Identify the Brønsted–Lowry acid–base pairs in each of the following equations: a. H2CO3(aq) + H2O(l) ? H3O+(aq) + HCO3?(aq) b. NH4+(aq) + H2O(l) ? H3O+(aq) + NH3(aq) c. HCN(aq) + NO2?(aq) ? CN?(aq) + HNO2(aq)

Problem 14QP Identify the Brønsted–Lowry acid–base pairs in each of the following equations: a. H3PO4(aq) + H2O(l) ? H3O+(aq) + H2PO4?(aq) b. CO32?(aq) + H2O(l) ? OH?(aq) + HCO3?(aq) c. H3PO4(aq) + NH3(aq) ? NH4+(aq) + H2PO4?(aq)

Problem 15QP 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”?

Problem 17CI Methane is a major component of purified natural gas used for heating and cooking. When 1.0 mole of methane gas burns with oxygen to produce carbon dioxide and water vapor, 883 kJ of heat is produced. At STP, methane gas has a density of 0.715 g/L. For transport, the natural gas is cooled to ?163°C to form liquefied natural gas (LNG) with a density of 0.45 g/mL. A tank on a ship can hold 7.0 million gallons of LNG. (1.10, 5.5, 6.1, 6.5, 6.6, 6.7, 6.9, 7.7) An LNG carrier transports liquefied natural gas. a. Draw the electron-dot formula for methane, which has the formula CH4. b. What is the mass, in kilograms, of LNG (assume that LNG is all methane) transported in one tank on a ship? c. What is the volume, in liters, of methane gas when the LNG (methane) from one tank is converted to gas at STP? d. Write the balanced equation for the combustion of methane in a gas burner, including the heat of reaction. Methane is the fuel burned in a gas cooktop. e. How many kilograms of oxygen are needed to react with all of the methane from one tank of LNG? f. How much heat, in kilojoules, is released after burning all of the methane from one tank of LNG?

Problem 17QP Answer true or false for each of the following: A strong acid a. is completely ionized in aqueous solution b. has a small value of Ka c. has a strong conjugate base d. has a weak conjugate base e. is slightly ionized in aqueous solution

Problem 18CI Automobile exhaust is a major cause of air pollution. One pollutant is nitrogen oxide, which forms from nitrogen and oxygen gases in the air at the high temperatures in an automobile engine. Once emitted into the air, nitrogen oxide reacts with oxygen to produce nitrogen dioxide, a reddish-brown gas with a sharp, pungent odor that makes up smog. One component of gasoline is octane, C8H18, which has a density of 0.803 g/mL. In one year, a typical automobile uses 550 gal of gasoline and produces 41 lb of nitrogen oxide. (1.10, 6.1, 6.5, 6.6, 6.7, 7.7) Two gases found in automobile exhaust are carbon dioxide and nitrogen oxide. a. Write balanced equations for the production of nitrogen oxide and nitrogen dioxide. b. If all the nitrogen oxide emitted by one automobile is converted to nitrogen dioxide in the atmosphere, how many kilograms of nitrogen dioxide are produced in one year by a single automobile? c. Write a balanced equation for the combustion of octane. d. How many moles of C8H18 are present in 15.2 gal of octane? e. How many liters of CO2 at STP are produced in one year from the gasoline used by the typical automobile?

Problem 18QP Answer true or false for each of the following: A weak acid a. is completely ionized in aqueous solution b. has a small value of Ka c. has a strong conjugate base d. has a weak conjugate base e. is slightly ionized in aqueous solution

Problem 19QP Using Table 10.3, identify the stronger acid in each of the following pairs: a. HBr or HNO2 b. H3PO4 or HSO4? c. NH4+ or H2CO3 TABLE 10.3 Some Conjugate Acid–Base Paris

Problem 20CI In wine making, glucose (C6H12O6) from grapes undergoes fermentation in the absence of oxygen to produce ethanol and carbon dioxide. A bottle of vintage port wine has a volume of 750 mL and contains 135 mL of ethanol (C2H6O). Ethanol has a density of 0.789 g/mL. In 1.5 lb of grapes, there are 26 g of glucose. (1.9, 1.10, 6.1, 6.5, 6.6, 6.7, 8.4) When the glucose in grapes is fermented, ethanol is produces. Port is a type of fortified wine that is produced in Portugal. a. Calculate the volume percent (v/v) of ethanol in the port wine. b. What is the molarity (M) of ethanol in the port wine? c. Write the balanced equation for the fermentation reaction of glucose. d. How many grams of glucose are required to produce one bottle of port wine? e. How many bottles of port wine can be produced from 1.0 ton of grapes? (1 ton = 2000 lb)

Problem 20QP Using Table 10.3, identify the stronger acid in each of the following pairs: a. NH4+ or H3O+ b. HNO2 or HCl c. H2O or H2CO3 TABLE 10.3 Some Conjugate Acid–Base Paris Step-by-step solution

Problem 21CI Consider the following reaction at equilibrium: 2H2(g) + S2(g) ? 2H2S(g) In a 10.0-L container, an equilibrium mixture contains 2.02 g of H2, 10.3 g of S2, and 68.2 g of H2S. (9.2, 9.3, 9.4. 9.5) a. What is the Kc value for this equilibrium mixture? b. If more H2 is added to the mixture, how will the equilibrium shift? c. How will the equilibrium shift if the mixture is placed in a 5.00-L container with no change in temperature? d. If a 5.00-L container has an equilibrium mixture of 0.300 mole of H2 and 2.50 moles of H2S, what is the [S2] if temperature is the same?

Problem 21QP Identify the weaker acid in each of the following pairs: a.HCl or HSO4? b.HNO2 or HF c.HCO3? or NH4+

Problem 22CI A mixture of 25.0 g of CS2 gas and 30.0 g of O2 gas is placed in 10.0-L container and heated to 125 °C. The products of the reaction are carbon dioxide gas and sulfur dioxide gas. (6.1, 6.5, 6.6, 6.7, 6.8, 7.8, 7.9) a. Write a balanced equation for the reaction. b. How many grams of CO2 are produced? c. What is the partial pressure of the remaining reactant? d. What is the final pressure in the container?

Problem 22QP Using Table 10.3, identify the weaker acid in each of the following pairs: a. HNO3 or HCO3? b. HSO4? or H2O c. H2SO4 or H2CO3 TABLE 10.3 Some Conjugate Acid–Base Paris

Problem 23CI A metal M with a mass of 0.420 g completely reacts with 34.8 mL of a 0.520 M HCl solution to form aqueous MCl3 and H2 gas. (6.1, 6.5, 6.6, 6.7, 7.8) When a metal reacts with a strong acid, hydrogen gas forms. a. Write a balanced equation for the reaction of the metal M(s) and HCl(aq). b. What volume, in milliliters, of H2 at 720. mmHg and 24 °C is produced? c. How many moles of metal M reacted? d. Use your results from part c to determine the molar mass and name of metal M. e. Write the balanced equation for the reaction.

Problem 23QP Using Table 10.3, predict whether each of the following reactions contains mostly reactants or products at equilibrium: a. H2CO3(aq) + H2O(l) ? H3O+(aq) + HCO3?(aq) b. NH4+(aq) + H2O(l) ? H3O+(aq) + NH3(aq) c. HNO2(aq) + NH3(aq) ? NO2?(aq) + NH4+(aq) TABLE 10.3 Some Conjugate Acid–Base Paris

Problem 24CI In a teaspoon (5.0 mL) of a liquid antacid, there are 400. mg of Mg(OH)2 and 400. mg of Al(OH)3. A 0.080 M HCl solution, which is similar to stomach acid, is used to neutralize 5.0 mL of the liquid antacid. (6.5, 6.6, 6.7, 10.4, 10.5) An antacid neutralizes stomach acid and raises the pH. a. Write the equation for the neutralization of HCl and Mg(OH)2. b. Write the equation for the neutralization of HCl and Al(OH)3. c. What is the pH of the HCl solution? d. How many milliliters of the HCl solution is needed to neutralize the Mg(OH)2? e. How many milliliters of the HCl solution is needed to neutralize the Al(OH)3?

Using Table 10.3, predict whether each of the following reactions contains mostly reactants or products at equilibrium: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{F}^{-}(a q) \rightleftarrows \mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)\) b. \(\mathrm{CO}_{3}{ }^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{OH}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q)\) c. \(\mathrm{HS}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-}(a q)\)

Consider the following acids and their dissociation constants: \(\begin{array}{r} \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{HSO}_{3}^{-}(a q) \\ K_{3}=1.2 \times 10^{-2} \end{array}\) \(\begin{array}{r} \mathrm{HS}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-}(a q) \\ K_{\mathrm{a}}=1.3 \times 10^{-19} \end{array}\) a. Which is the stronger acid, \(\mathrm{H}_{2} \mathrm{SO}_{3}\) or \(\mathrm{HS}^{-}\)? b. What is the conjugate base of \(\mathrm{H}_{2} \mathrm{SO}_{3}\)? c. Which acid has the weaker conjugate base? d. Which acid produces more ions?

Problem 26QP Consider the following acids and their dissociation constants: HPO42?(aq) + H2O(l) ? H3O+(aq) + PO43?(aq) Ka = 2.2 × 10?13 HCHO2(aq) + H2O(l) ? H3O+(aq) + CHO2?(aq) Ka = 1.8 × 10?4 a. Which is the weaker acid, HPO42? or HCHO2? b. What is the conjugate base of HPO42?? c. Which acid has the weaker conjugate base? d. Which acid produces more ions?

Problem 27QP Phosphoric acid dissociates to form dihydrogen phosphate and hydronium ion. Phosphoric acid has a Ka of 7.5 X 10?3. Write the equation for the reaction and the acid dissociation constant expression for phosphoric acid.

Problem 28QP Carbonic acid, a weak acid, reacts with water to form bicarbonate and hydronium ion. Write the equation for the dissociation of carbonic acid and the expression for its acid dissociation constant (Ka).

Problem 29QP Why are the concentrations of H3O + and OH equal in pure water?

Problem 30QP What is the meaning and value of Kw at 25 °C?

Problem 31QP In an acidic solution, how does the concentration of H3O+ compare to the concentration of OH??

Problem 32QP In a basic solution, how does the concentration of H3O+ compare to the concentration of OH??

Problem 33QP Indicate whether each of the following solutions is an acidic, basic, or neutral: a. [H3O + ] = 2.0 X 10?5M b.[H3O + ] = 1.4 X 10?9 M c.[OH? ] = 8.0 X 10?3 M d.[OH? ] = 3.5 X 10?10 M

Problem 34QP Indicate whether each of the following solutions is an acidic, basic, or neutral solution: a.[H3O + ] = 6.0 X 10?12M b.[H3O + ] = 1.4 X 10?4 M c.[OH? ] = 5.0 X 10?12 M d.[OH? ] = 4.5 X 10?2M

Problem 35QP Calculate the [H3O + ] of each aqueous solution with the following [OH? ]: a. coffee, 1.0 X 10?9M b. soap, 1.0 X 10?6 M c. cleanser, 2.0 X 10?5 M d. lemon juice, 4.0 X 10?13M

Problem 36QP Calculate the [H3O+] of each aqueous solution with the following [OH?]: a. dishwashing detergent, 1.0 × 10?3 M b. milk of magnesia, 1.0 × 10?5 M c. aspirin, 1.8 × 10?11 M d. seawater, 2.5 × 10?6 M

Problem 37QP Calculate the [OH? ] of each aqueous solution with the following [ H3O+ ] : a. vinegar, 1.0 X 10?3 M b. urine, 5.0 X 10?6 M c. ammonia solution, 1.8 X 10?12 M d. KOH solution, 4.0 X 10?13 M

Problem 38QP Calculate the [OH? ] of each aqueous solution with the following [ H3O+ ] : a. baking soda, 1.0 X 10-8M b. orange juice, 2.0 X 10?4M c. milk, 5.0 X 10?7M d. bleach, 4.8 X 10?12 M

Problem 39QP State whether each of the following is acidic, basic, or neutral: a. blood, pH 7.38 b. vinegar, pH 2.8 c. drain cleaner, pH 11.2 d. coffee, pH 5.54 e. tomatoes, pH 4.2 f. chocolate cake, pH 7.6

Problem 40QP State whether each of the following is acidic, basic, or neutral: a. soda, pH 3.22 b. shampoo, pH 5.7 c. laundry detergent, pH 9.4 d. rain, pH 5.83 e. honey, pH 3.9 f. cheese, pH 5.2

Problem 41QP Calculate the pH of each solution given the following: a. [H3O + ] = 1.0 X 10?4 M b.[h3O + ] = 3.0 X 10?9 M c.[OH? ] = 1.0 X 10?5 M d.[OH? ] = 2.5 X 10?11 M e.[h3O + ] = 6.7 X 10?8 M f.[OH? ] = 8.2 X 10?4 M

Problem 42QP Calculate the pH of each solution given the following: a.[H3O+ ] = 1.0 X 10?8 M b.[h3O + ] = 5.0 X 10?6 M c.[OH? ] = 4.0 X 10?2 M d. [OH? ] = 8.0 X 10?3 M e.[h3O + ] = 4.7 X 10?2 M f.[OH? ] = 3.9 X 10?6 M

Complete the following table:

Problem 44QP Complete the following table: [H3O+] [OH?] pH Acidic, Basic, or neutral? 10.00 Neutral 6.4 × 10?12 M 11.3

Predict the products and write the balanced equation for the reaction of HCl with each of the following metals: a. Li b. Mg c. Sr

Predict the products and write the balanced equation for the reaction of \(\mathrm{HNO}_{3}\) with each of the following metals: a. Ca b. Zn c. Al

Problem 47QP Predict the products and write the balanced equation for the reaction of HBr with each of the following carbonates or hydrogen carbonates: a. LiHCO3 b. MgCO3 c. SrCO3

Problem 48QP Predict the products and write the balanced equation for the reaction of H2SO4 with each of the following carbonates or hydrogen carbonates: a. CaCO3 b. Na2CO3 c. CsHCO3

Problem 49QP Balance each of the following neutralization reactions: a. HCl(aq) + Mg(OH)2(s) ? MgCl2(aq) + H2O(l) b. H3PO4(aq) + LiOH(aq) ? Li3PO4(aq) + H2O(l) c. H2SO4(aq) + Sr(OH)2(s) ? SrSO4(aq) + H2O(l)

Problem 50QP Balance each of the following neutralization reactions: a. HNO3(aq) + Ba(OH)2(s) ? Ba(NO3)2(aq) + H2O(l) b. H2SO4(aq) + Al(OH)3(s) ? Al2(SO4)3(aq) + H2O(l) c. H3PO4(aq) + KOH(aq) ? K3PO4(aq) + H2O(l)

Problem 51QP Write a balanced equation for the neutralization of each of the following: a. H2SO4(aq) and NaOH(aq) b. HCl (aq) and Fe (OH)3 (s) c. H2CO3(aq) and Mg(OH)2(s)

Problem 52QP Write a balanced equation for the neutralization of each of the following: a. H3PO4 (aq) and NaOH (aq) b. HI (aq) and LiOH (aq) c. HNO3(aq) and Ca(OH)2(s)

Problem 53QP What is the molarity of a solution of HCl if 5.00 mL of the HCl solution is titrated with 28.6 mL of 0.145 M NaOH solution? HCl (aq) + NaOH (aq) ?H2O(l) + NaCl (aq)

If 29.7 mL of a 0.205 M KOH solution is required to neutral­ize completely 25.0 mL of a solution of \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), what is the molarity of the acetic acid solution? \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \longrightarrow \mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

Problem 55QP If 38.2 mL of a 0.162 M KOH solution is required to neutralize completely 25.0 mL of an H2SO4 solution, what is the molarity of the acid solution? H2SO4(aq) + 2KOH(aq) ? K2SO4(aq) + 2H2O(l)

A solution of 0.162 M NaOH is used to neutralize 25.0 mL of a \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution. If 32.8 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution? \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

Problem 57QP A solution of 0.204 M NaOH is used to neutralize 50.0 mL of an H3PO4 solution. If 16.4 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution? H3PO4(aq) + 3NaOH(aq) ? Na3PO4(aq) + 3H2O(l)

Problem 58QP A solution of 0.312 M KOH is used to neutralize 15.0 mL of an H3PO4 solution. If 28.3 mL of the KOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution? H3PO4(aq) + 3KOH(aq) ? K3PO4(aq) + 3H2O(l)

Problem 59QP Which of the following represents a buffer system? Explain. a. NaOH and NaCl b. H2CO3 and NaHCO3 c. HF and KF d. KCl and NaCl

Problem 60QP Consider the following: (1) HClO2, (2) NaNO3, (3) HC2H3O2 and NaC2H3O2, and (4) HCl and NaOH. Which of these represent a buffer system? Explain.

Consider the buffer system of hydrofluoric acid, HF, and its salt, NaF. \(\mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{F}^{-}(a q)\) a. The purpose of the buffer system is to: 1. maintain [HF] 2. maintain \(\left[\mathrm{F}^{-}\right]\) 3. maintain pH 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. The addition of \(\mathrm{OH}^{-}\) 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

Problem 62QP Consider the buffer system of nitrous acid, HNO2, and its salt, NaNO2. HNO2(aq) + H2O(l) ? H3O+(aq) + NO2?(aq) a. The purpose of the buffer system is to: 1. maintain [HNO2] 2. maintain [NO2?] 3. maintain pH b. The weak acid is needed to: 1. provide the conjugate base 2. neutralize added OH? 3. provide the conjugate acid c. The addition of H3O+ is neutralized by: 1. the salt 2. H2O 3. OH? d. When OH? is added, the equilibrium shifts in the direction of the: 1. reactants 2. products 3. does not change

Problem 63QP Nitrous acid has a Ka of 4.5 X 104. What is the pH of a buffer solution containing 0.10 M HNO2 and 0.10 M NO2? ?

Problem 64QP Acetic acid has a Ka of 1.8 X 105. What is the pH of a buffer solution containing 0.15 M HC2H3O2 and 0.15 M C2H3O2? ?

Problem 65QP Using Table 14.5 for Ka values, compare the pH of a HF buffer that contains 0.10 M HF and 0.10 M NaF with another HF buffer that contains 0.060 M HF and 0.120 M NaF.

Using Table 10.4 for \(K_{\mathrm{a}}\) values, compare the \(\mathrm{pH}\) of an \(\mathrm{H}_2 \mathrm{CO}_3\) buffer that contains 0.10 \(\mathrm{M} \mathrm{H}_2 \mathrm{CO}_3\) and 0.10 \(\mathrm{M} \mathrm{NaHCO}_3\) with another \(\mathrm{H}_2 \mathrm{CO}_3\) buffer that contains 0.15 \(\mathrm{M} \mathrm{H}_2 \mathrm{CO}_3\) and 0.050 \(\mathrm{M} \mathrm{NaHCO}_3\).

Problem 67UTC In each of the following diagrams of acid solutions, determine if each diagram represents a strong acid or a weak acid. The acid has the formula HX. (10.2)

Problem 68UTC Adding a few drops of a strong acid to water will lower the pH appreciably. However, adding the same number of drops to a buffer does not appreciably alter the pH. Why? (10.6)

Problem 69UTC Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting. a. What changes occur in the blood pH during hyperventilation? b. How does breathing into a paper bag help return blood pH to normal?

Problem 70UTC In the blood plasma, pH is maintained by the carbonic acid–bicarbonate buffer system. (10.6) a. Which component of the carbonic acid–bicarbonate buffer reacts when acid is added? b. Which component of the carbonic acid–bicarbonate buffer reacts when base is added?

Problem 71AQP Identify each of the following as an acid, base, or salt, and give its name: (10.1) a. LiOH b. Ca(NO3)2 c. HBr d. Ba(OH)2 e. H2CO3 f. HClO2

Problem 72AQP Identify each of the following as an acid, base, or salt, and give its name: (10.1) a. H3PO4 b. MgBr2 c. NH3 d. H2SO4 e. NaCl f. KOH

Problem 73AQP Identify the conjugate acid–base pairs in each of the following equations and state whether the equilibrium mixture contains mostly products or mostly reactants: (10.5) a. NH3(aq) + HNO3(aq) ? NH4+(aq) + NO3?(aq) b. H2O(l) + HBr(aq) ? H3O+(aq) + Br?(aq)

Identify the conjugate acid–base pairs in each of the following equations and state whether the equilibrium mixture contains mostly products or mostly reactants: (10.5) a. \(\mathrm{HNO}_{2}(a q)+\mathrm{HS}^{-}(a q) \rightleftarrows \mathrm{H}_{2} \mathrm{~S}(g)+\mathrm{NO}_{2}^{-}(a q)\) b. \(\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{OH}^{-}(a q)+\mathrm{HCl}(a q)\)

Problem 75AQP Complete the following table: (10.1) Acid Conjugate Base Hl Cl? NH4+ HS?

Problem 76AQP Complete the following table: (10.1) Base Conjugate Acid HS? HC2H3O2 NH3 ClO4?

Problem 77AQP Are each of the following solutions acidic, basic, or neutral? a. rain, pH 5.2 b. tears, pH 7.5 c. tea, pH 3.8 d. cola, pH 2.5 e. photo developer, pH 12.0

Problem 78AQP Are each of the following solutions acidic, basic, or neutral? a. saliva, pH 6.8 b. urine, pH 5.9 c. pancreatic juice, pH 8.0 d. bile, pH 8.4 e. blood, pH 7.45

Using Table 10.3, identify the stronger acid in each of the following pairs: (10.2) a. \(\mathrm{HF}\) or \(\mathrm{H}_{2} \mathrm{~S}\) b. \(\mathrm{H}_{3} \mathrm{O}^{+}\) or \(\mathrm{H}_{2} \mathrm{CO}_{3}\) c. \(\mathrm{HNO}_{2}\) or \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. \(\mathrm{H}_{2} \mathrm{O}\) or \(\mathrm{HCO}_{3}^{-}\)

Problem 80AQP Using Table 10.3, identify the stronger base in each of the following pairs: (10.2) a. H2O or Cl? b. OH? or H2CO3 c. SO42? or NO2? d. CO32? or H2O TABLE 10.3 Some Conjugate Acid–Base Paris

Problem 81AQP Determine the pH and pOH for each of the following solutions: a.[H3O + ] = 2.0 X 10?8 M b.[H3O + ] = 5.0 X 10?2 M c.[OH? ] = 3.5 X 10?4 M d.[OH? ] = 0.0054 M

Problem 82AQP Determine the pH and pOH for each of the following solutions: a.[OH? ] = 1.0 X 10?7 M b.[H3O + ] = 4.2 X 10?3 M c.[H3O + ] = 0.0001 M d.[OH? ] = 8.5 X 10?9 M

Problem 83AQP Are the solutions in Problem 14.87 acidic, basic, or neutral? Problem 14.87 Determine the pH and pOH for each of the following solutions: a.[H3O + ] = 2.0 X 10?8 M b.[H3O + ] = 5.0 X 10?2 M c.[OH? ] = 3.5 X 10?4 M d.[OH? ] = 0.0054 M

Problem 84AQP Are the solutions in Problem 14.88 acidic, basic, or neutral? Problem 14.88 Determine the pH and pOH for each of the following solutions: a.[OH? ] = 1.0 X 10?7 M b.[H3O + ] = 4.2 X 10?3 M c.[H3O + ] = 0.0001 M d.[OH? ] = 8.5 X 10?9 M

Problem 85AQP What are the [H3O+] and [OH?] for a solution with each of the following pH values? (10.3, 10.4) a. 3.00 b. 6.48 c. 8.85 d. 11.00

Problem 86AQP What are the [H3O+] and [OH?] for a solution with each of the following pH values? (10.3, 10.4) a. 10.0 b. 5.0 c. 7.00 d. 1.82

Problem 87AQP Solution A has a pH of 4.5, and solution B has a pH of 6.7. a. Which solution is more acidic? b. What is the [H3O+] in each? c. What is the [OH?] in each?

Problem 88AQP A solution of borax (A) has a pH of 9.2, and human saliva (B) has a pH of 6.5. (10.4) a. Which solution is more acidic? b. What is the [H3O+] in each? c. What is the [OH?] in each?

Problem 89AQP What is the [OH-] in a solution that contains 0.225 g of NaOH in 0.250 L of solution?

Problem 90AQP What is the [H3O+]in a solution that contains 1.54 g of HNO3 in 0.500 L of solution?

What is the pH and pOH of a solution prepared by dissolving 2.5 g of HCl in water to make 425 mL of solution?

Problem 92AQP What is the pH and pOH of a solution prepared by dissolving 1.00 g of Ca (OH)2 in water to make 875 mL of solution?

Problem 93AQP a. Write the neutralization equation for KOH and H3PO4. (10.5) b. Calculate the volume (mL) of a 0.150 M KOH solution that will completely neutralize 10.0 mL of a 0.560 M H3PO4 solution.

Problem 94AQP a. Write the neutralization equation for NaOH and H2SO4. (10.5) b. How many milliliters of a 0.215 M NaOH solution are needed to completely neutralize 2.50 mL of a 0.825 M H2SO4 solution?

Problem 95CQ For each of the following: (10.1, 10.2) 1. H2S 2. H3PO4 a. Write the formula for the conjugate base. b. Write the Ka expression. c. Which is the weaker acid?

Problem 96CQ For each of the following: (10.1, 10.2) 1. HCO3? 2. HC2H3O2 a. Write the formula for the conjugate base. b. Write the Ka expression. c. Which is the stronger acid?

Problem 97CQ A solution of 0.205 M NaOH is used to neutralize 20.0 mL of a H2SO4 solution. If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4 solution? H2SO4(aq) + 2NaOH(aq) ? 2H2O(l) + Na2SO4(aq)

Problem 98CQ A 10.0-mL sample of vinegar, which is an aqueous solution of acetic acid, HC2H3O2, 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? HC2H3O2(aq) + NaOH (aq) ? H2O(l) + NaC2H3O2 (aq)

Problem 99CQ A buffer is made by dissolving H3PO4 and NaH2PO4 in water. (10.6) 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 0.10 M H3PO4 and 0.10 M 2PO4?; the Ka for H3PO4 is 7.5 × 10?3. d. Calculate the pH of this buffer if it contains 0.50 M H3PO4 and 0.20 M H2PO4?; the Ka for H3PO4 is 7.5 × 10?3.

A buffer 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. (10.6) 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 0.10 M \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and 0.10 M \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\); the \(K_{\mathrm{a}}\) for \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \text { is } 1.8 \times 10^{-5}\). d. Calculate the pH of this buffer if it contains 0.20 M \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and 0.40 M \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\); the\(K_{\mathrm{a}}\) for \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) is \(1.8 \times 10^{-5}\) . .

Problem 101CQ Determine each of the following for a 0.050 M KOH solution: (10.5) a. [H3O+] b. pH c. the balanced equation when reacted with H2SO4 d. milliliters of KOH solution required to neutralize 40.0 mL of a 0.035 M H2SO4 solution

Problem 102CQ Determine each of the following for a 0.100 M HBr solution:(10.5) a. [H3O+] b. pH c. the balanced equation when reacted with LiOH d. milliliters of HBr solution required to neutralize 36.0 mL of a 0.250 M LiOH solution

Problem 103CQ 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. (10.3, 10.4, 10.5) A helicopter drops calcium carbonate on an acidic lake to increase its pH. a. What are the [H3O+] and [OH?] of Little Echo Pond? b. What are the [H3O+] and [OH?] 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 (CaCO3). How many grams of CaCO3 are needed to neutralize 1.0 kL of the acidic water from Little Echo Pond if we assume all the acid is sulfuric acid? H2SO4(aq) + CaCO3(s) ? CO2(g) + H2O(l) + CaSO4(aq)

Problem 104CQ The daily output of stomach acid (gastric juice) is 1000 mL to 2000 mL. Prior to a meal, stomach acid (HCl) typically has a pH of 1.42. (10.3, 10.4, 10.5) a. What is the [H3O+] of stomach acid? b. One chewable tablet of the antacid Maalox contains 600. mg of CaCO3. 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 Mg(OH)2 per teaspoon. Write the neutralization equation and calculate the milliliters of stomach acid that are neutralized by 1 tablespoon of milk of magnesia (1 tablespoon = 3 teaspoons).

Problem 19CI A piece of magnesium with a mass of 0.121 g is added to 50.0 mL of a 1.00 M HCl solution at a temperature of 22.0°C. When the magnesium dissolves, the solution reaches a temperature of 33.0°C. (2.5, 6.5, 6.6, 6.7, 6.8, 7.8) Mg(s) + 2HCl(aq) ? MgCl2(aq) + H2(g) Magnesium metal reacts rapidly with HCl. a. What is the limiting reactant? b. What volume, in liters, of hydrogen gas would be produced if the pressure is 750. mmHg and the temperature is 33.0°C? c. How many joules were released by the reaction of the magnesium? Assume the density and specific heat of the HCl solution are the same as for water. d. What is the heat of reaction for magnesium in J/g? In kJ/mole?