What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2) is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H) and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 ´ 10–5) a. 2.52 b. 4.23 c. 4.44 d. 4.64 e. 4.74 ____ 5. If 0.50 L of a buffer containing 1.0 mol H2PO4- and 1.0 mol HPO42- is diluted to a volume of 5.0 L, the pH a. increases by 1. b. decreases by 1. c. increases by 10. d. decreases by 10. e. remains unchanged. ____ 6. Which of the following conditions is/are met at the equivalence point of the titration of a monoprotic weak base with a strong acid? 1. The moles of acid added from the buret equals the initial moles of weak base. 2. The volume of acid added from the buret must equal the volume of base titrated. 3. The pH of the solution is less than 7.00. a. 1 only b. 2 only c. 3 only d. 1 and 3 e. 2 and 3 ____ 7. A volume of 25.0 mL of 0.100 M C6H5CO2H(aq) is titrated with 0.100 M NaOH(aq). What is the pH after the addition of 12.5 mL of NaOH? (Ka of benzoic acid = 6.3 ´ 10–5) a. 2.60 b. 4.20 c. 5.40 d. 7.00 e. 8.60 ____ 8. A 50.0 mL sample of 0.155 M HNO2(aq) is titrated with 0.100 M NaOH(aq). What is the pH of a solution after the addition of 25.0 mL of NaOH? (Ka of HNO2 = 4.5 ´ 10–4) a. 3.02 b. 3.22 c. 3.67 d. 3.86 e. 4.05 ____ 9. The Ksp of BaSO4 is 1.1 ´ 10–10 at 25 °C. What mass of BaSO4 (molar mass = 233.4 g/mol) will dissolve in 1.0 L of water at 25 °C? a. 2.6 ´ 10-8 g b. 4.5 ´ 10-8 g c. 1.0 ´ 10-5 g d. 1.6 ´ 10-4 g e. 2.4 ´ 10-3 g ____ 10. The Ksp of AgI is 8.5 ´ 10–17 at 25 °C. Calculate the molar solubility of AgI in 0.0045 M KI(aq) at 25 °C. a. 1.9 ´ 10–14 mol/L b. 3.8 ´ 10–12 mol/L c. 9.2 ´ 10–9 mol/L d. 1.4 ´ 10–7 mol/L e. 2.0 ´ 10–6 mol/L ____ 11. What is the molar solubility of Fe(OH)3(s) in a solution that is buffered at pH 2.50 at 25 °C? The Ksp of Fe(OH)3 is 6.3 ´ 10–38 at 25 °C. a. 6.9 ´ 10–28 mol/L b. 2.0 ´ 10–26 mol/L c. 1.3 ´ 10–13 mol/L d. 2.0 ´ 10–3 mol/L e. 5.0 ´ 102 mol/L ____ 12. The concentration of Pb2+ in an aqueous solution is 5.5 ´ 10–3 M. What concentration of SO42– is required to begin precipitating PbSO4? The Ksp of PbSO4 is 2.5 ´ 10–8. a. 1.4 ´ 10–10 M b. 4.5 ´ 10–6 M c. 1.6 ´ 10–4 M d. 8.3 ´ 10–4 M e. 2.9 ´ 10–2 M ____ 13. An aqueous solution contains 0.010 M Br– and 0.010 M I–. If Ag+ is added until AgBr(s) just begins to precipitate, what are the concentrations of Ag+ and I–? (Ksp of AgBr = 5.4 ´ 10–13, Ksp of AgI = 8.5 ´ 10–17) a. [Ag+] = 5.4 ´ 10–11 M, [I–] = 1.0 ´ 10–2 M b. [Ag+] = 8.5 ´ 10–15 M, [I–] = 1.0 ´ 10–2 M c. [Ag+] = 5.4 ´ 10–11 M, [I–] = 1.6 ´ 10–6 M d. [Ag+] = 8.5 ´ 10–15 M, [I–] = 6.4 ´ 101 M e. [Ag+] = 8.5 ´ 10–15 M, [I–] = 1.6 ´ 10–6 M

What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2) is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H) and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 ´ 10–5) a. 2.52 b. 4.23 c. 4.44 d. 4.64 e. 4.74 5. If 0.50 L of a buffer containing 1.0 mol H2PO4- and 1.0 mol HPO42- is diluted to a volume of 5.0 L, the pH a. increases by 1. b. decreases by 1. c. increases by 10. d. decreases by 10. e. remains unchanged. 6. Which of the following conditions is/are met at the equivalence point of the titration of a monoprotic weak base with a strong acid? 1. The moles of acid added from the buret equals the initial moles of weak base. 2. The volume of acid added from the buret must equal the volume of base titrated. 3. The pH of the solution is less than 7.00. a. 1 only b. 2 only c. 3 only d. 1 and 3 e. 2 and 3 7. A volume of 25.0 mL of 0.100 M C6H5CO2H(aq) is titrated with 0.100 M NaOH(aq). What is the pH after the addition of 12.5 mL of NaOH? (Ka of benzoic acid = 6.3 ´ 10–5) a. 2.60 b. 4.20 c. 5.40 d. 7.00 e. 8.60 8. A 50.0 mL sample of 0.155 M HNO2(aq) is titrated with 0.100 M NaOH(aq). What is the pH of a solution after the addition of 25.0 mL of NaOH? (Ka of HNO2 = 4.5 ´ 10–4) a. 3.02 b. 3.22 c. 3.67 d. 3.86 e. 4.05 9. The Ksp of BaSO4 is 1.1 ´ 10–10 at 25 °C. What mass of BaSO4 (molar mass = 233.4 g/mol) will dissolve in 1.0 L of water at 25 °C? a. 2.6 ´ 10-8 g b. 4.5 ´ 10-8 g c. 1.0 ´ 10-5 g d. 1.6 ´ 10-4 g e. 2.4 ´ 10-3 g 10. The Ksp of AgI is 8.5 ´ 10–17 at 25 °C. Calculate the molar solubility of AgI in 0.0045 M KI(aq) at 25 °C. a. 1.9 ´ 10–14 mol/L b. 3.8 ´ 10–12 mol/L c. 9.2 ´ 10–9 mol/L d. 1.4 ´ 10–7 mol/L e. 2.0 ´ 10–6 mol/L 11. What is the molar solubility of Fe(OH)3(s) in a solution that is buffered at pH 2.50 at 25 °C? The Ksp of Fe(OH)3 is 6.3 ´ 10–38 at 25 °C. a. 6.9 ´ 10–28 mol/L b. 2.0 ´ 10–26 mol/L c. 1.3 ´ 10–13 mol/L d. 2.0 ´ 10–3 mol/L e. 5.0 ´ 102 mol/L 12. The concentration of Pb2+ in an aqueous solution is 5.5 ´ 10–3 M. What concentration of SO42– is required to begin precipitating PbSO4? The Ksp of PbSO4 is 2.5 ´ 10–8. a. 1.4 ´ 10–10 M b. 4.5 ´ 10–6 M c. 1.6 ´ 10–4 M d. 8.3 ´ 10–4 M e. 2.9 ´ 10–2 M 13. An aqueous solution contains 0.010 M Br– and 0.010 M I–. If Ag+ is added until AgBr(s) just begins to precipitate, what are the concentrations of Ag+ and I–? (Ksp of AgBr = 5.4 ´ 10–13, Ksp of AgI = 8.5 ´ 10–17) a. [Ag+] = 5.4 ´ 10–11 M, [I–] = 1.0 ´ 10–2 M b. [Ag+] = 8.5 ´ 10–15 M, [I–] = 1.0 ´ 10–2 M c. [Ag+] = 5.4 ´ 10–11 M, [I–] = 1.6 ´ 10–6 M d. [Ag+] = 8.5 ´ 10–15 M, [I–] = 6.4 ´ 101 M e. [Ag+] = 8.5 ´ 10–15 M, [I–] = 1.6 ´ 10–6 M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂) is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H) and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 ´ 10^–5)

a.	2.52
b.	4.23
c.	4.44
d.	4.64
e.	4.74

____ 5. If 0.50 L of a buffer containing 1.0 mol H₂PO₄^- and 1.0 mol HPO₄²^- is diluted to a volume of 5.0 L, the pH

a.	increases by 1.
b.	decreases by 1.
c.	increases by 10.
d.	decreases by 10.
e.	remains unchanged.

____ 6. Which of the following conditions is/are met at the equivalence point of the titration of a monoprotic weak base with a strong acid?

	1.	The moles of acid added from the buret equals the initial moles of weak base.
	2.	The volume of acid added from the buret must equal the volume of base titrated.
	3.	The pH of the solution is less than 7.00.

a.	1 only
b.	2 only
c.	3 only
d.	1 and 3
e.	2 and 3

____ 7. A volume of 25.0 mL of 0.100 M C₆H₅CO₂H(aq) is titrated with 0.100 M NaOH(aq). What is the pH after the addition of 12.5 mL of NaOH? (K_a of benzoic acid = 6.3 ´ 10^–5)

a.	2.60
b.	4.20
c.	5.40
d.	7.00
e.	8.60

____ 8. A 50.0 mL sample of 0.155 M HNO₂(aq) is titrated with 0.100 M NaOH(aq). What is the pH of a solution after the addition of 25.0 mL of NaOH? (K_a of HNO₂ = 4.5 ´ 10^–4)

a.	3.02
b.	3.22
c.	3.67
d.	3.86
e.	4.05

____ 9. The K_sp of BaSO₄ is 1.1 ´ 10^–10 at 25 °C. What mass of BaSO₄ (molar mass = 233.4 g/mol) will dissolve in 1.0 L of water at 25 °C?

a.	2.6 ´ 10^-⁸ g
b.	4.5 ´ 10^-⁸ g
c.	1.0 ´ 10^-⁵ g
d.	1.6 ´ 10^-⁴ g
e.	2.4 ´ 10^-³ g

____ 10. The K_sp of AgI is 8.5 ´ 10^–17 at 25 °C. Calculate the molar solubility of AgI in 0.0045 M KI(aq) at 25 °C.

a.	1.9 ´ 10^–14 mol/L
b.	3.8 ´ 10^–12 mol/L
c.	9.2 ´ 10^–9 mol/L
d.	1.4 ´ 10^–7 mol/L
e.	2.0 ´ 10^–6 mol/L

____ 11. What is the molar solubility of Fe(OH)₃(s) in a solution that is buffered at pH 2.50 at 25 °C? The K_sp of Fe(OH)₃ is 6.3 ´ 10^–38 at 25 °C.

a.	6.9 ´ 10^–28 mol/L
b.	2.0 ´ 10^–26 mol/L
c.	1.3 ´ 10^–13 mol/L
d.	2.0 ´ 10^–3 mol/L
e.	5.0 ´ 10² mol/L

____ 12. The concentration of Pb²⁺ in an aqueous solution is 5.5 ´ 10^–3 M. What concentration of SO₄^2– is required to begin precipitating PbSO₄? The K_sp of PbSO₄ is 2.5 ´ 10^–8.

a.	1.4 ´ 10^–10 M
b.	4.5 ´ 10^–6 M
c.	1.6 ´ 10^–4 M
d.	8.3 ´ 10^–4 M
e.	2.9 ´ 10^–2 M

____ 13. An aqueous solution contains 0.010 M Br^– and 0.010 M I^–. If Ag⁺ is added until AgBr(s) just begins to precipitate, what are the concentrations of Ag⁺ and I^–? (K_sp of AgBr = 5.4 ´ 10^–13, K_sp of AgI = 8.5 ´ 10^–17)

a.	[Ag⁺] = 5.4 ´ 10^–11 M, [I^–] = 1.0 ´ 10^–2 M
b.	[Ag⁺] = 8.5 ´ 10^–15 M, [I^–] = 1.0 ´ 10^–2 M
c.	[Ag⁺] = 5.4 ´ 10^–11 M, [I^–] = 1.6 ´ 10^–6 M
d.	[Ag⁺] = 8.5 ´ 10^–15 M, [I^–] = 6.4 ´ 10¹ M
e.	[Ag⁺] = 8.5 ´ 10^–15 M, [I^–] = 1.6 ´ 10^–6 M

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