Question 1

Calculate the molar solubility of silver carbonate. (Ksp (Ag2CO3 = 8.1 x 10-12))

Accepted Answer

A)  1.1 x 10-4 M 
B)  1.3 x 10-4 M 
C)  1.5 x 10-4 M 
D)  1.7 x 10-4 M 
E)  None of the above 
A)  1.1 x 10-4 M 
B)  1.3 x 10-4 M 
C)  1.5 x 10-4 M 
D)  1.7 x 10-4 M 
E)  None of the above

Question 2

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [Ka(HOCl) = 3.2 * 10-8]

Accepted Answer

A)  0.39 
B)  3.94 
C)  6.58 
D)  7.49 
E)  8.40 
A)  0.39 
B)  3.94 
C)  6.58 
D)  7.49 
E)  8.40

Question 3

Which response has both answers correct Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3?
[Ksp(Ag2CrO4) = 1.1 * 10-12] What is the concentration of the silver ion remaining in solution

Accepted Answer

A)  Yes, [Ag+] = 2.9 * 10-6 M 
B)  Yes, [Ag+] = 0.060 M 
C)  Yes, [Ag+] = 1.3 * 10-4 M 
D)  No, [Ag+] = 0.060 M 
E)  No, [Ag+] = 0.105 M 
A)  Yes, [Ag+] = 2.9 * 10-6 M 
B)  Yes, [Ag+] = 0.060 M 
C)  Yes, [Ag+] = 1.3 * 10-4 M 
D)  No, [Ag+] = 0.060 M 
E)  No, [Ag+] = 0.105 M

Question 4

A 50.0 mL sample of 2.0 * 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN)32- is 1.0 * 109. What is the copper(I) ion concentration in this system at equilibrium

Accepted Answer

A)  2.3 * 10-14 M 
B)  1.3 * 10-14 M 
C)  1.3 * 10-13 M 
D)  2.3 * 10-13 M 
E)  None of the above 
A)  2.3 * 10-14 M 
B)  1.3 * 10-14 M 
C)  1.3 * 10-13 M 
D)  2.3 * 10-13 M 
E)  None of the above

Question 5

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 
(Kb(NH3) = 1.8 * 10-5)

Accepted Answer

A)  7.6 g 
B)  2.4 g 
C)  5.4 g 
D)  11 g 
E)  3.3 g 
A)  7.6 g 
B)  2.4 g 
C)  5.4 g 
D)  11 g 
E)  3.3 g

Question 6

Will a precipitate (ppt) form when 300. mL of 5.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Accepted Answer

A)  Yes, the ppt is AgNO3(s) 
B)  Yes, the ppt is AgBr(s) 
C)  Yes, the ppt is NaBr(s) 
D)  Yes, the ppt is NaNO3(s) 
E)  No, a precipitate will not form 
A)  Yes, the ppt is AgNO3(s) 
B)  Yes, the ppt is AgBr(s) 
C)  Yes, the ppt is NaBr(s) 
D)  Yes, the ppt is NaNO3(s) 
E)  No, a precipitate will not form

Question 7

A sample of rainwater collected near a lead smelter is analyzed for acid content. Experiments show that a 100. mL sample of the rainwater is neutralized by 22.4 milliters of 0.0122 M NaOH. Assuming that the acid present is sulfurous acid, which resulted from the reaction of SO2 with water, what is the molarity of acid in the rainwater

Accepted Answer

A)  1.17 * 10-3 M 
B)  1.27 * 10-3 M 
C)  1.37 * 10-3 M 
D)  1.47 * 10-3 M 
E)  None of the above 
A)  1.17 * 10-3 M 
B)  1.27 * 10-3 M 
C)  1.37 * 10-3 M 
D)  1.47 * 10-3 M 
E)  None of the above

Question 8

The solubility of a salt increases as its Ksp increases.

Accepted Answer

A) True 
 B)False

Question 9

For PbCl2 (Ksp = 2.4 * 10-4), will a precipitate of PbCl2 form when 0.10 L of 3.0 * 10-2 M Pb(NO3)2 is added to 400 mL of 9.0 * 10-2 M NaCl

Accepted Answer

A) Yes, because Q > Ksp. 
B)  No, because Q sp. 
C)  No, because Q = Ksp 
D)  Yes, because Q sp. 
A) Yes, because Q > Ksp. 
B)  No, because Q sp. 
C)  No, because Q = Ksp 
D)  Yes, because Q sp.

Question 10

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH

Accepted Answer

A)  1.0 
B)  6.0 
C)  7.0 
D)  8.0 
E)  13.0 
A)  1.0 
B)  6.0 
C)  7.0 
D)  8.0 
E)  13.0

Question 11

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq) (Ksp (AgBr) = 7.7 x 10-13 ; Kf (Ag(NH3)2+) = 1.5 x 107.

Accepted Answer

A)  8.8 x 10-7 M 
B)  3.4 x 10-3 M 
C)  8.4 x 10-4 M 
D)  2.5 x 10-1 M 
E)  9.7 x 102 M 
A)  8.8 x 10-7 M 
B)  3.4 x 10-3 M 
C)  8.4 x 10-4 M 
D)  2.5 x 10-1 M 
E)  9.7 x 102 M

Question 12

The percent ionization of a weak acid HA is greater in a solution containing the salt NaA than it is in a solution of the weak acid only.

Accepted Answer

A) True 
 B)False

Question 13

Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 * 10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Accepted Answer

A)  green 
B)  red 
C)  blue 
D)  yellow 
E)  violet 
A)  green 
B)  red 
C)  blue 
D)  yellow 
E)  violet

Question 14

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF3 , Ksp = 6.6 * 10-11.)

Accepted Answer

A)  0.023 M 
B)  0.032 M 
C)  7.7 * 10-8 M 
D)  2.9 * 10-9 M 
E)  6.9 * 10-10 M 
A)  0.023 M 
B)  0.032 M 
C)  7.7 * 10-8 M 
D)  2.9 * 10-9 M 
E)  6.9 * 10-10 M

Question 15

The pH at the equivalence point of a titration may differ from 7.0 due to

Accepted Answer

A)  the initial concentration of the standard solution. 
B)  the indicator used. 
C)  the self-ionization of H2O. 
D)  the initial pH of the unknown. 
E)  hydrolysis of the salt formed. 
A)  the initial concentration of the standard solution. 
B)  the indicator used. 
C)  the self-ionization of H2O. 
D)  the initial pH of the unknown. 
E)  hydrolysis of the salt formed.

Question 16

Which of the following compounds is more soluble in a 0.10 M NaCN solution than in pure neutral water

Accepted Answer

A)  Mg(OH)2 
B)  Ca3(PO4)2 
C)  CaCO3 
D)  AgBr 
E)  NH4ClO4 
A)  Mg(OH)2 
B)  Ca3(PO4)2 
C)  CaCO3 
D)  AgBr 
E)  NH4ClO4

Question 17

500. mL of a solution containing 1.5 M NH3(aq) is mixed with 500. mL of a solution containing 0.50M of HCl(aq). What is the pH of the final solution
(Kb(NH3) = 1.8 x 10-5)

Accepted Answer

A)  9.16 
B)  9.36 
C)  9.56 
D)  9.76 
E)  None of the Above 
A)  9.16 
B)  9.36 
C)  9.56 
D)  9.76 
E)  None of the Above

Question 18

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution.[Ka(HCNO) = 2.0 * 10-4]

Accepted Answer

A)  0.97 
B)  3.10 
C)  4.40 
D)  3.70 
E)  4.30 
A)  0.97 
B)  3.10 
C)  4.40 
D)  3.70 
E)  4.30

Question 19

Which of the following is the most acidic solution

Accepted Answer

A)  0.10 M CH3COOH and 0.10 M CH3COONa 
B)  0.10 M CH3COOH 
C)  0.10 M HNO2 
D)  0.10 M HNO2 and 0.10 M NaNO2 
E)  0.10 M CH3COONa 
A)  0.10 M CH3COOH and 0.10 M CH3COONa 
B)  0.10 M CH3COOH 
C)  0.10 M HNO2 
D)  0.10 M HNO2 and 0.10 M NaNO2 
E)  0.10 M CH3COONa

Question 20

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Accepted Answer

A)  0.10 M NH3 and 0.10 M HCl 
B)  0.10 M NH4+ and 0.10 M KOH 
C)  0.20 M NH3 0.10 M KOH 
D)  0.20 M NH3 and 0.10 M HCl 
E)  0.20 M NH4+ and 0.10M HCl 
A)  0.10 M NH3 and 0.10 M HCl 
B)  0.10 M NH4+ and 0.10 M KOH 
C)  0.20 M NH3 0.10 M KOH 
D)  0.20 M NH3 and 0.10 M HCl 
E)  0.20 M NH4+ and 0.10M HCl

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Calculate the molar solubility of silver carbonate. (Ksp (Ag2CO3 = 8.1 x 10-12))

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [Ka(HOCl) = 3.2 * 10-8]

Which response has both answers correct Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 * 10-12] What is the concentration of the silver ion remaining in solution

A 50.0 mL sample of 2.0 * 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN)32- is 1.0 * 109. What is the copper(I) ion concentration in this system at equilibrium

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 (Kb(NH3) = 1.8 * 10-5)

Will a precipitate (ppt) form when 300. mL of 5.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

The solubility of a salt increases as its Ksp increases.

For PbCl2 (Ksp = 2.4 * 10-4), will a precipitate of PbCl2 form when 0.10 L of 3.0 * 10-2 M Pb(NO3)2 is added to 400 mL of 9.0 * 10-2 M NaCl

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq) (Ksp (AgBr) = 7.7 x 10-13 ; Kf (Ag(NH3)2+) = 1.5 x 107.

The percent ionization of a weak acid HA is greater in a solution containing the salt NaA than it is in a solution of the weak acid only.

Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 * 10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF3 , Ksp = 6.6 * 10-11.)

The pH at the equivalence point of a titration may differ from 7.0 due to

Which of the following compounds is more soluble in a 0.10 M NaCN solution than in pure neutral water

500. mL of a solution containing 1.5 M NH3(aq) is mixed with 500. mL of a solution containing 0.50M of HCl(aq). What is the pH of the final solution (Kb(NH3) = 1.8 x 10-5)

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution.[Ka(HCNO) = 2.0 * 10-4]

Which of the following is the most acidic solution

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

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Calculate the molar solubility of silver carbonate. (K_sp (Ag₂CO₃ = 8.1 x 10^-12))

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [K_a(HOCl) = 3.2 * 10^-8]

Which response has both answers correct Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄) = 1.1 * 10^-12] What is the concentration of the silver ion remaining in solution

A 50.0 mL sample of 2.0 * 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN)₃^2- is 1.0 * 10⁹. What is the copper(I) ion concentration in this system at equilibrium

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 (K_b(NH₃) = 1.8 * 10^-5)

Will a precipitate (ppt) form when 300. mL of 5.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

The solubility of a salt increases as its K_sp increases.

For PbCl₂ (K_sp = 2.4 * 10^-4), will a precipitate of PbCl₂ form when 0.10 L of 3.0 * 10^-2 M Pb(NO₃)₂ is added to 400 mL of 9.0 * 10^-2 M NaCl

Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq) (K_sp (AgBr) = 7.7 x 10^-13 ; K_f (Ag(NH₃)₂⁺) = 1.5 x 10⁷.

Methyl red is a common acid-base indicator. It has a K_a equal to 6.3 * 10^-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF₃ , K_sp = 6.6 * 10^-11.)

500. mL of a solution containing 1.5 M NH₃(aq) is mixed with 500. mL of a solution containing 0.50M of HCl(aq). What is the pH of the final solution (K_b(NH₃) = 1.8 x 10^-5)

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution.[K_a(HCNO) = 2.0 * 10^-4]