Question 1

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

Accepted Answer

A) 0.050 M H3PO4 and 0.050M HCl 
B) 0.050M H3PO4 and 0.025 M HCl 
C) 0.050M NaH2PO4 and 0.025M NaOH 
D) 0.050M Na3PO4 and 0.050M M NaOH 
E) 0.050M Na3PO4 and 0.025M NaOH 
A) 0.050 M H3PO4 and 0.050M HCl 
B) 0.050M H3PO4 and 0.025 M HCl 
C) 0.050M NaH2PO4 and 0.025M NaOH 
D) 0.050M Na3PO4 and 0.050M M NaOH 
E) 0.050M Na3PO4 and 0.025M NaOH

Question 2

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.

Accepted Answer

Prepare a solution h

Question 3

The molar solubility of manganese(II)carbonate is 4.2 × 10-6 M.What is Ksp for this compound?

Accepted Answer

A) 4.2 × 10-6 
B) 8.4 × 10-6 
C) 3.0 × 10-16 
D) 1.8 × 10-11 
E) 2.0 × 10-3 
A) 4.2 × 10-6 
B) 8.4 × 10-6 
C) 3.0 × 10-16 
D) 1.8 × 10-11 
E) 2.0 × 10-3

Question 4

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution?

Accepted Answer

A) H+ + H2O $\rarr$ H3O+ 
B) H+ + OCl- $\rarr$ HOCl 
C) HOCl $\rarr$ H+ + OCl- 
D) H+ + HOCl $\rarr$H2OCl+ 
E) HCl + HOCl $\rarr$H2O + Cl2 
A) H+ + H2O $\rarr$ H3O+ 
B) H+ + OCl- $\rarr$ HOCl 
C) HOCl $\rarr$ H+ + OCl- 
D) H+ + HOCl $\rarr$H2OCl+ 
E) HCl + HOCl $\rarr$H2O + Cl2

Question 5

The concentration of Mg2+ in seawater is 5.0 × 10-2 M.What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation? (For Mg(OH)2, Ksp = 1.2 × 10-11.)

Accepted Answer

Question 6

Calculate the pH of the solution resulting from the addition of 75.0 mL of 0.15 M KOH to 35.0 mL of 0.20 M HCN (Ka (HCN)= 4.9 × 10-10).

Accepted Answer

A) 9.31 
B) 9.18 
C) 9.52 
D) 11.63 
E) 12.59 
A) 9.31 
B) 9.18 
C) 9.52 
D) 11.63 
E) 12.59

Question 7

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

Accepted Answer

Question 8

Calculate the pH of the solution resulting from the addition of 25.0 mL of 0.20 M HCl to 50.0 mL of 0.10 M aniline (C6H5NH2).Kb (C6H5NH2)= 3.8 x 10-10

Accepted Answer

A) 9.42 
B) 9.12 
C) 7.00 
D) 2.30 
E) 2.88 
A) 9.42 
B) 9.12 
C) 7.00 
D) 2.30 
E) 2.88

Question 9

NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+.The Ksp's for CuCl, AgCl, and AuCl are 1.9 × 10-7, 1.8 × 10-10, and 2.0 × 10-13, respectively.Which compound will precipitate first?

Accepted Answer

Question 10

Calculate the silver ion concentration in a saturated solution of silver(I)sulfate (Ksp = 1.4 × 10-5).

Accepted Answer

A) 1.5 × 10-2 M 
B) 2.4 × 10-2 M 
C) 3.0 × 10-2 M 
D) 1.4 × 10-5 M 
E) None of the above. 
A) 1.5 × 10-2 M 
B) 2.4 × 10-2 M 
C) 3.0 × 10-2 M 
D) 1.4 × 10-5 M 
E) None of the above.

Question 11

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 12

The solubility of a salt increases as its Ksp increases.

Accepted Answer

A) True 
 B)False

Question 13

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.(For MgF2 , Ksp = 6.9 × 10-9.)

Accepted Answer

A) 1.4 × 107 M 
B) 6.9 × 10-9 M 
C) 6.9 × 10-8 M 
D) 1.7 × 10-7 M 
E) 6.9 × 10-7 M 
A) 1.4 × 107 M 
B) 6.9 × 10-9 M 
C) 6.9 × 10-8 M 
D) 1.7 × 10-7 M 
E) 6.9 × 10-7 M

Question 14

Calculate the equilibrium constant Kc for the net reaction shown below.
AgI(s)+ 2NH3(aq)    
Ag(NH3)2+(aq)+ I-(aq)
For AgI, Ksp = 8.3 × 10-17; for Ag(NH3)2+, Kf = 1.5 × 107.

Accepted Answer

Question 15

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 × 10-8; Ksp (AgI)= 8.3 × 10-17] What compound will precipitate first?

Accepted Answer

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

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 18

The Ksp for silver(I)phosphate is 1.8 × 10-18.Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

Accepted Answer

A) 1.6 × 10-5 M 
B) 2.1 × 10-5 M 
C) 3.7 × 10-5 M 
D) 1.1 × 10-13 M 
E) 4.8 × 10-5 M 
A) 1.6 × 10-5 M 
B) 2.1 × 10-5 M 
C) 3.7 × 10-5 M 
D) 1.1 × 10-13 M 
E) 4.8 × 10-5 M

Question 19

Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with 0.25 M NaOH.(For CH3COOH, Ka= 1.8 × 10-5)

Accepted Answer

Question 20

Calculate the molar solubility of Fe(OH)2 in a solution with pH = 13.15. (Ksp Fe(OH)2 = 1.6 x 10-14)

Accepted Answer

A) 1.6 x 10-14 M 
B) 1.1 x 10-13 M 
C) 1.6 x 10-5 M 
D) 8.0 x 10-13 M 
E) 3.4 x 10-7 M 
A) 1.6 x 10-14 M 
B) 1.1 x 10-13 M 
C) 1.6 x 10-5 M 
D) 8.0 x 10-13 M 
E) 3.4 x 10-7 M

Exam 16: Acid-Base Equilibria and Solubility Equilibria

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

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.

The molar solubility of manganese(II)carbonate is 4.2 × 10-6 M.What is Ksp for this compound?

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution?

The concentration of Mg2+ in seawater is 5.0 × 10-2 M.What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation? (For Mg(OH)2, Ksp = 1.2 × 10-11.)

Calculate the pH of the solution resulting from the addition of 75.0 mL of 0.15 M KOH to 35.0 mL of 0.20 M HCN (Ka (HCN)= 4.9 × 10-10).

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

Calculate the pH of the solution resulting from the addition of 25.0 mL of 0.20 M HCl to 50.0 mL of 0.10 M aniline (C6H5NH2).Kb (C6H5NH2)= 3.8 x 10-10

NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+.The Ksp's for CuCl, AgCl, and AuCl are 1.9 × 10-7, 1.8 × 10-10, and 2.0 × 10-13, respectively.Which compound will precipitate first?

Calculate the silver ion concentration in a saturated solution of silver(I)sulfate (Ksp = 1.4 × 10-5).

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.

The solubility of a salt increases as its Ksp increases.

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.(For MgF2 , Ksp = 6.9 × 10-9.)

Calculate the equilibrium constant Kc for the net reaction shown below. AgI(s)+ 2NH3(aq) Ag(NH3)2+(aq)+ I-(aq) For AgI, Ksp = 8.3 × 10-17; for Ag(NH3)2+, Kf = 1.5 × 107.

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 × 10-8; Ksp (AgI)= 8.3 × 10-17] What compound will precipitate first?

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

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?

The Ksp for silver(I)phosphate is 1.8 × 10-18.Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with 0.25 M NaOH.(For CH3COOH, Ka= 1.8 × 10-5)

Calculate the molar solubility of Fe(OH)2 in a solution with pH = 13.15. (Ksp Fe(OH)2 = 1.6 x 10-14)

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The molar solubility of manganese(II)carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

The concentration of Mg²⁺ in seawater is 5.0 × 10^-2M.What hydroxide concentration is needed to remove 90% of the Mg²⁺ by precipitation? (For Mg(OH)₂, K_sp = 1.2 × 10^-11.)

Calculate the pH of the solution resulting from the addition of 75.0 mL of 0.15 M KOH to 35.0 mL of 0.20 M HCN (K_a (HCN)= 4.9 × 10^-10).

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

Calculate the pH of the solution resulting from the addition of 25.0 mL of 0.20 M HCl to 50.0 mL of 0.10 M aniline (C₆H₅NH₂).K_b(C₆H₅NH₂)= 3.8 x 10^-10

NaCl is added slowly to a solution that is 0.010 M each in Cu⁺, Ag⁺, and Au⁺.The K_sp's for CuCl, AgCl, and AuCl are 1.9 × 10^-7, 1.8 × 10^-10, and 2.0 × 10^-13, respectively.Which compound will precipitate first?

Calculate the silver ion concentration in a saturated solution of silver(I)sulfate (K_sp = 1.4 × 10^-5).

The solubility of a salt increases as its K_sp increases.

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.(For MgF₂ , K_sp = 6.9 × 10^-9.)

Calculate the equilibrium constant K_c for the net reaction shown below. AgI(s)+ 2NH₃(aq) Ag(NH₃)₂⁺(aq)+ I^-(aq) For AgI, K_sp = 8.3 × 10^-17; for Ag(NH₃)₂⁺, K_f = 1.5 × 10⁷.

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 × 10^-8; K_sp (AgI)= 8.3 × 10^-17] What compound will precipitate first?

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?

The K_sp for silver(I)phosphate is 1.8 × 10^-18.Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

Calculate the pH at the equivalence point for the titration of 0.25 M CH₃COOH with 0.25 M NaOH.(For CH₃COOH, K_a= 1.8 × 10^-5)

Calculate the molar solubility of Fe(OH)₂ in a solution with pH = 13.15. (K_sp Fe(OH)₂ = 1.6 x 10^-14)