Question 1

The Ksp of Fe(OH) 3(s) is 3 × 10−39.What concentration of Fe3+ can exist in solution at pH 3.0?

Accepted Answer

A)   3 × 10−4 M
B)   3 × 10−6 M
C)   3 × 10−21 M
D)   3 × 10−24 M
E)   3 × 10−30 M

Question 2

The Ksp of aluminum hydroxide,Al(OH) 3,is 2 × 10−31.What pH is required to limit the Al3+ concentration to less than or equal to 1 × 10−10 M?

Accepted Answer

A)   3.6
B)   6.4
C)   7.1
D)   7.8
E)   11.5

Question 3

What volume of water is needed to completely dissolve 1.0 g of Ag2CrO4 (Ksp = 8.0 × 10−12,MM = 331.8 g/mol) ?

Accepted Answer

A)   0.94 L
B)   1.1 L
C)   1.7 L
D)   24 L
E)   2.6 × 105 L

Question 4

A saturated solution of lead(II) sulfate can be prepared by diluting 0.0101 g of PbSO4 to 250 mL.What is the Ksp of lead(II) sulfate?

Accepted Answer

A)   8.3 × 10−12
B)   1.6 × 10−9
C)   1.8 × 10−8
D)   4.5 × 10−8
E)   8.4 × 10−7

Question 5

For Mg(OH) 2,Ksp = 6 × 10−12.What will occur if 1.0 L of 0.010 M Mg(NO3) 2 is prepared at pH 10.00?

Accepted Answer

A)   Q > Ksp.A precipitate will form.
B)   Ksp > Q.A precipitate will form.
C)   Q = Ksp.No precipitate will form.
D)   Q > Ksp.No precipitate will form.
E)   Ksp > Q.No precipitate will form.

Question 6

The solubility of BaCrO4(s) in water is 3.7 milligrams in 1.0 L at 25°C.What is the value of Ksp for BaCrO4?

Accepted Answer

A)   2.1 × 10-10
B)   8.6 × 10-10
C)   1.4 × 10-5
D)   1.5 × 10-5
E)   2.9 × 10-5

Question 7

The Ksp of calcium iodate is 7.1 × 10−7.What is the concentration of Ca2+ in equilibrium with Ca(IO3) 2(s) if [IO3−] = 3.3 × 10−2 M?

Accepted Answer

A)   3.3 × 10−7 M
B)   2.2 × 10−5 M
C)   8.1 × 10−5 M
D)   6.5 × 10−4 M
E)   7.1 × 10−3 M

Question 8

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?

Accepted Answer

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

Question 9

What is the net ionic equation for the reaction of KCl with a strong base?

Accepted Answer

A)   KCl(s) + OH−(aq) → KOH(aq) + Cl−(aq) 
B)   KCl(aq) + OH−(aq) → KOH(aq) + Cl−(aq) 
C)   K+(aq) + OH−(aq) → KOH(s) 
D)   Cl−(aq) + OH−(aq) → HOCl(aq) 
E)   No reaction will occur.

Question 10

What is the concentration of Ag+ in a saturated solution of Ag2CrO4 if 
Ksp = 1 × 10−12?

Accepted Answer

A)   1 × 10−12 M
B)   5 × 10−5 M
C)   6 × 10−5 M
D)   1 × 10−4 M
E)   2 × 10−4 M

Question 11

Consider the equilibrium of Ca(OH) 2(s) in water. Ca(OH) 2(s)   ? Ca2+(aq) + 2OH?(aq) , What is the effect of raising the pH of the solution?

Accepted Answer

A)   Ca2+(aq) is reduced to Ca(s) .
B)   The concentration of hydronium ion increases.
C)   The concentration of Ca2+ increases as Ca(OH) 2 dissolves.
D)   Ca(OH) 2(s) precipitates until equilibrium is reestablished.
E)   Hydroxide ion is reduced to H2(g) .

Question 12

The formation constant for Ag(CN) 2−(aq) is 2 × 1020.At what cyanide ion concentration is [Ag+] = [ Ag(CN) 2−]?

Accepted Answer

A)   3 × 10−41 M
B)   5 × 10−21 M
C)   7 × 10−11 M
D)   6 × 10−6 M
E)   1 × 1010 M C

Question 13

What is the chemical equation that describes the dissolution of calcium iodate in water?

Accepted Answer

A)   CaI2(s)   ? Ca2+(aq) + 2I?(aq) 
B)   Ca2+(aq) + IO3?(aq)   ? CaIO3(s) 
C)   Ca(IO3) 2(s)   ? Ca(s) + I2(aq) + 3O2(g) 
D)   Ca(IO3) 2(s)   ? Ca2+(aq) + 2IO3?(aq) 
E)   Ca(IO3) 2(s)   ? CaI2(aq) + 3O2(g)

Question 14

What is the water solubility of PbI2 (Ksp = 8.4 × 10−9,MM = 461 g/mol) in moles per liter?

Accepted Answer

A)   8.4 × 10−9 M
B)   1.9 × 10−7 M
C)   9.1 × 10−5 M
D)   1.3 × 10−3 M
E)   2.0 × 10−3 M

Question 15

A solution containing an unknown metal ion is analyzed by qualitative analysis.Addition of chloride has no effect on the solution.Addition of H2S at pH 0.5 results in a precipitate.What group of cations is present?

Accepted Answer

A)   Group I
B)   Group II
C)   Group III
D)   Group IV
E)   Group V

Question 16

What is the water solubility of BaF2(s) in 0.033 M KF(aq) at 25°C? The Ksp of BaF2 is 1.8 × 10-7 at 25°C.

Accepted Answer

A)   2.7 × 10-6 M
B)   5.5 × 10-6 M
C)   4.1 × 10-5 M
D)   1.1 × 10-4 M
E)   1.7 × 10-4 M E

Question 17

For AgCl,Ksp = 1.8 × 10−10.What will occur if 250 mL of 1.5 × 10−3 M NaCl is mixed with 250 mL of 2.0 × 10−7M AgNO3?

Accepted Answer

A)   Q > Ksp.A precipitate will form.
B)   Ksp > Q.A precipitate will form.
C)   Q = Ksp.No precipitate will form.
D)   Q > Ksp.No precipitate will form.
E)   Ksp > Q.No precipitate will form.

Question 18

Consider the reaction Cu(OH) 2(s) + 4NH3(aq)   ? Cu(NH3) 42+(aq) + 2OH?(aq) 
K = 4 × 10?7
If the Kf for Cu(NH3) 42+ is 1 × 1012,what is the value of Ksp for Cu(OH) 2?

Accepted Answer

A)   4 × 10?19
B)   2 × 10?13
C)   5 × 10?12
D)   4 × 10?7
E)   4 × 105 A

Question 19

Which of the following equations is the solubility product of Cu(II) hydroxide,Cu(OH) 2?

Accepted Answer

A)    Ksp=[Cu(OH) 2][Cu2+][OH−]2K_{\mathrm{sp}}=\frac{\left[\mathrm{Cu}(\mathrm{OH}) _{2}\right]}{\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}}Ksp​=[Cu2+][OH−]2[Cu(OH) 2​]​ 
B)    Ksp=[Cu2+][OH−]2[Cu(OH) 2]K_{\mathrm{sp}}=\frac{\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}}{\left[\mathrm{Cu}(\mathrm{OH}) _{2}\right]}Ksp​=[Cu(OH) 2​][Cu2+][OH−]2​ 
C)    Ksp=[Cu2+][OH−]K_{\mathrm{sp}}=\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]Ksp​=[Cu2+][OH−] 
D)    Ksp=[Cu2+]2[OH−]K_{s p}=\left[\mathrm{Cu}^{2+}\right]^{2}\left[\mathrm{OH}^{-}\right]Ksp​=[Cu2+]2[OH−] 
E)    Ksp=[Cu2+][OH−]2K_{\mathrm{sp}}=\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}Ksp​=[Cu2+][OH−]2

Question 20

Which of the boxes below represents solid MX2 in equilibrium with M2+ (squares) and X− (circles) ?

Accepted Answer

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Exam 15: Complex Ion and Precipitation Equilibria

The Ksp of Fe(OH) 3(s) is 3 × 10−39.What concentration of Fe3+ can exist in solution at pH 3.0?

Correct AnswerverifiedShow Answer

The Ksp of aluminum hydroxide,Al(OH) 3,is 2 × 10−31.What pH is required to limit the Al3+ concentration to less than or equal to 1 × 10−10 M?

Correct AnswerverifiedShow Answer

What volume of water is needed to completely dissolve 1.0 g of Ag2CrO4 (Ksp = 8.0 × 10−12,MM = 331.8 g/mol) ?

Correct AnswerverifiedShow Answer

A saturated solution of lead(II) sulfate can be prepared by diluting 0.0101 g of PbSO4 to 250 mL.What is the Ksp of lead(II) sulfate?

Correct AnswerverifiedShow Answer

For Mg(OH) 2,Ksp = 6 × 10−12.What will occur if 1.0 L of 0.010 M Mg(NO3) 2 is prepared at pH 10.00?

Correct AnswerverifiedShow Answer

The solubility of BaCrO4(s) in water is 3.7 milligrams in 1.0 L at 25°C.What is the value of Ksp for BaCrO4?

Correct AnswerverifiedShow Answer

The Ksp of calcium iodate is 7.1 × 10−7.What is the concentration of Ca2+ in equilibrium with Ca(IO3) 2(s) if [IO3−] = 3.3 × 10−2 M?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

What is the net ionic equation for the reaction of KCl with a strong base?

Correct AnswerverifiedShow Answer

What is the concentration of Ag+ in a saturated solution of Ag2CrO4 if Ksp = 1 × 10−12?

Correct AnswerverifiedShow Answer

Consider the equilibrium of Ca(OH) 2(s) in water. Ca(OH) 2(s) ? Ca2+(aq) + 2OH?(aq) , What is the effect of raising the pH of the solution?

Correct AnswerverifiedShow Answer

The formation constant for Ag(CN) 2−(aq) is 2 × 1020.At what cyanide ion concentration is [Ag+] = [ Ag(CN) 2−]?

Correct AnswerverifiedC

What is the chemical equation that describes the dissolution of calcium iodate in water?

Correct AnswerverifiedShow Answer

What is the water solubility of PbI2 (Ksp = 8.4 × 10−9,MM = 461 g/mol) in moles per liter?

Correct AnswerverifiedShow Answer

A solution containing an unknown metal ion is analyzed by qualitative analysis.Addition of chloride has no effect on the solution.Addition of H2S at pH 0.5 results in a precipitate.What group of cations is present?

Correct AnswerverifiedShow Answer

What is the water solubility of BaF2(s) in 0.033 M KF(aq) at 25°C? The Ksp of BaF2 is 1.8 × 10-7 at 25°C.

Correct AnswerverifiedE

For AgCl,Ksp = 1.8 × 10−10.What will occur if 250 mL of 1.5 × 10−3 M NaCl is mixed with 250 mL of 2.0 × 10−7M AgNO3?

Correct AnswerverifiedShow Answer

Consider the reaction Cu(OH) 2(s) + 4NH3(aq) ? Cu(NH3) 42+(aq) + 2OH?(aq) K = 4 × 10?7 If the Kf for Cu(NH3) 42+ is 1 × 1012,what is the value of Ksp for Cu(OH) 2?

Correct AnswerverifiedA

Which of the following equations is the solubility product of Cu(II) hydroxide,Cu(OH) 2?

Correct AnswerverifiedShow Answer

Which of the boxes below represents solid MX2 in equilibrium with M2+ (squares) and X− (circles) ?

Correct AnswerverifiedShow Answer

The K_sp of Fe(OH) ₃(s) is 3 × 10−³⁹.What concentration of Fe³⁺ can exist in solution at pH 3.0?

Correct Answer
verified

The K_sp of aluminum hydroxide,Al(OH) ₃,is 2 × 10−³¹.What pH is required to limit the Al³⁺ concentration to less than or equal to 1 × 10−¹⁰ M?

Correct Answer
verified

What volume of water is needed to completely dissolve 1.0 g of Ag₂CrO₄ (K_sp = 8.0 × 10−¹²,MM = 331.8 g/mol) ?

Correct Answer
verified

A saturated solution of lead(II) sulfate can be prepared by diluting 0.0101 g of PbSO₄ to 250 mL.What is the K_sp of lead(II) sulfate?

Correct Answer
verified

For Mg(OH) ₂,K_sp = 6 × 10−¹².What will occur if 1.0 L of 0.010 M Mg(NO₃) ₂ is prepared at pH 10.00?

Correct Answer
verified

The solubility of BaCrO₄(s) in water is 3.7 milligrams in 1.0 L at 25°C.What is the value of K_sp for BaCrO₄?

Correct Answer
verified

The K_sp of calcium iodate is 7.1 × 10−⁷.What is the concentration of Ca²⁺ in equilibrium with Ca(IO₃) ₂(s) if [IO₃−] = 3.3 × 10−² M?

Correct Answer
verified

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?

Correct Answer
verified

Correct Answer
verified

What is the concentration of Ag⁺ in a saturated solution of Ag₂CrO₄ if K_sp = 1 × 10−¹²?

Correct Answer
verified

Consider the equilibrium of Ca(OH) ₂(s) in water. Ca(OH) ₂(s) ? Ca²⁺(aq) + 2OH?(aq) , What is the effect of raising the pH of the solution?

Correct Answer
verified

The formation constant for Ag(CN) ₂−(aq) is 2 × 10²⁰.At what cyanide ion concentration is [Ag⁺] = [ Ag(CN) ₂−]?

Correct Answer
verified
C

Correct Answer
verified

What is the water solubility of PbI₂ (K_sp = 8.4 × 10−⁹,MM = 461 g/mol) in moles per liter?

Correct Answer
verified

A solution containing an unknown metal ion is analyzed by qualitative analysis.Addition of chloride has no effect on the solution.Addition of H₂S at pH 0.5 results in a precipitate.What group of cations is present?

Correct Answer
verified

What is the water solubility of BaF₂(s) in 0.033 M KF(aq) at 25°C? The K_sp of BaF₂ is 1.8 × 10^-7 at 25°C.

Correct Answer
verified
E

For AgCl,K_sp = 1.8 × 10−¹⁰.What will occur if 250 mL of 1.5 × 10−³ M NaCl is mixed with 250 mL of 2.0 × 10−⁷M AgNO₃?

Correct Answer
verified

Consider the reaction Cu(OH) ₂(s) + 4NH₃(aq) ? Cu(NH₃) ₄²⁺(aq) + 2OH?(aq) K = 4 × 10?⁷ If the K_f for Cu(NH₃) ₄²⁺ is 1 × 10¹²,what is the value of K_sp for Cu(OH) ₂?

Correct Answer
verified
A

Which of the following equations is the solubility product of Cu(II) hydroxide,Cu(OH) ₂?

Correct Answer
verified

Which of the boxes below represents solid MX₂ in equilibrium with M²⁺ (squares) and X− (circles) ?

Correct Answer
verified