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] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

A) 3.0 * 10-14 M B) 5.0 * 10-14 M C) 7.0 * 10-14 M D) 9.0 * 10-14 M E) None of the above A) 3.0 * 10-14 M B) 5.0 * 10-14 M C) 7.0 * 10-14 M D) 9.0 * 10-14 M E) None of the above

Calculate the molar solubility of Mg(OH)2 in a solution with pH = 12.20.(Ksp (Mg(OH)2 = 1.2 x 10-11)

A) 4.8 x 10-8 M B) 7.6 x 10-10 M C) 3.5 x 10-6 M D) 1.4 x 10-4 M E) 2.4 x 10-6 M A) 4.8 x 10-8 M B) 7.6 x 10-10 M C) 3.5 x 10-6 M D) 1.4 x 10-4 M E) 2.4 x 10-6 M

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10-3 M MgCl2 are added to 300. mL of 1.4 * 10-2 M NaF? [Ksp (MgF2) = 6.9 * 10-9]

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

Will a precipitate (ppt) form when 20.0 mL of 1.1 * 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 * 10-4 M Na2CO3

A) Yes, the ppt is Ba(NO3 )2 B) Yes, the ppt is NaNO3 C) Yes, the ppt is BaCO3 D) Yes, the ppt is Na2CO3 E) No, a precipitate will not form A) Yes, the ppt is Ba(NO3 )2 B) Yes, the ppt is NaNO3 C) Yes, the ppt is BaCO3 D) Yes, the ppt is Na2CO3 E) No, a precipitate will not form

Will a precipitate (ppt) form when 300. mL of 2.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

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

At 25$\circ$C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the percentage ionization of a 0.150 M solution of ammonia at 25 $\circ$C.

A) 0.2% B) 0.9% C) 1.1% D) 2.5% E) None of the above A) 0.2% B) 0.9% C) 1.1% D) 2.5% E) None of the above

Exam 16: Acid-Base Equilibria and Solubility Equilibria

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] Calculate the Ag⁺ concentration when PbI₂ just begins to precipitate.

(Multiple Choice)

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Question 21

The equation shown here is the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8): HCO₃^- + OH^- $\rarr$ CO₃^2- + H₂O

(True/False)

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Question 22

At 25 ^$\circ$C, the base ionization constant for NH₃ is 1.8 * 10^-5. If 0.0800 mole of solid magnesium chloride is dissolved in a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100. ml of 0.150 M ammonia, a precipitate of magnesium hydroxide will form. (Assume the volume of the solution is unchanged. The solubility product constant for magnesium hydroxide is 1.5 * 10^-11.)

(True/False)

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Question 23

The net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO₂/HNO₂ buffer is correctly shown here: H⁺ + NO₂^- $\rarr$ HNO₂

(True/False)

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Question 24

There will be no Fe(OH)₃ precipitate in a buffer solution that is 0.60 M CH₃COOH and 0.10 M CH₃COONa, if the solution is also made to be 0.001 M in Fe³⁺. For Fe(OH)₃, K_sp = 6.8 * 10^-36.

(True/False)

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Question 25

The solubility product for calcium phosphate is K_sp = 1.3 * 10^-26. What is the molar solubility of calcium phosphate

(Multiple Choice)

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Question 26

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH₃ (K_b = 1.8 * 10^-5).

(Multiple Choice)

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Question 27

550. mL of a 0.40M solution of NaOH is titrated with 0.25 M HCl. Calculate the pH of the solution after 650. mL of the HCl has been added.

(Multiple Choice)

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Question 28

Calculate the molar solubility of Mg(OH)₂ in a solution with pH = 12.20.(K_sp (Mg(OH)₂ = 1.2 x 10^-11)

(Multiple Choice)

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Question 29

500. mL of a solution containing 1.5 M NH₄Cl(aq) is mixed with 500. mL of a solution containing 0.50M of NaOH(aq). What is the pH of the final solution (K_b(NH₃) = 1.8 x 10^-5)

(Multiple Choice)

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Question 30

The net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO₂/HNO₂ buffer is correctly shown here: OH^- + HNO₂ $\rarr$ NO₂^- + H₂O

(True/False)

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Question 31

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

(Multiple Choice)

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Question 32

What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, K_a = 1.7 * 10^-4.)

(Multiple Choice)

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Question 33

Will a precipitate (ppt) form when 20.0 mL of 1.1 * 10^-3 M Ba(NO₃)₂ are added to 80.0 mL of 8.4 * 10^-4 M Na₂CO₃

(Multiple Choice)

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Question 34

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa. (K_a = 1.7 * 10^-4)

(Multiple Choice)

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Question 35

Will a precipitate (ppt) form when 300. mL of 2.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

(Multiple Choice)

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Question 36

At 25^$\circ$C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the percentage ionization of a 0.150 M solution of ammonia at 25 ^$\circ$C.

(Multiple Choice)

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Question 37

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 $\pm$ 0.02. What molar ratio of CH₃COOH to CH₃COONa should be used

(Multiple Choice)

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Question 38

Which of the following would decrease the K_sp for PbI₂

(Multiple Choice)

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Question 39

35.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pH of the solution after 40.00 mL of the NaOH has been added

(Multiple Choice)

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Question 40

Showing 21 - 40 of 145

Exam 16: Acid-Base Equilibria and Solubility Equilibria

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] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

The equation shown here is the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 * 10-7, Ka2 = 2.4 * 10-8): HCO3- + OH- →\rarr→ CO32- + H2O

The net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer is correctly shown here: H+ + NO2- →\rarr→ HNO2

There will be no Fe(OH)3 precipitate in a buffer solution that is 0.60 M CH3COOH and 0.10 M CH3COONa, if the solution is also made to be 0.001 M in Fe3+. For Fe(OH)3, Ksp = 6.8 * 10-36.

The solubility product for calcium phosphate is Ksp = 1.3 * 10-26. What is the molar solubility of calcium phosphate

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 * 10-5).

550. mL of a 0.40M solution of NaOH is titrated with 0.25 M HCl. Calculate the pH of the solution after 650. mL of the HCl has been added.

Calculate the molar solubility of Mg(OH)2 in a solution with pH = 12.20.(Ksp (Mg(OH)2 = 1.2 x 10-11)

500. mL of a solution containing 1.5 M NH4Cl(aq) is mixed with 500. mL of a solution containing 0.50M of NaOH(aq). What is the pH of the final solution (Kb(NH3) = 1.8 x 10-5)

The net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO2/HNO2 buffer is correctly shown here: OH- + HNO2 →\rarr→ NO2- + H2O

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10-3 M MgCl2 are added to 300. mL of 1.4 * 10-2 M NaF? [Ksp (MgF2) = 6.9 * 10-9]

What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, Ka = 1.7 * 10-4.)

Will a precipitate (ppt) form when 20.0 mL of 1.1 * 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 * 10-4 M Na2CO3

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa. (Ka = 1.7 * 10-4)

Will a precipitate (ppt) form when 300. mL of 2.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

At 25 ∘\circ∘ C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the percentage ionization of a 0.150 M solution of ammonia at 25 ∘\circ∘ C.

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 ±\pm± 0.02. What molar ratio of CH3COOH to CH3COONa should be used

Which of the following would decrease the Ksp for PbI2

35.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pH of the solution after 40.00 mL of the NaOH has been added

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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] Calculate the Ag⁺ concentration when PbI₂ just begins to precipitate.

The equation shown here is the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8): HCO₃^- + OH^- $\rarr$ CO₃^2- + H₂O

The net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO₂/HNO₂ buffer is correctly shown here: H⁺ + NO₂^- $\rarr$ HNO₂

There will be no Fe(OH)₃ precipitate in a buffer solution that is 0.60 M CH₃COOH and 0.10 M CH₃COONa, if the solution is also made to be 0.001 M in Fe³⁺. For Fe(OH)₃, K_sp = 6.8 * 10^-36.

The solubility product for calcium phosphate is K_sp = 1.3 * 10^-26. What is the molar solubility of calcium phosphate

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH₃ (K_b = 1.8 * 10^-5).

Calculate the molar solubility of Mg(OH)₂ in a solution with pH = 12.20.(K_sp (Mg(OH)₂ = 1.2 x 10^-11)

500. mL of a solution containing 1.5 M NH₄Cl(aq) is mixed with 500. mL of a solution containing 0.50M of NaOH(aq). What is the pH of the final solution (K_b(NH₃) = 1.8 x 10^-5)

The net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO₂/HNO₂ buffer is correctly shown here: OH^- + HNO₂ $\rarr$ NO₂^- + H₂O

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, K_a = 1.7 * 10^-4.)

Will a precipitate (ppt) form when 20.0 mL of 1.1 * 10^-3 M Ba(NO₃)₂ are added to 80.0 mL of 8.4 * 10^-4 M Na₂CO₃

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa. (K_a = 1.7 * 10^-4)

Will a precipitate (ppt) form when 300. mL of 2.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

At 25^$\circ$C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the percentage ionization of a 0.150 M solution of ammonia at 25 ^$\circ$C.

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 $\pm$ 0.02. What molar ratio of CH₃COOH to CH₃COONa should be used

Which of the following would decrease the K_sp for PbI₂