Suppose 50.00 mL of 2.0 $\times$ 10-6 M Fe(NO3)3 is added to 50.00 mL of 2.0 $\times$ 10-4 M KIO3.Which of the following statements is true? For Fe(IO3)3,Ksp = 1.0 $\times$ 10-14.

A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc sp. C) No precipitate forms because Qc sp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp. A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc sp. C) No precipitate forms because Qc sp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp.

What is the minimum mass of Cs2CO3 (molar mass = 325.821 g/mol)that must be added to 54.8 mL of a 5.0 $\times$ 10-4 M AgNO3 solution in order for precipitation to occur? The Ksp of Ag2CO3 is 8.6 $\times$ 10-12.Assume no volume change occurs upon addition of Cs2CO3.

A) 8.9 $\times$ 10-3 g B) 9.6 $\times$ 10-4 g C) 4.5 $\times$ 10-3 g D) 3.1 $\times$ 10-7 g E) 6.1 $\times$ 10-4 g A) 8.9 $\times$ 10-3 g B) 9.6 $\times$ 10-4 g C) 4.5 $\times$ 10-3 g D) 3.1 $\times$ 10-7 g E) 6.1 $\times$ 10-4 g

The Ksp of BaSO4 is 1.1 $\times$ 10-10 at 25 S1U1P1$\circ$S1S1P0C.What mass of BaSO4 (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25 S1U1P1$\circ$S1S1P0C?

A) 2.6 $\times$ 10-8 g B) 4.5 $\times$ 10-8 g C) 1.0 $\times$ 10-5 g D) 1.6 $\times$ 10-4 g E) 2.4 $\times$ 10-3 g A) 2.6 $\times$ 10-8 g B) 4.5 $\times$ 10-8 g C) 1.0 $\times$ 10-5 g D) 1.6 $\times$ 10-4 g E) 2.4 $\times$ 10-3 g

What is the molar solubility of Mn(OH)2(s)in a solution that is buffered at pH 8.00 at 25 S1U1P1$\circ$S1S1P0C? The Ksp of Mn(OH)2 is 1.9 $\times$ 10-13 at 25 S1U1P1$\circ$S1S1P0C.

A) 3.6 $\times$ 10-8 mol/L B) 1.9 $\times$ 10-7 mol/L C) 3.6 $\times$ 10-5 mol/L D) 1.9 $\times$ 10-1 mol/L E) 1.9 $\times$ 103 mol/L A) 3.6 $\times$ 10-8 mol/L B) 1.9 $\times$ 10-7 mol/L C) 3.6 $\times$ 10-5 mol/L D) 1.9 $\times$ 10-1 mol/L E) 1.9 $\times$ 103 mol/L

What is the pH of a buffer that results when 0.40 mol NaHCO2 is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (Ka of HCO2H = 1.8 $\times$ 10-4)

A) (-0.301) B) 3.05 C) 3.44 D) 3.74 E) 4.05 A) (-0.301) B) 3.05 C) 3.44 D) 3.74 E) 4.05

What is the minimum concentration of Cu2+ required to begin precipitating Cu(OH)2(s)in a solution buffered at pH 10.63? The Ksp of Cu(OH)2 is 2.6 $\times$ 10-19 and Kw = 1.01 $\times$ 10-14.

A) 2.1 $\times$ 10-4 M B) 1.1 $\times$ 10-8 M C) 6.1 $\times$ 10-16 M D) 1.4 $\times$ 10-12 M E) 2.3 $\times$ 10-21 M A) 2.1 $\times$ 10-4 M B) 1.1 $\times$ 10-8 M C) 6.1 $\times$ 10-16 M D) 1.4 $\times$ 10-12 M E) 2.3 $\times$ 10-21 M

An impure sample of sodium carbonate,Na2CO3,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na2CO3(aq) CO2(g)+ H2O( )+ 2 NaCl(aq) What is the percent of Na2CO3 in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na2CO3 is 106.0 g/mol.

A) 0.295% B) 15.7% C) 25.5% D) 51.1% E) 67.9% A) 0.295% B) 15.7% C) 25.5% D) 51.1% E) 67.9%

What is the pH of a solution made by combining 175 mL of 0.33 M NaC2H3O2 with 126 mL of 0.48 M HC2H3O2? The Ka of acetic acid is 1.75 $\times$ 10-5.

A) 4.74 B) 4.78 C) 5.79 D) 4.69 E) 5.24 A) 4.74 B) 4.78 C) 5.79 D) 4.69 E) 5.24

Exam 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria

What is the effect of adding NaOH(aq)to an aqueous solution of ammonia? 1)The pH of the solution will increase. 2)The concentration of NH₄⁺(aq)will decrease. 3)The concentration of NH₃(aq)will increase.

(Multiple Choice)

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Question 21

What is the solubility product expression for Fe(OH)₃?

(Multiple Choice)

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Question 22

What is the molar solubility of silver(I)bromide at 25°C? The solubility product constant for silver(I)bromide is 5.0 $\times$ 10^-13 at 25°C.

(Multiple Choice)

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Question 23

Suppose 50.00 mL of 2.0 $\times$ 10^-6 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 $\times$ 10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃)₃,K_sp = 1.0 $\times$ 10^-14.

(Multiple Choice)

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Question 24

What is the minimum mass of Cs₂CO₃ (molar mass = 325.821 g/mol)that must be added to 54.8 mL of a 5.0 $\times$ 10^-4 M AgNO₃ solution in order for precipitation to occur? The K_sp of Ag₂CO₃ is 8.6 $\times$ 10^-12.Assume no volume change occurs upon addition of Cs₂CO₃.

(Multiple Choice)

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Question 25

Given the following equilibrium constants, Cd(IO₃)₂ K_sp = Cd(NH₃)₄²⁺K_f = Determine K for the dissolution of the sparingly soluble salt Cd(IO₃)₂ in aqueous ammonia (shown below).Cd(IO₃)₂(s)+ 4NH₃(aq) Cd(NH₃)₄²⁺(aq)+ 2IO₃^-(aq)

(Multiple Choice)

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Question 26

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 $\times$ 10^-13,K_sp of AgI = 8.5 $\times$ 10^-17)

(Multiple Choice)

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Question 27

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.143 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What was the original concentration of the propionic acid?

(Multiple Choice)

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Question 28

The K_sp of BaSO₄ is 1.1 $\times$ 10^-10 at 25 ^$\circ$C.What mass of BaSO₄ (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25 ^$\circ$C?

(Multiple Choice)

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Question 29

What is the molar solubility of Mn(OH)₂(s)in a solution that is buffered at pH 8.00 at 25 ^$\circ$C? The K_sp of Mn(OH)₂ is 1.9 $\times$ 10^-13 at 25 ^$\circ$C.

(Multiple Choice)

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Question 30

What is the concentration of silver(I)ion in a saturated solution of silver(I)carbonate containing 0.0024 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 $\times$ 10^-12.

(Multiple Choice)

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Question 31

What is the pH of a buffer that results when 0.40 mol NaHCO₂ is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (K_a of HCO₂H = 1.8 $\times$ 10^-4)

(Multiple Choice)

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Question 32

What is the minimum concentration of Cu²⁺ required to begin precipitating Cu(OH)₂(s)in a solution buffered at pH 10.63? The K_sp of Cu(OH)₂ is 2.6 $\times$ 10^-19 and K_w = 1.01 $\times$ 10^-14.

(Multiple Choice)

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Question 33

Which acid-base combination is depicted by this titration curve? The dot on the curve is located at the titrant volume where the titration solution pH equals 7.

(Multiple Choice)

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Question 34

To make a buffer with a pH of 8.00,you should use a weak acid with a K_a close to _______.

(Essay)

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Question 35

An impure sample of sodium carbonate,Na₂CO₃,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na₂CO₃(aq) CO₂(g)+ H₂O( )+ 2 NaCl(aq) What is the percent of Na₂CO₃ in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na₂CO₃ is 106.0 g/mol.

(Multiple Choice)

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Question 36

How many moles of solid NaF would have to be added to 1.0 L of 2.39 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(K_a for HF = 7.2 $\times$ 10^-4)

(Multiple Choice)

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Question 37

A 50.00-mL solution of 0.0729 M chloroacetic acid (K_a = 1.4 $\times$ 10^-3)is titrated with a 0.0181 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (K_w = 1.00 $\times$ 10^-14)

(Multiple Choice)

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Question 38

What is the pH of a solution made by combining 175 mL of 0.33 M NaC₂H₃O₂ with 126 mL of 0.48 M HC₂H₃O₂? The K_a of acetic acid is 1.75 $\times$ 10^-5.

(Multiple Choice)

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Question 39

An acid-base equilibrium system is created by dissolving 0.50 mol CH₃CO₂H in water to a volume of 1.0 L.What is the effect of adding 0.50 mol CH₃CO₂^-(aq)to this solution? 1)The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2)Some CH₃CO₂H(aq)will ionize,increasing the concentration of CH₃CO₂^-(aq)and increasing the pH. 3)Some CH₃CO₂^-(aq)will react with H₃O⁺,increasing the concentration of CH₃CO₂H(aq)and reestablishing the solution equilibrium.

(Multiple Choice)

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Question 40

Showing 21 - 40 of 88

Exam 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria

What is the effect of adding NaOH(aq)to an aqueous solution of ammonia? 1)The pH of the solution will increase. 2)The concentration of NH4+(aq)will decrease. 3)The concentration of NH3(aq)will increase.

What is the solubility product expression for Fe(OH)3?

What is the molar solubility of silver(I)bromide at 25°C? The solubility product constant for silver(I)bromide is 5.0 ×\times× 10-13 at 25°C.

Suppose 50.00 mL of 2.0 ×\times× 10-6 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×\times× 10-4 M KIO3.Which of the following statements is true? For Fe(IO3)3,Ksp = 1.0 ×\times× 10-14.

What is the minimum mass of Cs2CO3 (molar mass = 325.821 g/mol)that must be added to 54.8 mL of a 5.0 ×\times× 10-4 M AgNO3 solution in order for precipitation to occur? The Ksp of Ag2CO3 is 8.6 ×\times× 10-12.Assume no volume change occurs upon addition of Cs2CO3.

Given the following equilibrium constants, Cd(IO3)2 Ksp = Cd(NH3)42+ Kf = Determine K for the dissolution of the sparingly soluble salt Cd(IO3)2 in aqueous ammonia (shown below).Cd(IO3)2(s)+ 4NH3(aq) Cd(NH3)42+(aq)+ 2IO3-(aq)

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 ×\times× 10-13,Ksp of AgI = 8.5 ×\times× 10-17)

A 25.00-mL sample of propionic acid,HC3H5O2,of unknown concentration was titrated with 0.143 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What was the original concentration of the propionic acid?

The Ksp of BaSO4 is 1.1 ×\times× 10-10 at 25 ∘\circ∘ C.What mass of BaSO4 (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25 ∘\circ∘ C?

What is the molar solubility of Mn(OH)2(s)in a solution that is buffered at pH 8.00 at 25 ∘\circ∘ C? The Ksp of Mn(OH)2 is 1.9 ×\times× 10-13 at 25 ∘\circ∘ C.

What is the concentration of silver(I)ion in a saturated solution of silver(I)carbonate containing 0.0024 M Na2CO3? For Ag2CO3,Ksp = 8.6 ×\times× 10-12.

What is the pH of a buffer that results when 0.40 mol NaHCO2 is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (Ka of HCO2H = 1.8 ×\times× 10-4)

What is the minimum concentration of Cu2+ required to begin precipitating Cu(OH)2(s)in a solution buffered at pH 10.63? The Ksp of Cu(OH)2 is 2.6 ×\times× 10-19 and Kw = 1.01 ×\times× 10-14.

Which acid-base combination is depicted by this titration curve? The dot on the curve is located at the titrant volume where the titration solution pH equals 7.

To make a buffer with a pH of 8.00,you should use a weak acid with a Ka close to _______.

An impure sample of sodium carbonate,Na2CO3,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na2CO3(aq) CO2(g)+ H2O( )+ 2 NaCl(aq) What is the percent of Na2CO3 in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na2CO3 is 106.0 g/mol.

How many moles of solid NaF would have to be added to 1.0 L of 2.39 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(Ka for HF = 7.2 ×\times× 10-4)

A 50.00-mL solution of 0.0729 M chloroacetic acid (Ka = 1.4 ×\times× 10-3)is titrated with a 0.0181 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (Kw = 1.00 ×\times× 10-14)

What is the pH of a solution made by combining 175 mL of 0.33 M NaC2H3O2 with 126 mL of 0.48 M HC2H3O2? The Ka of acetic acid is 1.75 ×\times× 10-5.

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What is the effect of adding NaOH(aq)to an aqueous solution of ammonia? 1)The pH of the solution will increase. 2)The concentration of NH₄⁺(aq)will decrease. 3)The concentration of NH₃(aq)will increase.

What is the solubility product expression for Fe(OH)₃?

What is the molar solubility of silver(I)bromide at 25°C? The solubility product constant for silver(I)bromide is 5.0 $\times$ 10^-13 at 25°C.

Suppose 50.00 mL of 2.0 $\times$ 10^-6 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 $\times$ 10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃)₃,K_sp = 1.0 $\times$ 10^-14.

What is the minimum mass of Cs₂CO₃ (molar mass = 325.821 g/mol)that must be added to 54.8 mL of a 5.0 $\times$ 10^-4 M AgNO₃ solution in order for precipitation to occur? The K_sp of Ag₂CO₃ is 8.6 $\times$ 10^-12.Assume no volume change occurs upon addition of Cs₂CO₃.

Given the following equilibrium constants, Cd(IO₃)₂ K_sp = Cd(NH₃)₄²⁺K_f = Determine K for the dissolution of the sparingly soluble salt Cd(IO₃)₂ in aqueous ammonia (shown below).Cd(IO₃)₂(s)+ 4NH₃(aq) Cd(NH₃)₄²⁺(aq)+ 2IO₃^-(aq)

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 $\times$ 10^-13,K_sp of AgI = 8.5 $\times$ 10^-17)

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.143 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What was the original concentration of the propionic acid?

The K_sp of BaSO₄ is 1.1 $\times$ 10^-10 at 25 ^$\circ$C.What mass of BaSO₄ (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25 ^$\circ$C?

What is the molar solubility of Mn(OH)₂(s)in a solution that is buffered at pH 8.00 at 25 ^$\circ$C? The K_sp of Mn(OH)₂ is 1.9 $\times$ 10^-13 at 25 ^$\circ$C.

What is the concentration of silver(I)ion in a saturated solution of silver(I)carbonate containing 0.0024 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 $\times$ 10^-12.

What is the pH of a buffer that results when 0.40 mol NaHCO₂ is mixed with 100.0 mL of 2.00 M HCl(aq)and diluted with water to 250 mL? (K_a of HCO₂H = 1.8 $\times$ 10^-4)

What is the minimum concentration of Cu²⁺ required to begin precipitating Cu(OH)₂(s)in a solution buffered at pH 10.63? The K_sp of Cu(OH)₂ is 2.6 $\times$ 10^-19 and K_w = 1.01 $\times$ 10^-14.

To make a buffer with a pH of 8.00,you should use a weak acid with a K_a close to _______.

How many moles of solid NaF would have to be added to 1.0 L of 2.39 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(K_a for HF = 7.2 $\times$ 10^-4)

A 50.00-mL solution of 0.0729 M chloroacetic acid (K_a = 1.4 $\times$ 10^-3)is titrated with a 0.0181 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (K_w = 1.00 $\times$ 10^-14)

What is the pH of a solution made by combining 175 mL of 0.33 M NaC₂H₃O₂ with 126 mL of 0.48 M HC₂H₃O₂? The K_a of acetic acid is 1.75 $\times$ 10^-5.