Calculate the molar concentration of uncomplexed Zn2+(aq)in a solution that contains 0.24 M Zn(NH3)42+ and 0.3671 M NH3 at equilibrium.Kf for Zn(NH3)42+ is .

A) M B) M C) M D) M E) M A) M B) M C) M D) M E) M A

What mass of solid NaCH3CO2 (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH3CO2H to make a buffer with a pH of 7.21? (pKa of CH3CO2H = 7.21)

A) 0.0 g B) 1.9 g C) 41 g D) 71 g E) 1.6 $\times$ 102 g A) 0.0 g B) 1.9 g C) 41 g D) 71 g E) 1.6 $\times$ 102 g C

The Ksp of Ca(OH)2 is 5.5 $\times$10-5 at 25 S1U1P1$\circ$S1S1P0C.What is the concentration of OH-(aq)in a saturated solution of Ca(OH)2(aq)?

A) 1.9 $\times$ 10-3 M B) 7.4 $\times$ 10-3 M C) 2.4 $\times$ 10-2 M D) 4.0 $\times$ 10-2 M E) 4.8 $\times$ 10-2 M A) 1.9 $\times$ 10-3 M B) 7.4 $\times$ 10-3 M C) 2.4 $\times$ 10-2 M D) 4.0 $\times$ 10-2 M E) 4.8 $\times$ 10-2 M

How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq)to make a buffer with a pH of 9.00? (pKa of NH4+ = 9.25)

A) 0.36 mol B) 0.44 mol C) 0.56 mol D) 0.64 mol E) 1.8 mol A) 0.36 mol B) 0.44 mol C) 0.56 mol D) 0.64 mol E) 1.8 mol

What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2)is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H)and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 $\times$ 10-5)

A) 2.52 B) 4.23 C) 4.44 D) 4.64 E) 4.74 A) 2.52 B) 4.23 C) 4.44 D) 4.64 E) 4.74

What is the pH of a saturated solution of Fe(OH)2? For Fe(OH)2,Ksp = 8.0 $\times$ 10-16 and Kw = 1.01 $\times$ 10-14.

A) 4.93 B) 8.77 C) 5.23 D) 9.07 E) 7.00 A) 4.93 B) 8.77 C) 5.23 D) 9.07 E) 7.00

What is the value of the dissociation constant,Kd,for the complex ion Cd(NH3)42+? For Cd(NH3)42+,Kf = 1.0 $\times$ 107.

A) 1.0 $\times$ 10-7 B) 2.5 $\times$ 106 C) 1.0 $\times$ 107 D) 5.6 $\times$ 101 E) 1.0 $\times$ 10 -7 A) 1.0 $\times$ 10-7 B) 2.5 $\times$ 106 C) 1.0 $\times$ 107 D) 5.6 $\times$ 101 E) 1.0 $\times$ 10 -7

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

Calculate the molar concentration of uncomplexed Zn²⁺(aq)in a solution that contains 0.24 M Zn(NH₃)₄²⁺ and 0.3671 M NH₃ at equilibrium.K_f for Zn(NH₃)₄²⁺ is .

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

A 25.0 mL sample of 0.200 M HCO₂H(aq)is titrated with 0.100 M KOH(aq).What is the pH at the equivalence point? (K_a of HCO₂H = 1.8 $\times$ 10^-4)

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

What mass of solid NaCH₃CO₂ (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH₃CO₂H to make a buffer with a pH of 7.21? (pK_a of CH₃CO₂H = 7.21)

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

The K_sp of Ca(OH)₂ is 5.5 $\times$ 10^-5 at 25 ^$\circ$C.What is the concentration of OH^-(aq)in a saturated solution of Ca(OH)₂(aq)?

(Multiple Choice)

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Question 4

How many moles of HCl must be added to 1.0 L of 1.0 M NH₃(aq)to make a buffer with a pH of 9.00? (pK_a of NH₄⁺ = 9.25)

(Multiple Choice)

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Question 5

Hyperventilation can cause your blood pH to rise.One way to lower your blood pH is to breath into a paper bag,thus recycling the air you exhale.Why does this procedure lower your blood pH?

(Essay)

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Question 6

Why do salts containing basic anions have a greater solubility in water than predicted from calculations using K_sp values? Examples of such salts are CaCO₃,PbF₂,and Ca₃(PO₄)₂.

(Essay)

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Question 7

For a monoprotic acid titration,the ________ point in a titration is the point where the moles of strong base added equals the moles of acid initially present.

(Short Answer)

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Question 8

What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂)is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H)and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 $\times$ 10^-5)

(Multiple Choice)

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Question 9

A 4.0 $\times$ 10^-4M solution of MnSO₄ is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? The K_sp of Mn(OH)₂ is 2.0 $\times$ 10^-13 and K_w = 1.01 $\times$ 10^-14.

(Multiple Choice)

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Question 10

What is the pH of a saturated solution of Fe(OH)₂? For Fe(OH)₂,K_sp = 8.0 $\times$ 10^-16 and K_w = 1.01 $\times$ 10^-14.

(Multiple Choice)

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Question 11

A solution containing 10.mmol of CO₃^2- and 5.0 mmol of HCO₃^-is titrated with 1.7 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

(Multiple Choice)

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Question 12

What is the pH of a solution that is 0.028 M in HA and also 0.0054 M in NaA? (K_a = 3.2 $\times$ 10^-6)

(Multiple Choice)

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Question 13

What is the solution pH when 0.10 mol of H⁺ is added to a 2.0-liter buffered solution created from 0.45 M NH₃ (K_b = 1.8 $\times$ 10^-5)and 0.26 M NH₄F.

(Multiple Choice)

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Question 14

The solubility of barium carbonate (BaCO₃)in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

(Multiple Choice)

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Question 15

A 1.0-liter solution contains 0.25 M HF and 0.32 M NaF (K_afor HF is 7.2 $\times$ 10^-4).If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the $\underline{\text{ change }}$ in pH?

(Multiple Choice)

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Question 16

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 $\times$ 10^-3,K_a2 = 6.2 $\times$ 10^-8,and K_a3 = 3.6 $\times$ 10^-13)

(Multiple Choice)

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Question 17

When a weak base is titrated with a strong acid,the pH at the equivalence point is ___.

(Multiple Choice)

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Question 18

What is the value of the dissociation constant,K_d,for the complex ion Cd(NH₃)₄²⁺? For Cd(NH₃)₄²⁺,K_f = 1.0 $\times$ 10⁷.

(Multiple Choice)

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Question 19

When mixed in appropriate amounts,each of the following mixtures can produce an effective buffer solution EXCEPT

(Multiple Choice)

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Question 20

Showing 1 - 20 of 88

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

Calculate the molar concentration of uncomplexed Zn2+(aq)in a solution that contains 0.24 M Zn(NH3)42+ and 0.3671 M NH3 at equilibrium.Kf for Zn(NH3)42+ is .

A 25.0 mL sample of 0.200 M HCO2H(aq)is titrated with 0.100 M KOH(aq).What is the pH at the equivalence point? (Ka of HCO2H = 1.8 ×\times× 10-4)

What mass of solid NaCH3CO2 (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH3CO2H to make a buffer with a pH of 7.21? (pKa of CH3CO2H = 7.21)

The Ksp of Ca(OH)2 is 5.5 ×\times× 10-5 at 25 ∘\circ∘ C.What is the concentration of OH-(aq)in a saturated solution of Ca(OH)2(aq)?

How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq)to make a buffer with a pH of 9.00? (pKa of NH4+ = 9.25)

Hyperventilation can cause your blood pH to rise.One way to lower your blood pH is to breath into a paper bag,thus recycling the air you exhale.Why does this procedure lower your blood pH?

Why do salts containing basic anions have a greater solubility in water than predicted from calculations using Ksp values? Examples of such salts are CaCO3,PbF2,and Ca3(PO4)2.

For a monoprotic acid titration,the ________ point in a titration is the point where the moles of strong base added equals the moles of acid initially present.

What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2)is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H)and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 ×\times× 10-5)

A 4.0 ×\times× 10-4 M solution of MnSO4 is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? The Ksp of Mn(OH)2 is 2.0 ×\times× 10-13 and Kw = 1.01 ×\times× 10-14.

What is the pH of a saturated solution of Fe(OH)2? For Fe(OH)2,Ksp = 8.0 ×\times× 10-16 and Kw = 1.01 ×\times× 10-14.

A solution containing 10.mmol of CO32- and 5.0 mmol of HCO3-is titrated with 1.7 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

What is the pH of a solution that is 0.028 M in HA and also 0.0054 M in NaA? (Ka = 3.2 ×\times× 10-6)

What is the solution pH when 0.10 mol of H+ is added to a 2.0-liter buffered solution created from 0.45 M NH3 (Kb = 1.8 ×\times× 10-5)and 0.26 M NH4F.

The solubility of barium carbonate (BaCO3)in water at 25°C is g/L.What is the Ksp of this sparingly soluble salt?

A 1.0-liter solution contains 0.25 M HF and 0.32 M NaF (Ka for HF is 7.2 ×\times× 10-4).If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the change ‾\underline{\text{ change }} change ​ in pH?

What is the pH of a buffer that results when 0.50 mole of H3PO4 is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are Ka1 = 7.5 ×\times× 10-3,Ka2 = 6.2 ×\times× 10-8,and Ka3 = 3.6 ×\times× 10-13)

When a weak base is titrated with a strong acid,the pH at the equivalence point is ___.

What is the value of the dissociation constant,Kd,for the complex ion Cd(NH3)42+? For Cd(NH3)42+,Kf = 1.0 ×\times× 107.

When mixed in appropriate amounts,each of the following mixtures can produce an effective buffer solution EXCEPT

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Calculate the molar concentration of uncomplexed Zn²⁺(aq)in a solution that contains 0.24 M Zn(NH₃)₄²⁺ and 0.3671 M NH₃ at equilibrium.K_f for Zn(NH₃)₄²⁺ is .

A 25.0 mL sample of 0.200 M HCO₂H(aq)is titrated with 0.100 M KOH(aq).What is the pH at the equivalence point? (K_a of HCO₂H = 1.8 $\times$ 10^-4)

What mass of solid NaCH₃CO₂ (molar mass = 82.0 g/mol)should be added to 1.0 L of 0.50 M CH₃CO₂H to make a buffer with a pH of 7.21? (pK_a of CH₃CO₂H = 7.21)

The K_sp of Ca(OH)₂ is 5.5 $\times$ 10^-5 at 25 ^$\circ$C.What is the concentration of OH^-(aq)in a saturated solution of Ca(OH)₂(aq)?

How many moles of HCl must be added to 1.0 L of 1.0 M NH₃(aq)to make a buffer with a pH of 9.00? (pK_a of NH₄⁺ = 9.25)

Why do salts containing basic anions have a greater solubility in water than predicted from calculations using K_sp values? Examples of such salts are CaCO₃,PbF₂,and Ca₃(PO₄)₂.

What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂)is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H)and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 $\times$ 10^-5)

A 4.0 $\times$ 10^-4M solution of MnSO₄ is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? The K_sp of Mn(OH)₂ is 2.0 $\times$ 10^-13 and K_w = 1.01 $\times$ 10^-14.

What is the pH of a saturated solution of Fe(OH)₂? For Fe(OH)₂,K_sp = 8.0 $\times$ 10^-16 and K_w = 1.01 $\times$ 10^-14.

A solution containing 10.mmol of CO₃^2- and 5.0 mmol of HCO₃^-is titrated with 1.7 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

What is the pH of a solution that is 0.028 M in HA and also 0.0054 M in NaA? (K_a = 3.2 $\times$ 10^-6)

What is the solution pH when 0.10 mol of H⁺ is added to a 2.0-liter buffered solution created from 0.45 M NH₃ (K_b = 1.8 $\times$ 10^-5)and 0.26 M NH₄F.

The solubility of barium carbonate (BaCO₃)in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

A 1.0-liter solution contains 0.25 M HF and 0.32 M NaF (K_afor HF is 7.2 $\times$ 10^-4).If one adds 0.30 liters of 0.020 M KOH to the solution,what will be the $\underline{\text{ change }}$ in pH?

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 $\times$ 10^-3,K_a2 = 6.2 $\times$ 10^-8,and K_a3 = 3.6 $\times$ 10^-13)

What is the value of the dissociation constant,K_d,for the complex ion Cd(NH₃)₄²⁺? For Cd(NH₃)₄²⁺,K_f = 1.0 $\times$ 10⁷.