Question 1

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO.What is the pH of this solution?

Accepted Answer

A) The pH will be greater than the pKa of hypochlorous acid. 
B) The pH will be less than the pKa of hypochlorous acid. 
C) The pH will be equal to the pKa of hypochlorous acid. 
D) The pH will equal the pKb of sodium hypochlorite. 
E) The pH will be none of these. 
A) The pH will be greater than the pKa of hypochlorous acid. 
B) The pH will be less than the pKa of hypochlorous acid. 
C) The pH will be equal to the pKa of hypochlorous acid. 
D) The pH will equal the pKb of sodium hypochlorite. 
E) The pH will be none of these.

Question 2

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Accepted Answer

A) increases 
B) decreases 
C) does not change 
D) first increases,then decreases 
E) first decreases,then increases 
A) increases 
B) decreases 
C) does not change 
D) first increases,then decreases 
E) first decreases,then increases

Question 3

The solubility of magnesium phosphate is 2.27 $\times$ 10-3 g/1.0 L of solution.What is the Ksp for Mg3(PO4)2?

Accepted Answer

A) 6.5 $\times$ 10-12 
B) 6.0 $\times$ 10-14 
C) 5.2 $\times$ 10-24 
D) 4.8 $\times$ 10-26 
E) 1.0 $\times$ 10-26 
A) 6.5 $\times$ 10-12 
B) 6.0 $\times$ 10-14 
C) 5.2 $\times$ 10-24 
D) 4.8 $\times$ 10-26 
E) 1.0 $\times$ 10-26

Question 4

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Accepted Answer

A) 0.025 mol HCl 
B) 0.063 mol HCl 
C) 0.082 mol HCl 
D) 0.50 mol HCl 
E) 1.0 mol HCl 
A) 0.025 mol HCl 
B) 0.063 mol HCl 
C) 0.082 mol HCl 
D) 0.50 mol HCl 
E) 1.0 mol HCl

Question 5

Hydrochloric acid (0.100 mol L-1,25.00 mL aliquot)is being titrated with sodium hydroxide of the same molarity.Calculate the solution pH after addition of 24.80 mL of the sodium hydroxide.Make any reasonable approximations.

Accepted Answer

Question 6

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 NH4Cl?
Kb = 1.8 $\times$ 10-5

Accepted Answer

A) 1.1 $\times$ 10-5 M 
B) 3.0 $\times$ 10-6 M 
C) 3.3 $\times$ 10-9 M 
D) 9.3 $\times$ 10-10 M 
E) None of these choices is correct. 
A) 1.1 $\times$ 10-5 M 
B) 3.0 $\times$ 10-6 M 
C) 3.3 $\times$ 10-9 M 
D) 9.3 $\times$ 10-10 M 
E) None of these choices is correct.

Question 7

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA)and 0.250 mol of sodium propenoate (NaA)? (Ka for propenoic acid is 5.52 $\times$ 10-5. )

Accepted Answer

The answer of What is the pH of 375 mL...

Question 8

Calculate the solubility of silver phosphate,Ag3PO4,in pure water.Ksp = 2.6 $\times$ 10-18

Accepted Answer

A) 4.0 $\times$ 10-5 M 
B) 1.8 $\times$ 10-5 M 
C) 4.0 $\times$ 10-6 M 
D) 1.5 $\times$ 10-6 M 
E) -6 M 
A) 4.0 $\times$ 10-5 M 
B) 1.8 $\times$ 10-5 M 
C) 4.0 $\times$ 10-6 M 
D) 1.5 $\times$ 10-6 M 
E) -6 M

Question 9

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 $\times$ 10-5 for calcium sulfate

Accepted Answer

A) 1.2 $\times$ 10-2 mol 
B) 4.9 $\times$ 10-3 mol 
C) 3.5 $\times$ 10-3 mol 
D) 1.2 $\times$ 10-5 mol 
E) 4.8 $\times$ 10-8 mol 
A) 1.2 $\times$ 10-2 mol 
B) 4.9 $\times$ 10-3 mol 
C) 3.5 $\times$ 10-3 mol 
D) 1.2 $\times$ 10-5 mol 
E) 4.8 $\times$ 10-8 mol

Question 10

Which one of the following aqueous solutions,when mixed with an equal volume of 0.10 mol L-1 aqueous NH3,will produce a buffer solution?

Accepted Answer

A) 0.10 mol L-1 HCl 
B) 0.20 mol L-1 HCl 
C) 0.10 mol L-1 CH3COOH 
D) 0.050 mol L-1 NaOH 
E) 0.20 mol L-1 NH4Cl 
A) 0.10 mol L-1 HCl 
B) 0.20 mol L-1 HCl 
C) 0.10 mol L-1 CH3COOH 
D) 0.050 mol L-1 NaOH 
E) 0.20 mol L-1 NH4Cl

Question 11

A 25.0-mL sample of 0.10 M C2H3NH2 (ethylamine)is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine?
Kb = 6.5 $\times$ 10-4

Accepted Answer

A) 11.08 
B) 10.88 
C) 10.74 
D) 10.55 
E) 10.49 
A) 11.08 
B) 10.88 
C) 10.74 
D) 10.55 
E) 10.49

Question 12

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa?
Ka = 1.7 $\times$ 10-4

Accepted Answer

A) 1.1 $\times$ 10-4 M 
B) 2.6 $\times$ 10-4 M 
C) 4.3 $\times$ 10-4 M 
D) 6.7 $\times$ 10-5 M 
E) None of these choices is correct. 
A) 1.1 $\times$ 10-4 M 
B) 2.6 $\times$ 10-4 M 
C) 4.3 $\times$ 10-4 M 
D) 6.7 $\times$ 10-5 M 
E) None of these choices is correct.

Question 13

Lead(II)iodide,PbI2,is an ionic compound with a solubility product constant Ksp of 7.9 $\times$ 10-9.Calculate the solubility of this compound in
a.pure water.
b.0.50 mol L-1 KI solution.

Accepted Answer

a.1.3 @#LAT-DLM& 10^-3

Question 14

The solubility of silver chromate is 0.0287 g/1.0 L of solution.What is the Ksp for Ag2CrO4?

Accepted Answer

A) 9.5 $\times$ 10-5 
B) 2.4 $\times$ 10-5 
C) 2.6 $\times$ 10-12 
D) 6.5 $\times$ 10-13 
E) -13 
A) 9.5 $\times$ 10-5 
B) 2.4 $\times$ 10-5 
C) 2.6 $\times$ 10-12 
D) 6.5 $\times$ 10-13 
E) -13

Question 15

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Accepted Answer

A) True 
 B)False

Question 16

Write the ion product expression for calcium phosphate,Ca3(PO4)2.

Accepted Answer

A) 
  
B) 
  
C) 
  
D) 
  
E) None of these is the correct ion product expression. 
A) 
  
B) 
  
C) 
  
D) 
  
E) None of these is the correct ion product expression.

Question 17

What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid)and 0.75 M NaHC6H6O6 (sodium ascorbate)?
Ka = 6.8 $\times$ 10-5

Accepted Answer

A) 3.76 
B) 3.99 
C) 4.34 
D) 4.57 
E) 5.66 
A) 3.76 
B) 3.99 
C) 4.34 
D) 4.57 
E) 5.66

Question 18

Which one of the following pairs of 0.100 mol L-1 solutions,when mixed,will produce a buffer solution?

Accepted Answer

A) 50.mL of aqueous CH3COOH and 25.mL of aqueous HCl 
B) 50.mL of aqueous CH3COOH and 100.mL of aqueous NaOH 
C) 50.mL of aqueous NaOH and 25.mL of aqueous HCl 
D) 50.mL of aqueous CH3COONa and 25.mL of aqueous NaOH 
E) 50.mL of aqueous CH3COOH and 25.mL of aqueous CH3COONa 
A) 50.mL of aqueous CH3COOH and 25.mL of aqueous HCl 
B) 50.mL of aqueous CH3COOH and 100.mL of aqueous NaOH 
C) 50.mL of aqueous NaOH and 25.mL of aqueous HCl 
D) 50.mL of aqueous CH3COONa and 25.mL of aqueous NaOH 
E) 50.mL of aqueous CH3COOH and 25.mL of aqueous CH3COONa

Question 19

What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?

Accepted Answer

A) 4.00 mL 
B) 8.00 mL 
C) 12.5 mL 
D) 16.0 mL 
E) 32.0 mL 
A) 4.00 mL 
B) 8.00 mL 
C) 12.5 mL 
D) 16.0 mL 
E) 32.0 mL

Question 20

An acetate buffer has a pH of 4.40.Which of the following changes will cause the pH to decrease?

Accepted Answer

A) dissolving a small amount of solid sodium acetate 
B) adding a small amount of dilute hydrochloric acid 
C) adding a small amount of dilute sodium hydroxide 
D) dissolving a small amount of solid sodium chloride 
E) diluting the buffer solution with water 
A) dissolving a small amount of solid sodium acetate 
B) adding a small amount of dilute hydrochloric acid 
C) adding a small amount of dilute sodium hydroxide 
D) dissolving a small amount of solid sodium chloride 
E) diluting the buffer solution with water

Exam 19: Ionic Equilibria in Aqueous Systems

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO.What is the pH of this solution?

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

The solubility of magnesium phosphate is 2.27 ×\times× 10-3 g/1.0 L of solution.What is the Ksp for Mg3(PO4)2?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Hydrochloric acid (0.100 mol L-1,25.00 mL aliquot)is being titrated with sodium hydroxide of the same molarity.Calculate the solution pH after addition of 24.80 mL of the sodium hydroxide.Make any reasonable approximations.

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 NH4Cl? Kb = 1.8 ×\times× 10-5

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA)and 0.250 mol of sodium propenoate (NaA)? (Ka for propenoic acid is 5.52 ×\times× 10-5. )

Calculate the solubility of silver phosphate,Ag3PO4,in pure water.Ksp = 2.6 ×\times× 10-18

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 ×\times× 10-5 for calcium sulfate

Which one of the following aqueous solutions,when mixed with an equal volume of 0.10 mol L-1 aqueous NH3,will produce a buffer solution?

A 25.0-mL sample of 0.10 M C2H3NH2 (ethylamine)is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? Kb = 6.5 ×\times× 10-4

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? Ka = 1.7 ×\times× 10-4

Lead(II)iodide,PbI2,is an ionic compound with a solubility product constant Ksp of 7.9 ×\times× 10-9.Calculate the solubility of this compound in a.pure water. b.0.50 mol L-1 KI solution.

The solubility of silver chromate is 0.0287 g/1.0 L of solution.What is the Ksp for Ag2CrO4?

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Write the ion product expression for calcium phosphate,Ca3(PO4)2.

What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid)and 0.75 M NaHC6H6O6 (sodium ascorbate)? Ka = 6.8 ×\times× 10-5

Which one of the following pairs of 0.100 mol L-1 solutions,when mixed,will produce a buffer solution?

What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?

An acetate buffer has a pH of 4.40.Which of the following changes will cause the pH to decrease?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

The solubility of magnesium phosphate is 2.27 $\times$ 10^-3 g/1.0 L of solution.What is the K_sp for Mg₃(PO₄)₂?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Hydrochloric acid (0.100 mol L^-1,25.00 mL aliquot)is being titrated with sodium hydroxide of the same molarity.Calculate the solution pH after addition of 24.80 mL of the sodium hydroxide.Make any reasonable approximations.

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 NH₄Cl? K_b = 1.8 $\times$ 10^-5

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA)and 0.250 mol of sodium propenoate (NaA)? (K_a for propenoic acid is 5.52 $\times$ 10^-5. )

Calculate the solubility of silver phosphate,Ag₃PO₄,in pure water.K_sp = 2.6 $\times$ 10^-18

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂ before precipitation of calcium sulfate begins? K_sp = 2.4 $\times$ 10^-5 for calcium sulfate

Which one of the following aqueous solutions,when mixed with an equal volume of 0.10 mol L^-1 aqueous NH₃,will produce a buffer solution?

A 25.0-mL sample of 0.10 M C₂H₃NH₂ (ethylamine)is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? K_b = 6.5 $\times$ 10^-4

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? K_a = 1.7 $\times$ 10^-4

Lead(II)iodide,PbI₂,is an ionic compound with a solubility product constant K_sp of 7.9 $\times$ 10^-⁹.Calculate the solubility of this compound in a.pure water. b.0.50 mol L^-1 KI solution.

The solubility of silver chromate is 0.0287 g/1.0 L of solution.What is the K_sp for Ag₂CrO₄?

Write the ion product expression for calcium phosphate,Ca₃(PO₄)₂.

What is the pH of a solution that consists of 0.50 M H₂C₆H₆O₆ (ascorbic acid)and 0.75 M NaHC₆H₆O₆ (sodium ascorbate)? K_a = 6.8 $\times$ 10^-5

Which one of the following pairs of 0.100 mol L^-1 solutions,when mixed,will produce a buffer solution?

What volume of 0.500 M H₂SO₄ is needed to react completely with 20.0 mL of 0.400 M LiOH?