Question 1

Consider the following table of KS1U1B1sp S1U1B0values.  
-Which compound listed below has the smallest molar solubility in water?

Accepted Answer

A)  CdCO3 
B)  CaF2  
C)  Cd(OH)2  
D)  ZnCO3  
E)  AgI 
A)  CdCO3 
B)  CaF2  
C)  Cd(OH)2  
D)  ZnCO3  
E)  AgI

Question 2

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10- 5.

Accepted Answer

Question 3

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.37 × 10- 4.

Accepted Answer

A)  4.13 
B)  3.57 
C)  5.48 
D)  14.28 
E)  10.43 
A)  4.13 
B)  3.57 
C)  5.48 
D)  14.28 
E)  10.43

Question 4

What is the molar solubility of magnesium carbonate ( MgCO3 ) in water? The solubility- product constant for MgCO3 is 3.5 × 10- 8 at 25°C.

Accepted Answer

A)  7.0 × 10- 8  
B)  1.8 × 10- 8  
C)  1.9 × 10- 4  
D)  7.46 
E)  2.6 × 10- 4 
A)  7.0 × 10- 8  
B)  1.8 × 10- 8  
C)  1.9 × 10- 4  
D)  7.46 
E)  2.6 × 10- 4

Question 5

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Accepted Answer

A)  3.92 
B)  21.2 
C)  0.245 
D)  0.153 
E)  29.5 
A)  3.92 
B)  21.2 
C)  0.245 
D)  0.153 
E)  29.5

Question 6

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10- 5.

Accepted Answer

Question 7

A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the present in the buffer solution. The Ka of hydrazoic acid is 1.9 × 10- 5.

Accepted Answer

A)  azide 
B)  This is a buffer solution:
The pH does not change upon addition of acid or base. 
C)  H3O+ 
D)  H2O 
E)  hydrazoic acid 
A)  azide 
B)  This is a buffer solution:
The pH does not change upon addition of acid or base. 
C)  H3O+ 
D)  H2O 
E)  hydrazoic acid

Question 8

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Accepted Answer

A)  0.020 M BaCl2 
B)  0.020 KCl 
C)  pure water 
D)  0.020 AgNO3 
E)  0.015 NaCl 
A)  0.020 M BaCl2 
B)  0.020 KCl 
C)  pure water 
D)  0.020 AgNO3 
E)  0.015 NaCl

Consider the following table of K_spvalues. -Which compound listed below has the smallest molar solubility in water?

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10^-⁵.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_aof lactic acid is 1.37 × 10^-⁴.

What is the molar solubility of magnesium carbonate ( MgCO₃) in water? The solubility- product constant for MgCO₃is 3.5 × 10^-⁸at 25°C.

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10^-⁵.

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

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Exam 17: Additional Aspects of Equilibria

Consider the following table of Ksp values. -Which compound listed below has the smallest molar solubility in water?

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10- 5.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.37 × 10- 4.

What is the molar solubility of magnesium carbonate ( MgCO3 ) in water? The solubility- product constant for MgCO3 is 3.5 × 10- 8 at 25°C.

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10- 5.

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

Consider the following table of K_spvalues. -Which compound listed below has the smallest molar solubility in water?

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10^-⁵.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_aof lactic acid is 1.37 × 10^-⁴.

What is the molar solubility of magnesium carbonate ( MgCO₃) in water? The solubility- product constant for MgCO₃is 3.5 × 10^-⁸at 25°C.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10^-⁵.