Question 1

What name is given to a solution that contains a weak acid and its conjugate base?

Accepted Answer

The answer of What name is given to a solution...

Question 2

Write the ion product expression for calcium phosphate,Ca3(P O4)2.

Accepted Answer

A)    
B)    
C)    
D)    
E) (3 × [Ca2+])(2 × [P O43- ] 
A)    
B)    
C)    
D)    
E) (3 × [Ca2+])(2 × [P O43- ]

Question 3

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH3 with 0.20 M HCl. [Kb(NH3)= 1.8 × 10-5]

Accepted Answer

A) 2.87 
B) 4.98 
C) 5.13 
D) 7.00 
E) 11.13 
A) 2.87 
B) 4.98 
C) 5.13 
D) 7.00 
E) 11.13

Question 4

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M)with a strong base of the same concentration?

Accepted Answer

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

Question 5

A 25.0-mL sample of 0.10 M C2H5NH2 (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(C2H5NH2)= 6.5 × 10-4]

Accepted Answer

A) 11.08 
B) 10.74 
C) 10.81 
D) 10.55 
E) 10.49 
A) 11.08 
B) 10.74 
C) 10.81 
D) 10.55 
E) 10.49

Question 6

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.)   What is Ksp for MX?

Accepted Answer

A) 1.5 ×10-5 
B) 6.0 ×10-6 
C) 3.6 ×10-1 
D) 1.8 ×10-3 
E) 9.0 ×10-6 
A) 1.5 ×10-5 
B) 6.0 ×10-6 
C) 3.6 ×10-1 
D) 1.8 ×10-3 
E) 9.0 ×10-6

Question 7

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO)and 1.0 mole of cyanic acid (HCNO)in enough water to make 1.0 liter of solution. [Ka(HCNO)= 2.0 × 10-4]

Accepted Answer

A) 0.00 
B) 3.00 
C) 3.70 
D) 4.40 
E) 5.00 
A) 0.00 
B) 3.00 
C) 3.70 
D) 4.40 
E) 5.00

Question 8

Which is more soluble in a basic solution than in pure water?

Accepted Answer

A) AgF 
B) AgCN 
C) CO2 
D) NaCl 
E) CH3COOK 
A) AgF 
B) AgCN 
C) CO2 
D) NaCl 
E) CH3COOK

Question 9

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

Accepted Answer

A) True 
 B)False

What name is given to a solution that contains a weak acid and its conjugate base?

Write the ion product expression for calcium phosphate,Ca₃(P O₄)₂.

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH₃ with 0.20 M HCl. [Kb(NH₃)= 1.8 × 10^-5]

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H₂A (0.10 M)with a strong base of the same concentration?

A 25.0-mL sample of 0.10 M C₂H₅NH₂ (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(C₂H₅NH₂)= 6.5 × 10^-4]

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.) What is K_sp for MX?

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO)and 1.0 mole of cyanic acid (HCNO)in enough water to make 1.0 liter of solution. [K_a(HCNO)= 2.0 × 10^-4]

Which is more soluble in a basic solution than in pure water?

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

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

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Exam 17: Acid-Base Equilibria and Solubility Equilibria

What name is given to a solution that contains a weak acid and its conjugate base?

Write the ion product expression for calcium phosphate,Ca3(P O4)2.

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH3 with 0.20 M HCl. [Kb(NH3)= 1.8 × 10-5]

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M)with a strong base of the same concentration?

A 25.0-mL sample of 0.10 M C2H5NH2 (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(C2H5NH2)= 6.5 × 10-4]

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.) What is Ksp for MX?

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO)and 1.0 mole of cyanic acid (HCNO)in enough water to make 1.0 liter of solution. [Ka(HCNO)= 2.0 × 10-4]

Which is more soluble in a basic solution than in pure water?

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

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

Write the ion product expression for calcium phosphate,Ca₃(P O₄)₂.

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH₃ with 0.20 M HCl. [Kb(NH₃)= 1.8 × 10^-5]

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H₂A (0.10 M)with a strong base of the same concentration?

A 25.0-mL sample of 0.10 M C₂H₅NH₂ (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(C₂H₅NH₂)= 6.5 × 10^-4]

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.) What is K_sp for MX?

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO)and 1.0 mole of cyanic acid (HCNO)in enough water to make 1.0 liter of solution. [K_a(HCNO)= 2.0 × 10^-4]