Question 1

Which of the following is an acidic salt?

Accepted Answer

A)  RbCl 
B)  Sr(NO2)2 
C)  CaNO2 
D)  CaBr2 
E)  MnI2 
A)  RbCl 
B)  Sr(NO2)2 
C)  CaNO2 
D)  CaBr2 
E)  MnI2 E

Question 2

A reaction between an acid and a base is called a combustion reaction.

Accepted Answer

A) True 
 B)False  False

Question 3

Which of the following is required to react with Zn(OH)2 to produce Zn3(PO4)2?

Accepted Answer

A)  H2PO3 
B)  H2PO4 
C)  HPO4 
D)  H3PO4 
E)  H2P2O4 
A)  H2PO3 
B)  H2PO4 
C)  HPO4 
D)  H3PO4 
E)  H2P2O4 D

Question 4

Which of the following can be a component in a buffer?

Accepted Answer

A)  LiBr 
B)  NaI 
C)  KNO3 
D)  K3PO4 
E)  SrI2 
A)  LiBr 
B)  NaI 
C)  KNO3 
D)  K3PO4 
E)  SrI2

Question 5

Which of the following is an Arrhenius acid?

Accepted Answer

A)  H2SO3 
B)  NaOH 
C)  Na2CO3 
D)  HgI2 
E)  Al2(SO4)3 
A)  H2SO3 
B)  NaOH 
C)  Na2CO3 
D)  HgI2 
E)  Al2(SO4)3

Question 6

Briefly describe conjugate acid-base pairs.

Accepted Answer

In the reaction between NH₃ and H₂O, two s

Question 7

A _____is any species that can accept a proton (H+) from another molecule.

Accepted Answer

Question 8

Differentiate between Arrhenius acids and Arrhenius bases.

Accepted Answer

An Arrhenius acid is a compoun

Question 9

A 0.0788 M solution of HC2H3O2 is 3.0% ionized into H+ ions and C2H3O2− ions. What is [OH−] for this solution?

Accepted Answer

A)  8.5 *10-12 M 
B)  2.1 *10-12 M 
C)  4.2 *10-12 M 
D)  8.5 * 1012 M 
E)  0.0788 M 
A)  8.5 *10-12 M 
B)  2.1 *10-12 M 
C)  4.2 *10-12 M 
D)  8.5 * 1012 M 
E)  0.0788 M

Question 10

If pH is _____, then the solution is acidic.

Accepted Answer

The answer of If pH is _____, then the solution...

Question 11

Differentiate between strong acids and weak acids.

Accepted Answer

Any acid that dissociates 100%

Question 12

Consider the product of the two concentrations, [H+][OH−]. If one concentration goes up, the other must go up to compensate so that their product equals the value of the autoionization constant of water.

Accepted Answer

A) True 
 B)False

Question 13

In the reaction H3PO4 + OH− $\rightarrow$H2PO4− + H2O, H3PO4 and H2PO4− are a conjugate acid-base pair.

Accepted Answer

A) True 
 B)False

Question 14

Small amounts of weak acids and bases can change the pH of a solution very quickly.

Accepted Answer

A) True 
 B)False

Question 15

A reaction between an acid and a base is called a(n):

Accepted Answer

A)  combustion reaction. 
B)  decomposition reaction. 
C)  hydrogenation reaction. 
D)  neutralization reaction. 
E)  alkylation reaction. 
A)  combustion reaction. 
B)  decomposition reaction. 
C)  hydrogenation reaction. 
D)  neutralization reaction. 
E)  alkylation reaction.

Question 16

HCl is an Arrhenius acid.

Accepted Answer

A) True 
 B)False

Question 17

Which of the following combinations of compounds can make a buffer solution?

Accepted Answer

A)  HCOOH and CH3COOH 
B)  NaCl and BaCl2 
C)  HCl and Ca(OH)2 
D)  H3PO4 and Li3PO4 
E)  NH3 and NaOH 
A)  HCOOH and CH3COOH 
B)  NaCl and BaCl2 
C)  HCl and Ca(OH)2 
D)  H3PO4 and Li3PO4 
E)  NH3 and NaOH

Question 18

When ammonia reacts with water, water acts like a_____.

Accepted Answer

The answer of When ammonia reacts with water, water acts...

Question 19

What is the pOH of a solution when [H+] is 5.88 × 10−11 M?

Accepted Answer

A)  10.1 
B)  7.88 
C)  10.23 
D)  3.77 
E)  15.6 
A)  10.1 
B)  7.88 
C)  10.23 
D)  3.77 
E)  15.6

Question 20

Water molecules act as acids (proton donors) and bases (proton acceptors) with each other to a tiny extent in all aqueous solutions. This is known as the _____.

Accepted Answer

autoioniza

Which of the following is an acidic salt?

A reaction between an acid and a base is called a combustion reaction.

Which of the following is required to react with Zn(OH)₂to produce Zn₃(PO₄)₂?

Which of the following can be a component in a buffer?

Which of the following is an Arrhenius acid?

Briefly describe conjugate acid-base pairs.

A _____is any species that can accept a proton (H⁺) from another molecule.

Differentiate between Arrhenius acids and Arrhenius bases.

A 0.0788 M solution of HC₂H₃O₂ is 3.0% ionized into H⁺ ions and C₂H₃O₂⁻ ions. What is [OH⁻] for this solution?

If pH is _____, then the solution is acidic.

Differentiate between strong acids and weak acids.

Consider the product of the two concentrations, [H⁺][OH⁻]. If one concentration goes up, the other must go up to compensate so that their product equals the value of the autoionization constant of water.

In the reaction H₃PO₄ + OH⁻ $\rightarrow$ H₂PO₄⁻ + H₂O, H₃PO₄ and H₂PO₄⁻ are a conjugate acid-base pair.

Small amounts of weak acids and bases can change the pH of a solution very quickly.

A reaction between an acid and a base is called a(n):

HCl is an Arrhenius acid.

Which of the following combinations of compounds can make a buffer solution?

When ammonia reacts with water, water acts like a_____.

What is the pOH of a solution when [H⁺] is 5.88 × 10⁻¹¹ M?

Water molecules act as acids (proton donors) and bases (proton acceptors) with each other to a tiny extent in all aqueous solutions. This is known as the _____.

What Is Chemistry

Measurements

Atoms, Molecules, and Ions

Chemical Reactions and Equations

Stoichiometry and the Mole

Gases

Energy and Chemistry

Electronic Structure

Chemical Bonds

Solids and Liquids

Solutions

Chemical Equilibrium

Oxidation and Reduction

Nuclear Chemistry

Organic Chemistry

Filters

Exam 12: Acids and Bases

Which of the following is an acidic salt?

A reaction between an acid and a base is called a combustion reaction.

Which of the following is required to react with Zn(OH)2 to produce Zn3(PO4)2?

Which of the following can be a component in a buffer?

Which of the following is an Arrhenius acid?

Briefly describe conjugate acid-base pairs.

A _____is any species that can accept a proton (H+) from another molecule.

Differentiate between Arrhenius acids and Arrhenius bases.

A 0.0788 M solution of HC2H3O2 is 3.0% ionized into H+ ions and C2H3O2− ions. What is [OH−] for this solution?

If pH is _____, then the solution is acidic.

Differentiate between strong acids and weak acids.

Consider the product of the two concentrations, [H+][OH−]. If one concentration goes up, the other must go up to compensate so that their product equals the value of the autoionization constant of water.

In the reaction H3PO4 + OH− →\rightarrow→ H2PO4− + H2O, H3PO4 and H2PO4− are a conjugate acid-base pair.

Small amounts of weak acids and bases can change the pH of a solution very quickly.

A reaction between an acid and a base is called a(n):

HCl is an Arrhenius acid.

Which of the following combinations of compounds can make a buffer solution?

When ammonia reacts with water, water acts like a_____.

What is the pOH of a solution when [H+] is 5.88 × 10−11 M?

Water molecules act as acids (proton donors) and bases (proton acceptors) with each other to a tiny extent in all aqueous solutions. This is known as the _____.

What Is Chemistry

Measurements

Atoms, Molecules, and Ions

Chemical Reactions and Equations

Stoichiometry and the Mole

Gases

Energy and Chemistry

Electronic Structure

Chemical Bonds

Solids and Liquids

Solutions

Chemical Equilibrium

Oxidation and Reduction

Nuclear Chemistry

Organic Chemistry

Filters

Which of the following is required to react with Zn(OH)₂to produce Zn₃(PO₄)₂?

A _____is any species that can accept a proton (H⁺) from another molecule.

A 0.0788 M solution of HC₂H₃O₂ is 3.0% ionized into H⁺ ions and C₂H₃O₂⁻ ions. What is [OH⁻] for this solution?

Consider the product of the two concentrations, [H⁺][OH⁻]. If one concentration goes up, the other must go up to compensate so that their product equals the value of the autoionization constant of water.

In the reaction H₃PO₄ + OH⁻ $\rightarrow$ H₂PO₄⁻ + H₂O, H₃PO₄ and H₂PO₄⁻ are a conjugate acid-base pair.

What is the pOH of a solution when [H⁺] is 5.88 × 10⁻¹¹ M?