Question 1

For a solution labeled "0.10 M H2SO4(aq),"

Accepted Answer

A) [HSO4-] is greater than 0.10 M. 
B) the pH is less than 1.0. 
C) [SO42-] = 0.10 M. 
D) the pH equals 1.0. 
E) the pH is greater than 1.0. 
A) [HSO4-] is greater than 0.10 M. 
B) the pH is less than 1.0. 
C) [SO42-] = 0.10 M. 
D) the pH equals 1.0. 
E) the pH is greater than 1.0.

Question 2

What is the [H+] for a solution labeled "0.0500 M H2SO3(aq)" if pKa1 = 1.81,and pKa2 = 6.91?

Accepted Answer

A) 0.021 M 
B) 0.029 M 
C) 0.015 M 
D) 0.025 M 
E) 0.050 M 
A) 0.021 M 
B) 0.029 M 
C) 0.015 M 
D) 0.025 M 
E) 0.050 M

Question 3

The fractional composition diagram for the amino acid alanine is shown below.   What do the two points represent where alpha is 0.5?

Accepted Answer

The answer of The fractional composition diagram for the amino...

Question 4

What is the pKa of the conjugate acid of hydrazine,given that the pKb of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

Accepted Answer

Question 5

All of the following are Lewis bases except

Accepted Answer

A) OH- 
B) H2O 
C) SO3 
D) Br- 
A) OH- 
B) H2O 
C) SO3 
D) Br-

Question 6

the pH of 0.10 M and 0.40 M NaHCO3(aq)solutions is 8.31 for both?

Accepted Answer

A) True 
 B)False

Question 7

A 0.0010 M solution of a weak acid,HA,with Ka = 2 * 10-10 produces [H3O+] -6 M.Which of the following equations can be used to determine [H3O+]?

Accepted Answer

A) The acid is so weak that the pH is about 7. 
B) [H3O+]2 + Ka [H3O+] - [HA]initialKa = 0 
C) [H3O+] = (Kw + Ka[HA]initial)½ 
D) [H3O+] = [HA]initial  
E) [H3O+] = (Ka[HA]initial)½ 
A) The acid is so weak that the pH is about 7. 
B) [H3O+]2 + Ka [H3O+] - [HA]initialKa = 0 
C) [H3O+] = (Kw + Ka[HA]initial)½ 
D) [H3O+] = [HA]initial  
E) [H3O+] = (Ka[HA]initial)½

Question 8

Calculate the hydroxide ion concentration for an aqueous solution that has a pH of 3.45.

Accepted Answer

A) 3.2 * 10-2 M 
B) 0.54 M 
C) 3.5 * 10-4 M 
D) 2.8 * 10-11 M 
E) 2.6 * 10-5 M 
A) 3.2 * 10-2 M 
B) 0.54 M 
C) 3.5 * 10-4 M 
D) 2.8 * 10-11 M 
E) 2.6 * 10-5 M

Question 9

The equation that represents Ka2 for phosphoric acid is

Accepted Answer

A) HPO42-(aq)+ H2O(l)↔ PO43-(aq)+ H3O+(aq) 
B) H2PO4(aq)+ H2O(l)↔ HPO42(aq)+ H3O+(aq). 
C) H3PO4(aq)+ 2H2O(l)↔ HPO42-(aq)+ 2H3O+(aq). 
D) HPO42-(aq)+ H2O(l)↔ H2PO4-(aq)+ OH-(aq). 
E) H3PO4(aq)+ H2O(l)↔ H2PO4-(aq)+ H3O+(aq). 
A) HPO42-(aq)+ H2O(l)↔ PO43-(aq)+ H3O+(aq) 
B) H2PO4(aq)+ H2O(l)↔ HPO42(aq)+ H3O+(aq). 
C) H3PO4(aq)+ 2H2O(l)↔ HPO42-(aq)+ 2H3O+(aq). 
D) HPO42-(aq)+ H2O(l)↔ H2PO4-(aq)+ OH-(aq). 
E) H3PO4(aq)+ H2O(l)↔ H2PO4-(aq)+ H3O+(aq).

Question 10

Calculate the hydrogen ion concentration for an aqueous solution that has a pH of 3.45.

Accepted Answer

A) 0.54 M 
B) 3.5 * 10-4 M 
C) 2.8 * 10-11  
D) 3.2 * 10-2 M 
E) 1.22 M 
A) 0.54 M 
B) 3.5 * 10-4 M 
C) 2.8 * 10-11  
D) 3.2 * 10-2 M 
E) 1.22 M

Question 11

The conjugate acid of HPO42- is

Accepted Answer

A) HPO42-. 
B) PO43-. 
C) H2PO4-. 
D) H3O+. 
E) H3PO4. 
A) HPO42-. 
B) PO43-. 
C) H2PO4-. 
D) H3O+. 
E) H3PO4.

Question 12

All of the following 0.1 M aqueous solutions are acidic except

Accepted Answer

A) Na2SO4. 
B) Cr(ClO4)3. 
C) C6H5OH. 
D) C2H5NH3Cl. 
A) Na2SO4. 
B) Cr(ClO4)3. 
C) C6H5OH. 
D) C2H5NH3Cl.

Question 13

If the pKa of acetic acid is 4.75,the pKa of CH3CH2OH is

Accepted Answer

A) about 4. 
B) much less than 4.75. 
C) about 16. 
D) also 4.75. 
E) about 7. 
A) about 4. 
B) much less than 4.75. 
C) about 16. 
D) also 4.75. 
E) about 7.

Question 14

The Ka of phenol is 1.3 * 10-10.For a solution labeled "1.0 *10-3 M aqueous phenol,"

Accepted Answer

A) Kw/[H3O+] >> [phenol]initial. 
B) Kw/[H3O+] initial. 
C) [H3O+] > 10-6. 
D) pH ~ 4. 
E) [H3O+] = [H3O+]2/[phenol]initial. 
A) Kw/[H3O+] >> [phenol]initial. 
B) Kw/[H3O+] initial. 
C) [H3O+] > 10-6. 
D) pH ~ 4. 
E) [H3O+] = [H3O+]2/[phenol]initial.

Question 15

Which of the following is not a Lewis acid?

Accepted Answer

A) H3O+ 
B) SO3 
C) NO2- 
D) BF3  
E) BCl3 
A) H3O+ 
B) SO3 
C) NO2- 
D) BF3  
E) BCl3

Question 16

The conjugate base of OH- is

Accepted Answer

A) H+. 
B) OH-. 
C) O2-. 
D) H3O+. 
E) H2O. 
A) H+. 
B) OH-. 
C) O2-. 
D) H3O+. 
E) H2O.

Question 17

The amino acid alanine,HOOC-CH(CH3)NH3+,has Ka1 = 4.5 * 10-3 and Ka2 = 1.4 * 10-10.Calculate $\alpha$(HOOC-CH(CH3)NH3+)at pH 3.

Accepted Answer

A) 0 
B) 0.82 
C) 0.58 
D) 0.29 
E) 0.18 
A) 0 
B) 0.82 
C) 0.58 
D) 0.29 
E) 0.18

Question 18

Of the following,which does not have an amphoteric oxide?

Accepted Answer

A) BeO 
B) PbO 
C) SnO 
D) Al2O3 
E) MgO 
A) BeO 
B) PbO 
C) SnO 
D) Al2O3 
E) MgO

Question 19

Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

Accepted Answer

A) True 
 B)False

Question 20

The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where A is the solution of lowest pH and E is the solution of highest pH.   Match each box with the correct compound.
phenol,pKa = 9.89
cyanide ion,pKb = 4.69
pyridine,pKb = 8.75
hydrogen sulfate ion,pKa = 1.92
sodium nitrate

Accepted Answer

phenol,pK_a = 9.89 (B) cyanide i

For a solution labeled "0.10 M H₂SO₄(aq),"

What is the [H⁺] for a solution labeled "0.0500 M H₂SO₃(aq)" if pK_a1 = 1.81,and pK_a2 = 6.91?

The fractional composition diagram for the amino acid alanine is shown below. $The fractional composition diagram for the amino acid alanine is shown below. What do the two points represent where alpha is 0.5?$ What do the two points represent where alpha is 0.5?

What is the pK_a of the conjugate acid of hydrazine,given that the pK_b of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

All of the following are Lewis bases except

the pH of 0.10 M and 0.40 M NaHCO₃(aq)solutions is 8.31 for both?

A 0.0010 M solution of a weak acid,HA,with K_a = 2 * 10^-10 produces [H₃O⁺] < 10^-6 M.Which of the following equations can be used to determine [H₃O⁺]?

Calculate the hydroxide ion concentration for an aqueous solution that has a pH of 3.45.

The equation that represents K_a2 for phosphoric acid is

Calculate the hydrogen ion concentration for an aqueous solution that has a pH of 3.45.

The conjugate acid of HPO₄^2- is

All of the following 0.1 M aqueous solutions are acidic except

If the pK_a of acetic acid is 4.75,the pK_a of CH₃CH₂OH is

The K_a of phenol is 1.3 * 10^-10.For a solution labeled "1.0 *10^-3 M aqueous phenol,"

Which of the following is not a Lewis acid?

The conjugate base of OH^- is

The amino acid alanine,HOOC-CH(CH₃)NH₃⁺,has K_a1 = 4.5 * 10^-3 and K_a2 = 1.4 * 10^-10.Calculate $\alpha$ (HOOC-CH(CH₃)NH₃⁺)at pH 3.

Of the following,which does not have an amphoteric oxide?

Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

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Exam 12: Acids and Bases

For a solution labeled "0.10 M H2SO4(aq),"

What is the [H+] for a solution labeled "0.0500 M H2SO3(aq)" if pKa1 = 1.81,and pKa2 = 6.91?

The fractional composition diagram for the amino acid alanine is shown below. What do the two points represent where alpha is 0.5?

What is the pKa of the conjugate acid of hydrazine,given that the pKb of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

All of the following are Lewis bases except

the pH of 0.10 M and 0.40 M NaHCO3(aq)solutions is 8.31 for both?

A 0.0010 M solution of a weak acid,HA,with Ka = 2 * 10-10 produces [H3O+] < 10-6 M.Which of the following equations can be used to determine [H3O+]?

Calculate the hydroxide ion concentration for an aqueous solution that has a pH of 3.45.

The equation that represents Ka2 for phosphoric acid is

Calculate the hydrogen ion concentration for an aqueous solution that has a pH of 3.45.

The conjugate acid of HPO42- is

All of the following 0.1 M aqueous solutions are acidic except

If the pKa of acetic acid is 4.75,the pKa of CH3CH2OH is

The Ka of phenol is 1.3 * 10-10.For a solution labeled "1.0 *10-3 M aqueous phenol,"

Which of the following is not a Lewis acid?

The conjugate base of OH- is

The amino acid alanine,HOOC-CH(CH3)NH3+,has Ka1 = 4.5 * 10-3 and Ka2 = 1.4 * 10-10.Calculate α\alphaα (HOOC-CH(CH3)NH3+)at pH 3.

Of the following,which does not have an amphoteric oxide?

Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Chemical Equilibria

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

Filters

For a solution labeled "0.10 M H₂SO₄(aq),"

What is the [H⁺] for a solution labeled "0.0500 M H₂SO₃(aq)" if pK_a1 = 1.81,and pK_a2 = 6.91?

The fractional composition diagram for the amino acid alanine is shown below. $The fractional composition diagram for the amino acid alanine is shown below. What do the two points represent where alpha is 0.5?$ What do the two points represent where alpha is 0.5?

What is the pK_a of the conjugate acid of hydrazine,given that the pK_b of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

the pH of 0.10 M and 0.40 M NaHCO₃(aq)solutions is 8.31 for both?

A 0.0010 M solution of a weak acid,HA,with K_a = 2 * 10^-10 produces [H₃O⁺] < 10^-6 M.Which of the following equations can be used to determine [H₃O⁺]?

The equation that represents K_a2 for phosphoric acid is

The conjugate acid of HPO₄^2- is

If the pK_a of acetic acid is 4.75,the pK_a of CH₃CH₂OH is

The K_a of phenol is 1.3 * 10^-10.For a solution labeled "1.0 *10^-3 M aqueous phenol,"

The conjugate base of OH^- is

The amino acid alanine,HOOC-CH(CH₃)NH₃⁺,has K_a1 = 4.5 * 10^-3 and K_a2 = 1.4 * 10^-10.Calculate $\alpha$ (HOOC-CH(CH₃)NH₃⁺)at pH 3.