Question 1

HClO4 is a strong acid, therefore ClO4- must be a _____ base

Accepted Answer

weak

Question 2

What is the hydrogen ion concentration of a can of cola with pH = 2.77?

Accepted Answer

A)  588 mol dm-3 
B)  2.34 x 10-3 mol dm-3 
C)  0.56 x 10-3 mol dm-3 
D)  1.70 x 10-3 mol dm-3 
A)  588 mol dm-3 
B)  2.34 x 10-3 mol dm-3 
C)  0.56 x 10-3 mol dm-3 
D)  1.70 x 10-3 mol dm-3 D

Question 3

HF has the ability to dissolve glass, it is a _____ acid.

Accepted Answer

weak

Question 4

In water the H+ ion is always hydrated and found as the H3O+ ion.

Accepted Answer

A) True 
 B)False

Question 5

The strength of an oxoacid, HmXOn containing m hydroxide groups and (n - m) double bonded oxygen atoms is related to?

Accepted Answer

A)  n 
B)  n - m 
C)  n + m 
D)  m 
A)  n 
B)  n - m 
C)  n + m 
D)  m

Question 6

Identify the type of species highlighted in red in the following equation:
NH3 (aq) + HF (aq) ⇌ NH4+ (aq) + F- (aq)
Please select all that apply.

Accepted Answer

A)  Arrhenius base 
B)  Brønsted-Lowry acid 
C)  Arrhenius acid 
D)  Brønsted-Lowry base 
A)  Arrhenius base 
B)  Brønsted-Lowry acid 
C)  Arrhenius acid 
D)  Brønsted-Lowry base

Question 7

A buffer can be made from a weak base and the ____ of that base.

Accepted Answer

The answer of A buffer can be made from a...

Question 8

What is the pH of a buffer solution containing 0.155 mol dm-3 of benzoic acid and 0.315 mol dm-3 sodium benzoate. (Ka of benzoic acid is 4.20.)

Accepted Answer

A)  0.50 
B)  -0.50 
C)  3.89 
D)  4.51 
A)  0.50 
B)  -0.50 
C)  3.89 
D)  4.51

Question 9

The pH of a 0.111 mol dm-3 HCO2H solution at 298 K is 0.95.

Accepted Answer

A) True 
 B)False

Question 10

Which of the following statements apply to a weak acid?

Accepted Answer

A)  In the equilibrium equation:
HA (aq) + H2O (l) ⇌ A- (aq) + H3O+ (aq)
The equilibrium lies almost entirely to the right. 
B)  pKa is less than 0. 
C)  The pH would be greater than zero. 
D)  The pH would be less than zero. 
A)  In the equilibrium equation:
HA (aq) + H2O (l) ⇌ A- (aq) + H3O+ (aq)
The equilibrium lies almost entirely to the right. 
B)  pKa is less than 0. 
C)  The pH would be greater than zero. 
D)  The pH would be less than zero.

Question 11

The conjugate acid of H2PO4- is H3PO4.

Accepted Answer

A) True 
 B)False

Question 12

Kw falls with temperature as the self-ionization of water is exothermic.

Accepted Answer

A) True 
 B)False

Question 13

Water can be described as amphoteric as it can be both a proton donor and a proton acceptor.

Accepted Answer

A) True 
 B)False

Question 14

Which of the following indicators would be suitable for the titration of HCO2H with sodium hydroxide?

Accepted Answer

A)  Phenolphthalein 
B)  Methyl orange 
C)  Bromocresol blue 
D)  Thymol blue 
A)  Phenolphthalein 
B)  Methyl orange 
C)  Bromocresol blue 
D)  Thymol blue

Question 15

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated.
-H3PO4

Accepted Answer

A)  H2PO4- 
B)  NH2- 
C)  H3SO3+ 
D)  H3O+ 
A)  H2PO4- 
B)  NH2- 
C)  H3SO3+ 
D)  H3O+

Question 16

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated.
-NH3

Accepted Answer

A)  H2PO4- 
B)  NH2- 
C)  H3SO3+ 
D)  H3O+ 
A)  H2PO4- 
B)  NH2- 
C)  H3SO3+ 
D)  H3O+

Question 17

Which of the following statements are true when referring to a buffer solution? Please select all that apply.

Accepted Answer

A)  A buffer can consist of a weak acid and its salt. 
B)  A buffer solution is resistant to addition of small quantities of acid. 
C)  A buffer can consist of a weak base and its salt. 
D)  A buffer solution is resistant to addition of small quantities of base. 
A)  A buffer can consist of a weak acid and its salt. 
B)  A buffer solution is resistant to addition of small quantities of acid. 
C)  A buffer can consist of a weak base and its salt. 
D)  A buffer solution is resistant to addition of small quantities of base.

Question 18

Choose which expression for the equilibrium constant for the reaction of water with perchloric (HClO4) acid is correct.

Accepted Answer

A)  $K_{\mathrm{a}}=\frac{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}{\left[\mathrm{HClO}_{4}\right]}$ 
B)  $K_{\mathrm{a}}=\frac{\left[\mathrm{HClO}_{4}\right]}{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}$ 
C)  $K_{\mathrm{c}}=\frac{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}{\left[\mathrm{H}_{2} \mathrm{O}\right]}$ 
D)  $K_{a}=\frac{\left[\mathrm{HClO}_{4}\right]\left[\mathrm{H}_{2} \mathrm{O}\right]}{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}$ 
A)  $K_{\mathrm{a}}=\frac{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}{\left[\mathrm{HClO}_{4}\right]}$ 
B)  $K_{\mathrm{a}}=\frac{\left[\mathrm{HClO}_{4}\right]}{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}$ 
C)  $K_{\mathrm{c}}=\frac{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}{\left[\mathrm{H}_{2} \mathrm{O}\right]}$ 
D)  $K_{a}=\frac{\left[\mathrm{HClO}_{4}\right]\left[\mathrm{H}_{2} \mathrm{O}\right]}{\left[\mathrm{ClO}_{4}^{-}\right]\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}$

Question 19

The position of neutral pH on the pH scale changes with temperature.

Accepted Answer

A) True 
 B)False

Question 20

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated.
-H2SO3

Accepted Answer

A)  H2PO4- 
B)  NH2- 
C)  H3SO3+ 
D)  H3O+ 
A)  H2PO4- 
B)  NH2- 
C)  H3SO3+ 
D)  H3O+

Exam 7: Acids and Bases

HClO4 is a strong acid, therefore ClO4- must be a _____ base

What is the hydrogen ion concentration of a can of cola with pH = 2.77?

HF has the ability to dissolve glass, it is a _____ acid.

In water the H+ ion is always hydrated and found as the H3O+ ion.

The strength of an oxoacid, HmXOn containing m hydroxide groups and (n - m) double bonded oxygen atoms is related to?

Identify the type of species highlighted in red in the following equation: NH3 (aq) + HF (aq) ⇌ NH4+ (aq) + F- (aq) Please select all that apply.

A buffer can be made from a weak base and the ____ of that base.

What is the pH of a buffer solution containing 0.155 mol dm-3 of benzoic acid and 0.315 mol dm-3 sodium benzoate. (Ka of benzoic acid is 4.20.)

The pH of a 0.111 mol dm-3 HCO2H solution at 298 K is 0.95.

Which of the following statements apply to a weak acid?

The conjugate acid of H2PO4- is H3PO4.

Kw falls with temperature as the self-ionization of water is exothermic.

Water can be described as amphoteric as it can be both a proton donor and a proton acceptor.

Which of the following indicators would be suitable for the titration of HCO2H with sodium hydroxide?

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated. -H3PO4

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated. -NH3

Which of the following statements are true when referring to a buffer solution? Please select all that apply.

Choose which expression for the equilibrium constant for the reaction of water with perchloric (HClO4) acid is correct.

The position of neutral pH on the pH scale changes with temperature.

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated. -H2SO3

Fundamentals

The Language of Organic Chemistry

Atomic Structure and Properties

Diatomic Molecules

Polyatomic Molecules

Solids

Gases

Reaction Kinetics

Molecular Spectroscopy

Analytical Chemistry

Molecular Characterisation

Energy and Thermochemistry

Entropy and Gibbs Energy

Electrochemistry

Phase Equilibrium and Solutions

Isomerism and Stereochemistry

Organic Reaction Mechanisms

Halogenoalkanes: Substitution and Elimination Reactions

Alkenes and Alkynes: Electrophilic Addition and Pericyclic Reactions

Benzene and Other Aromatic Compounds: Electrophilic Substitution Reactions

Aldehydes and Ketones: Nucleophilic Addition and Α-Substitution Reactions

Carboxylic Acids and Derivatives: Nucleophilic Acyl Substitution and Α-Substitution Reactions

Hydrogen

S-Block Chemistry

P-Block Chemistry

D-Block Chemistry

Filters

HClO₄ is a strong acid, therefore ClO₄^- must be a _____ base

In water the H⁺ ion is always hydrated and found as the H₃O⁺ ion.

The strength of an oxoacid, H_mXO_ncontaining m hydroxide groups and (n - m) double bonded oxygen atoms is related to?

Identify the type of species highlighted in red in the following equation: NH₃(aq) + HF(aq) ⇌ NH₄⁺(aq) + F^-(aq) Please select all that apply.

What is the pH of a buffer solution containing 0.155 mol dm^-3 of benzoic acid and 0.315 mol dm^-3 sodium benzoate. (K_a of benzoic acid is 4.20.)

The pH of a 0.111 mol dm^-3 HCO₂H solution at 298 K is 0.95.

The conjugate acid of H₂PO₄^- is H₃PO₄.

K_wfalls with temperature as the self-ionization of water is exothermic.

Which of the following indicators would be suitable for the titration of HCO₂H with sodium hydroxide?

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated. -H₃PO₄

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated. -NH₃

Choose which expression for the equilibrium constant for the reaction of water with perchloric (HClO₄) acid is correct.

Many solvents self ionize to form an anion and cation that are the Brønsted- Lowry base and acid of the original solvent. Match the ions with the solvent from which they are generated. -H₂SO₃