Question 1

Which one of the following solutions would have the highest pH?

Accepted Answer

1.0 mol/L sodium hydroxide

Answer

1.0 mol/L ammonium chloride

Answer

1.0 mol/L ethanoic acid

Answer

1.0 mol/L hydrochloric acid

Question 2

Which one of the following represents a concentrated solution of a weak acid?

Accepted Answer

6.0 mol/L $CH_3COOH$

Answer

0.01 mol/L $CH_3COOH$

Answer

0.01 mol/L HCl

Answer

6.0 mol/L HCl

Question 3

Which one of the following is the conjugate base of $OH^-?$

Accepted Answer

$O^{2-}$

Answer

$H_3O^+$

Answer

$H_2O$

Answer

NaOH

Question 4

Which one of the following can act as either a Bronsted-Lowry acid or base in aqueous solutions?

Accepted Answer

$HS^-$

Answer

$CO_3^{2-}$

Answer

$NH_4^+$

Answer

$CH_4$

Question 5

Which of the following acids can be classified as polyprotic in the water?
$CH_3COOH$, $H_2SO_3$, $NH_4^+$

Accepted Answer

$H_2SO_3$ only

Answer

$CH_3COOH$ and $H_2SO_3$ only

Answer

All three acids

Answer

$CH_3COOH$ only

Question 6

Consider the following statements, which compare 20.00 mL of a 0.10 mol/L solution of nitric acid with 20.00 mL of a 0.10 mol/L solution of ethanoic acid.
I. Both solutions have the same strength.
II. The pH of the nitric acid solution is higher
III. The electrical conductivity of the nitric acid solution is higher
IV. Both solutions require the same volume of 0.10 mol/L NaOH for neutralization

Accepted Answer

III and IV

Answer

I and II

Answer

II and IV

Answer

I and III

Question 7

Beakers X and Y both contain nitric acid. The pH of the acid in beaker X is 3 whereas the pH of the acid in beaker Y is 1. From this information, what can be deduced about the concentration of hydrogen ions in beaker X?

Accepted Answer

It is one-hundredth of that in beaker Y

Answer

It is one hundred times that in beaker Y

Answer

It is three times that in beaker Y

Answer

It is one-third of that in beaker Y

Question 8

A solution of NaOH has a pH of 13 at $25^0C$. What mass of sodium hydroxide is present in 500 mL of this solution?

Accepted Answer

2.0 g

Answer

4.0 g

Answer

0.050 g

Answer

$2.0x10^{-12}$ g

Question 9

Since the mid-1700s the pH of the world’s oceans has changed from 8.2 to 8.1. Which of the following substances is the main cause of this change?

Accepted Answer

$CO_2$

Answer

$SO_2$

Answer

$CaCO_3$

Answer

$H_2SO_4$

Question 10

Which of the following represents a conjugate acid-base pair?

Accepted Answer

$NH_4^+/NH_3$

Answer

$NH_3/NH_2^-$

Answer

$NH_4/NH_3^+$

Answer

$NH_3/NH^{2-}$

Question 11

The salt lithium sulfate could be formed from the neutralization reaction between which two compounds?

Accepted Answer

Sulfuric acid and lithium hydroxide

Answer

Lithium hydroxide and nitric acid

Answer

Sodium carbonate and lithium hydroxide

Answer

Sodium sulfate and lithium sulfate

Question 12

Which of the following is an example of a dilute solution of a strong acid?

Accepted Answer

0.001 mol/L $H_2SO_4$

Answer

0.001 mol/L $CH_3COOH$

Answer

2.0 mol/L $CH_3COOH$

Answer

2.0 mol/L $H_2SO_4$

Question 13

Select the alternative that correctly describes a basic solution.

Accepted Answer

$[H_3O^+]$ < $10^{-7}$ mol/L, pH > 7, pOH < 7

Answer

$[H_3O^+]$ < $10^{-7}$ mol/L, pH < 7, pOH > 7

Answer

$[H_3O^+]$ > $10^{-7}$ mol/L, pH < 7, pOH < 7

Answer

$[H_3O^+]$ > $10^{-7}$ mol/L, pH > 7, pOH < 7

Question 14

50 mL of 0.020 mol/L NaOH solution at $25^0C$ is made up to 100 mL with deionized water. What is the pOH value of the diluted solution?

Accepted Answer

2.00

Answer

12.00

Answer

12.60

Answer

1.40

Question 15

The following table shows the labels on four different solutions.
Arrange the solutions in order of least acidic to most acidic.

Accepted Answer

Y X W Z

Answer

Z W X Y

Answer

Y Z W X

Answer

Y W X Z

Question 16

The expression for the acidity constant of a particular weak acid is
		$K_a$ = $[H_3O^+][HCOO^-]$ / [HCOOH]
This expression is the acidity constant for which one of the following reactions?

Accepted Answer

HCOOH(aq) + $H_2O(l)$ ⇌ $H_3O^+(aq)$ + $HCOO^-(aq)$

Answer

$H_3O^+(aq)$ + $HCOO^-(aq)$ ⇌ HCOOH(aq) + $H_2O(l)$

Answer

HCOOH(aq) + $H_2O(l)$ → $H_3O^+(aq)$ + $HCOO^-(aq)$

Answer

HCOOH(aq) ⇌ $H_3O^+(aq)$ + $HCOO^-(aq)$

Question 17

The equilibrium present in the ethanoic acid/ethanoate buffer is
$CH_3COOH(aq)$ + $H_2O(l)$ ⇌ $CH_3COO^-(aq)$ + $H_3O^+(aq)$
When a small amount of NaOH is added to this system, which of the following will occur?

Accepted Answer

The $OH^-$ ions will react with the $CH_3COOH$, producing more $CH_3COO^-$ ions.

Answer

The $OH^-$ ions will react with the $CH_3COO^-$ ions to make $CH_3COOH$

Answer

The $Na^+$ ions will react with the $CH_3COOH$ to form NaOH

Answer

The $OH^-$ ions will react with the water to form more $H_3O^+$ ions.

Question 18

The following acid-base titration curve shows the way pH changes when a base is added from a burette to a measured volume of acid. The concentration of both acid and base is 0.1 mol/L.
From the shape of the curve, what can be deduced about the relative strength of the acid and base?

Accepted Answer

The acid is weak and base is strong

Answer

The acid is strong and the base is strong

Answer

The acid weak and the base is weak

Answer

The acid is strong and the base is weak

Question 19

The following acid-base titration curve shows the way pH changes when a base is added from a burette to a measured volume of acid. The concentration of both acid and base is 0.1 mol/L.
Which one or more of the following indicators could be used for this titration?

Accepted Answer

phenolphthalein only

Answer

methyl orange only

Answer

bromothymol blue only

Answer

methyl orange and methyl red only

Question 20

A standard solution of HCl is titrated four times against some NaOH. The following titres are obtained: 21.05 mL, 20.75 mL, 20.65 mL, 20.75 mL.
The average titre is then calculated and used to determine the concentration of NaOH. The correct value for the average titre is:

Accepted Answer

20.72 mL

Answer

20.80 mL

Answer

20.65 mL

Answer

20.75 mL

Question 21

The self-ionization of water is affected by temperature, as shown below.
$H_2O(l)$ + $H_2O(l)$ ⇌ $H_3O+(aq)$ + $OH^-(aq)$ $K_w$ = $[H_3O^+][OH^-]$
What can be inferred from this data?

Accepted Answer

Equilibrium for the reaction lies well to the left with mainly reactants present.

Answer

Self-ionization of water is an exothermic reaction.

Answer

The pH of pure water at $35^0C$ is greater than 7.

Answer

In pure water at 150C, $[OH^-]$ is lower than $[H_3O^+]$

Related quizzes

Related quizzes