WorksheetsChapter 8 - Acids and Bases SL
Total questions: 20
Worksheet time: 13mins
Which pH value is that of an aqueous solution of carbon dioxide?
2.1
5.6
9.8
12.2
At 25°C, Ka for an acid is 1.0 x 10-2. What is the value of Kb for its conjugate base?
1.0 x 102
1.0 x 10-2
1.0 x 1012
1.0 x 10-12
Which substance, when dissolved in water, to give a 0.1 mol/dm3 solution, has the highest pH?
HCl
NaCl
NH3
NaOH
Which methods will distinguish between equimolar solutions of a strong base and a strong acid?
I. Add magnesium to each solution and look for the formation of gas bubbles II. Add aqueous sodium hydroxide to each solution and measure the temperature change III. Use each solution in a circuit with a battery and lamp and see how bright the lamp glows
I and II only
I and III only
II and III only
I, II, and III
If 20 cm3 samples of 0.1 mol dm-3 solutions of the acids below are taken, which acid would require a different volume of 0.1 mol dm-3 sodium hydroxide for complete neutralization?
Nitric acid
Sulfuric acid
Ethanoic acid
Hydrochloric acid
What is the formula for the conjugate base of the hydrogenphosphate ion, HPO42-?
H2PO4-
H3PO4
HPO4-
PO43-
Which list contains only strong acid?
CH3COOH, H2CO3, H3PO4
HCl, HNO3, H2CO3
CH3COOH, HNO3, H2SO4
HCl, HNO3, H2SO4
Ammonia acts as a weak base when it reacts with water. What is the Kb expression for this reaction?
[NH4+][OH-]/[NH3][H2O]
[NH3][H2O]/[NH4+][OH-]
[NH3]/[NH4+][OH-]
[NH4+][OH-]/[NH3]
100 cm3 of a NaOH solution of pH 12 is mixed with 900 cm3 of water. What is the pH of the resulting solution?
1
3
11
13
An example of a strong acid solution is perchloric acid, HClO4, in water. Which statement is correct for this solution?
HClO4 is completely dissociated in the solution
HClO4 exists mainly as molecules in the solution
The solution reacts only with strong bases
The solution has a pH value greater than 7
What is the approximate pH of a 0.01 mol dm-3 ammonia solution?
2
More than 2 but less than 7
More than 7 but less than 12
12
Which are definitions of an acid according to the Bronsted-Lowry and Lewis theories?
Bronsted-Lowry theory is a proton donor, Lewis theory is electron pair acceptor
Bronsted-Lowry theory is a proton acceptor, Lewis theory is electron pair acceptor
Bronsted-Lowry theory is a proton acceptor, Lewis theory is electron pair donor
Bronsted-Lowry theory is a proton donor, Lewis theory is electron pair donor
What is the correct expression for the ionic product constant of water, Kw?
[H+]/[OH-]
[H2O]/[H+][OH-]
[H+] + [OH-]
[H+][OH-]
When equal volumes of four 0.1 mol dm-3 solutions are arranged in order of increasing pH (lowest pH first) what is the correct order?
CH3COOH < HNO3 < CH3CH2NH2 < KOH
HNO3 < CH3COOH < CH3CH2NH2 < KOH
CH3CH2NH2 < HNO3 < CH3COOH < KOH
KOH < CH3CH2NH2 < CH3COOH < HNO3
For equal volumes of 1.0 mol dm-3 solutions of hydrochloric acid, HCl, and methanoic acid, HCOOH, which statements are correct?
I. HCl dissociates more than HCOOH II. HCl is a better electrical conductor than HCOOH III. HCl will neutralize more NaOH than HCOOH
I and II only
I and III only
II and III only
I, II, and III
A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must be correct?
Acid A is stronger than acid B
[A] > [B]
The concentration of H+ ions in A is higher than in B
The concentration of H+ ions in B is twice the concentration of H+ ions in A
Which of the following are weak acids in aqueous solution?
I. CH3COOH II. H2CO3 III. HCl
I and II only
I and III only
II and III only
I, II, and III
Which species behave as Bronsted-Lowry acids in the following reversible reaction?
H2PO4-(aq) + CN-(aq) ↔ HCN(aq) + HPO42-(aq)
HCN and CN-
HCN and HPO42-
H2PO4- and HPO42-
HCN and H2PO42-
What is the pH at the equivalence point.
The pH is approximately 5
The pH is approximately 6
The pH is approximately 8
The pH is approximately 9
