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WorksheetsAcid Base BL quiz
Total questions: 14
Worksheet time: 7mins
1. A student dissolves 4.0 g of NaOH(s) to make 1.0 L of NaOH solution and then predicts the [H3O+(aq)] of the solution. The best prediction is ______________ mol/L
1.0 x 10-14
1.0 x 10-13
1.0 x 10-7
1.0 x 10-1
1. An acidic solution may be operationally defined as one that
is nonelectrolytic
reacts with zinc
neutralizes CH3COOH
tastes bitter
A solution of an unknown substance has [H3O+(aq)] = 4 x 10-8 mol/L. If HCl solution is added drop by drop, the pH
increases and the solution becomes more basic
decreases and the solution becomes more basic
increases and the solution becomes more acidic
decreases and the solution becomes more acidic
A solution of 0.0300 mol/L HI(aq) has a pH of
2.48
2.00
1.52
0.480
The pH of a 0.001 mol/L LiOH solution is
3
7
10
11
The pH of 0.10 mol/L NaNO2(aq) will be:
less than 7.00
7.00
greater than 7.00
greater than 14.00
As a solution becomes more basic, the
[H3O+(aq)] decreases and the pH increases
[H3O+(aq)] decreases and the pH decreases
[H3O+(aq)] increases and the pH increases
[H3O+(aq)] increases and the pH decreases
In the reaction HSO3-(aq) + NH3(aq) ↔ NH4+(aq) + SO32-(aq), both
HSO3-(aq) and NH4+(aq) act as acids
HSO3-(aq) and SO32-(aq) act as acids
HSO3-(aq) and NH4+(aq) act as bases
NH3(aq) and NH4+(aq) act as bases
Use the following reactions to answer question 2.
1) HCO3-(aq) + HSO3-(aq) ⇌ H2CO3(aq) + SO32-(aq)
2) HSO3-(aq) + PO43-(aq) ⇌ HPO42-(aq) + SO32-(aq)
3) HCO3-(aq) + HS-(aq) ⇌ CO32-(aq) + H2S(aq)
Identify the substance that behaves as both an acid and a base.
HPO42-(aq)
HSO3-(aq)
HS-(aq)
HCO3-(aq)
In the chemical equation NH3(aq) + H2O(l) ↔ NH4+(aq) + OH-(aq), a Bronsted-Lowry conjugate acid-base pair is
NH4+(aq) , H2O(l)
H2O(l), OH-(aq)
NH3(aq) , H2O(l)
NH4+(aq) , OH-(aq)
Use the following information to answer question 4.
When rainwater falls, it can become slightly acidic
due to the presence of combustion products in the atmosphere. A pH recording of 5.6 for rainwater is
not uncommon.
The Bronsted-Lowry equation that explains the acidic nature of rainwater is
CO2(g) + 2H2O(l) ↔ H3O+(aq) + HCO3-(aq)
2H2O(l) ↔ H3O+(aq) + OH-(aq)
2H2O(l) ↔ O2(g) + 4H+(aq)
CO2(g) + H2O(l) ↔ OH-(aq) + HCO2-(aq)
Which of the following is amphiprotic?
NH4+(aq)
HSO3-(aq)
HNO2(aq)
SO32-(aq)
The equation that does NOT represent a Bronsted-Lowry acid-base reaction is
H2O(l) + H2O(l) ↔ H3O+(aq) + OH-(aq)
HS-(aq) + HSO4-(aq) ↔ H2S(aq) + SO42-(aq)
2Cl-(aq) + 2H2O(l) ↔ H2(g) + Cl2(g) + 2OH-(aq)
HCl(aq) + HCO3-(aq) ↔ H2CO3(aq) + Cl-(aq)
In the equation H2SO4(aq) + CH3COO(aq) ↔ CH3COOH(aq) + HSO4-(aq) ,
the Bronsted-Lowry bases are
CH3COOH(aq) and CH3COO-(aq)
CH3COO-(aq) and HSO4-(aq)
CH3COOH(aq) and HSO4-(aq)
H2SO4(aq) and CH3COOH(aq)
