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WorksheetsAcids, Bases, pH, Molarity & Dilutions
Total questions: 58
Worksheet time: 3hrs 29mins
Name
Class
Date
1.
Write a balanced equation for the neutralization of:
copper (III) hydroxide + sulfuric acid
copper (III) hydroxide + sulfuric acid
a)
2 Cu(OH)3 + 3 H2SO4 → 1 Cu2(SO4)3 + 6 H2O
b)
2 Cu(OH)3 + 3 H2SO4 → 1 CuSO4 + 3 H2O
c)
2 Cu(OH)3 + 3 H2S→ 2 CuS + 6 H2O
2.
Write a balanced chemical equation for the neutralization of :
nitrous acid + aluminum hydroxide→
a)
3 HNO2 + 1 Al(OH)3 → 1 Al(NO2)3 + 3 H2O
b)
1HNO3 + 1 Al(OH)3 → 1 AlNO3 + 1 H2O
c)
3 HNO3 + 1 Al(OH)3 → 1 Al(NO3)3 + 3 H2O
3.
Is corrosive with metals
a)
acid
b)
base
c)
salt
d)
acid or base
4.
calcium hydroxide
a)
acid
b)
salt
c)
acid or base
d)
base
5.
Contains neither hydrogen ions or hydroxide ions
a)
acid
b)
base
c)
salt
d)
acid or base
6.
Feels slippery in solution
a)
acid
b)
base
c)
salt
d)
acid or base
7.
Has a sour taste.
a)
acid
b)
base
c)
salt
d)
acid or base
8.
Conducts electrical current.
a)
acid
b)
base
c)
salt
d)
acid, base, or salt
9.
Made from an acid and a base
a)
salt
b)
acid
c)
base
d)
acid, base, or salt
10.
Reacts with an indicator to produce a color change.
a)
acid
b)
base
c)
salt
d)
acid or base
11.
How much 18 M nitric acid is need to prepare a 6.0 M solution of 250 mL?
(M1V1 = M2V2)
(M1V1 = M2V2)
a)
0.750 L
b)
75 L
c)
83.3 L
d)
0.083L
12.
Which model states tha an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions?
a)
Lewis
b)
Arrhenius
c)
Hydrogen
d)
Brønsted-Lowry
13.
A _?_ base is a substance that produces hydroxide ions in solution.
a)
Arrhenius
b)
conjugate
c)
Brønsted-Lowry
d)
Lewis
14.
How is the concentration of an acid or base different from the strength of an acid or base?
a)
Strength refers to the amount of acid or base dissolved in solution. Concentration refers to how well the acid or base ionizes in solution.
b)
Concentration refers to the amount of acid or base dissolved in solution. Strength refers to how well the acid or base ionizes in solution.
15.
Identify the Bronsted-Lowry acid and conjugate base pair in the equation:
H2SO4 + H2O ---> H3O+1 + HSO4-1
H2SO4 + H2O ---> H3O+1 + HSO4-1
a)
H2SO4 + HSO4-1
b)
H2SO4 + H3O+1
c)
H2O + H3O+1
d)
H2O + HSO4-1
16.
Determine the identity of HPO4-2:
H2PO4-1 + OH -1 → H2O + HPO4-2
H2PO4-1 + OH -1 → H2O + HPO4-2
a)
Brønsted-Lowry acid
b)
Brønsted-Lowry base
c)
conjugate acid
d)
conjugate base
17.
_?_ of a solution refers to the ease with which an acid or base forms ions in solution.
a)
Concentration
b)
Strength
c)
pH
d)
Acidity
18.
What is meant by a "weak acid"?
a)
Its hydrogen ions only partially ionize in solution.
b)
Its hydroxide ions only partially ionize in solution.
c)
Its hydrogen ions completely ionize in solution.
d)
Its hydroxide ions completely ionize in solution.
19.
An acid can be defined as _?_
a)
a proton donor.
b)
neither a proton donor nor a proton acceptor.
c)
a proton acceptor
d)
both a proton donor and a proton acceptor.
20.
Why is hydrochloric acid stronger than hydrofluoric acid?
a)
HCl completely ionizes in solution.
b)
HCl doesn't completely ionize in solution.
c)
Hydrofluoric acid completely ionizes in solution.
21.
Ammonia is a weak base because it produces _?_ ions in solution.
a)
strong
b)
only a few
c)
weak
d)
many
22.
Sulfuric acid is a strong acid because it produces _?_ ions in solution.
a)
strong
b)
only a few
c)
weak
d)
many
23.
What is the pH of milk given the hydrogen ion concentration is 9.80 x 10-9 M?
a)
8.00
b)
1.00
c)
6.00
d)
cannot be determined
24.
The pH scale allows scientists to define the acidity of a substance on a scale of _?_.
a)
0-14
b)
1-14
c)
0-7
d)
7-14
25.
Calculate the [H+] concentration of a solution, given the concentration of [OH-]= 1 x 10-9 M.
a)
1 x 10-5 M
b)
1 x 10-14 M
c)
9
d)
5
26.
If the pOH is 5.60, what is the hydrogen ion concentration?
a)
3.98 x 10-9 M
b)
2.51 x 10-6 M
c)
7.48 x 10-1 M
27.
An aqueous solution has a pOH of 5.6. What is the pH?
a)
8.4
b)
2.5 x 10
c)
2.5 x 108 M
d)
-6
28.
Determine the [H+] concentration of 0.850 M LiOH solution.
a)
1.25 x 10-14 M
b)
1.17x 10-14M
c)
7.11 x 10-2 M
29.
If the [H3O+1] > [OH-1] the solution is...
a)
acidic
b)
basic
c)
neutral
30.
If the [H3O+1] < [OH-1] the solution is...
a)
acidic
b)
basic
c)
neutral
31.
If the [H3O+1] = [OH-1] the solution is...
a)
acidic
b)
basic
c)
neutral
32.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
33.
Which is an acid?
a)
Turns blue litmus red
b)
Turns red litmus blue
c)
Has a pH of 11
d)
Has a pH of 7
34.
Which of these substances is acidic?
a)
tap water
b)
lemon
c)
ammonia
d)
baking soda
35.
According to ___________________, a base is any substance with an increased concentration of OH- ions.
a)
Ahrrenius
b)
Brønsted-Lowry
c)
Lewis
d)
Newman-Wrightøø
36.
According to ___________________, a base is any substance that accepts a proton.
a)
Ahrrenius
b)
Bronsted-Lowry
c)
Lewis
d)
Newman-Wright
37.
A ______________ acid can only donate one proton.
a)
Monoprotic
b)
Polyprotic
c)
Diprotic
d)
Triprotic
38.
A ______________ acid can donate 2 protons.
a)
Monoprotic
b)
Polyprotic
c)
Diprotic
d)
Triprotic
39.
The Kw constant is:
a)
1.0 x 10-14
b)
1.0 x 1014
c)
6.022 x 1023
d)
6.0634 x 10-34
40.
A reaction in which H+ and OH- cancel each other out is known as a __________________ reaction.
a)
Neutralization
b)
Combustion
c)
Single Replacement
d)
Synthetic
41.
What is the conjugate base in the following reaction?
a)
HCO3-
b)
HCl
c)
H2CO3
d)
Cl-
42.
If a solution has a [H+] of 1.2 x 10-4M what is the [OH-]?
a)
8.3 x 10-4M
b)
8.3 x 10-11M
c)
1.2 x 1010M
d)
1.2 x 10-4M
43.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.0 x 10-4 M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
44.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
45.
Which donates protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
46.
Find the molarity of 186.55 g of sucrose, C12H22O11 in 250 mL of water.
(M = mol solute/ L solution)
(M = mol solute/ L solution)
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
47.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
(M = mol solute/ L solution)
(M = mol solute/ L solution)
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
48.
How many grams of AgNO3 are needed to prepare 0.125M solution in 250 mL of water?
(M = mol solute/ L solution)
(M = mol solute/ L solution)
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
49.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
(M1V1 = M2V2)
(M1V1 = M2V2)
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
50.
You have 286.7g of PbO. For lab, you need 2.50M PbO. How many mL of PbO solution can you make?
(M = mol solute/ L solution)
(M = mol solute/ L solution)
a)
114.7 mL
b)
554 mL
c)
514 mL
d)
3.21 L
51.
How many grams of calcium hydroxide are needed to produce 500. ml of 1.66 M calcium hydroxide solution?
(M = mol solute/ L solution)
(M = mol solute/ L solution)
a)
38.7 g
b)
61.5 g
c)
94.0 g
d)
19.7 g
52.
What are the products of the following reaction?
H2SO4 + KOH -->
H2SO4 + KOH -->
a)
HK + HSO4
b)
H2O + KSO4
c)
H2O + K2SO4
d)
H2 + K2SO4
53.
Complete the following reaction:
Hydrochloric acid + magnesium hydroxide -->
Hydrochloric acid + magnesium hydroxide -->
a)
Magnesium chloride + water
b)
Magnesium + water
c)
Magnesium chloride + hydrogen gas
d)
Magnesium chloride + water + carbon dioxide
54.
What might happen if you mixed a strong acid with an equally strong base?
a)
You would see an explosive chemical reaction.
b)
The acid would destroy the base.
c)
The base would destroy the acid.
d)
You'd wind up with a pH-neutral substance.
55.
A neutralization reaction will always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
56.
What are the products of the neutralization shown below?
Calcium hydroxide + carbonic acid —>
Calcium hydroxide + carbonic acid —>
a)
H2O + Ca2CO3
b)
CaO + CO3
c)
H2O + CaCO3
57.
In the first graph, what strength base is used with the titration of a strong acid?
a)
strong base
b)
weak base
58.
In the second graph, what strength base is used in the titration with a weak acid?
a)
strong base
b)
weak base
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