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6. Basic Chemistry: Reaction in Aqueous Solution

Total questions: 25

Worksheet time: 3hrs 37mins

Name
Class
Date
1.

Tono and Budi are conducting a chemistry experiment. They are observing a reaction where one reactant loses electrons and the other gains them. What type of reaction are they observing?

a)
Synthesis reaction
b)

Neutralization reaction

c)

Precipitation reaction

d)
Acid-base reaction
e)
Redox reaction
2.

Reduction is a process in a chemical reaction. What reduction reaction is?

a)

Reduction reaction is the process where a substance destroys electrons during a chemical reaction.

b)
A reduction reaction involves the loss of electrons by a chemical species.
c)
A reduction reaction involves the gain of electrons by a chemical species.
d)

Reduction reaction is the process where a substance creates electrons during a chemical reaction.

e)
A reduction reaction involves the release of electrons by a chemical species.
3.

What is the meaning of oxidation in redox reaction?

a)
Gain of electrons
b)

The destruction of electrons.

c)
Increase in mass
d)

The creation of electrons.

e)
Loss of electrons
4.

An aqueous solution is .........................

a)
a solution that contains oil as the solvent
b)
a solution that is solid at room temperature
c)
a solution in which the solvent is water
d)

any liquid with another compound dissolved in it

e)

an ionic compound with water dissolved in it

5.

Which of the following compounds is soluble?

a)

potassium carbonate

b)

copper carbonate

c)

aluminium carbonate

d)

calcium carbonate

e)

ammonium carbonate

6.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

PbK2

b)

PbSO4

c)

KSO4

d)

Pb(NO3)2

e)

KNO3

7.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

Which compound would not form ions in the complete ionic equation?

a)

PbI2

b)

all species form ions

c)

KNO3

d)

Pb(NO3)2

e)
KI
8.

Which of the following statements about writing molecular, complete, and net ionic equations is true?

a)

A molecular equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction.

b)

A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution.

c)

A net ionic equation is an equation showing only the species that actually participate in the reaction.

d)

A spectator ion remains unchanged in the reaction and appears on both sides of the equation.

e)
All three types of equations are essential in different contexts and serve different purposes.
9.

Which of the following compounds is insoluble?

a)
AgCl
b)

MgSO4

c)
KBr
d)

Na2CO3

e)

AlCl3

10.

What is the molarity of a solution containing 4 moles of KCl in 2.5 L of solution?

a)
2.5 M
b)

10.0 M

c)
0.8 M
d)
1.6 M
e)
5.6 M
11.

What is the molarity of a solution containing 4.26 g of KCl in 1.25 L of solution?

Molar mass of KCl = 74.55 g/mol

a)
0.86 M
b)

3.41 M

c)

0.0571 M

d)

0.046 M

e)
1.08 M
12.

What is the number of moles of solute in 550 mL of a 0.2 M solution?

a)
0.11
b)

27.5

c)
0.15
d)

110

e)

0.36

13.

What mass of HCl is needed to make 4 L of a 3 M solution? The molar mass of HCl is 36.5 g/mol.

a)

0.329 g

b)
730 g
c)

36.46 g

d)

437.52 g

e)

12 g

14.

Which donates protons?

a)

Arrhenius Acids

b)

Brønsted-Lowry Acids

c)

Arrhenius Bases

d)

Brønsted-Lowry Bases

e)
Electrons
15.

Which of the following statements is not true about what happens in displacement reactions?

a)
In displacement reactions, the less reactive element displaces a more reactive element from its compound.
b)
Displacement reactions occur only in aqueous solutions.
c)
Displacement reactions involve the transfer of electrons between reactants.
d)
Displacement reactions always result in the formation of a precipitate.
e)
In displacement reactions, the more reactive element displaces a less reactive element from its compound.
16.

Which of the following statements is correct about what happens in combustion reactions?

a)
Combustion reactions do not release heat
b)
During combustion reactions, a fuel reacts with oxygen to produce heat, light, carbon dioxide, and water.
c)
Combustion reactions produce only water
d)
Combustion reactions do not involve oxygen
e)
Combustion reactions do not involve a fuel
17.

Which of the following statements is true about what happens in combination reactions?

a)
Two or more substances combine to form a single product.
b)
Combination reactions result in the formation of a mixture.
c)
The reactants in combination reactions are always elements.
d)
Combination reactions involve the release of energy.
e)
Three substances combine to form two products.
18.

Which of the following statements is not true about what happens in decomposition reactions?

a)
Decomposition reactions release energy
b)
Decomposition reactions involve a single reactant
c)

Decomposition reactions may also be an oxidation-reduction reaction

d)

Decomposition reactions result in the formation of multiple products

e)
During decomposition reactions, energy is always absorbed.
19.

Consider the following reaction.

NO3− (aq) + Cu (s) → NO (g) + Cu2+ (aq)

Which statement is correct?

a)
NO3− is oxidized
b)
NO is reduced
c)
Cu is oxidized
d)
NO3− is reduced
e)
Cu2+ is reduced
20.

A diluted solution is prepared by mixing 10 mL of 2.5 M stock solution with water to a total volume of 100 mL. What is the concentration of the diluted solution?

a)

0,025 M

b)

25 M

c)
1.0 M
d)
0.25 M
e)
0.5 M
21.

What is the Molarity of a solution that has 0.4 moles of HCl in 9.5 L of solution?

a)

10.8 M

b)

9.1 M

c)

23.75 M

d)

3.8 M

e)
0.0421 M
22.

How many mL of a 1.00 M stock solution should be used to make 2.00 L of a 0.300 M sulphuric acid solution?

a)
1.00 L
b)
1.50 L
c)

666,7 mL

d)
300 mL
e)
600 mL
23.

A student is making 1.0 L of a 0.5 M aqueous solution of calcium bromide, CaBr2. Student puts the 0.5 moles of CaBr2 and then puts in how much water?

a)

approximately 0.25 L of water.

b)

enough water to make 2.0 L of solution.

c)

1.5 L of water.

d)

approximately 1.0 L of water.

e)

exactly 0.5 L of water.

24.

What volume of a 0.200 M KOH solution is required to titrate 50.0 mL of a 0.250 M HNO3 solution?

a)

12.5 mL

b)

70.0 mL

c)
25.0 mL
d)
62.5 mL
e)
50.0 mL
25.

A 50.0 mL of an unknown HCl solution was titrated with 0.449 M NaOH. To reach the equivalence point, 38.4 mL of the NaOH was used. What was the concentration of the HCl?

a)
0.225 M
b)
0.400 M
c)
0.500 M
d)

0.345 M

e)
0.150 M

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