$$M = \dfrac{\text{moles of solute}}{\text{volume of solution in liters}}$$

Question 1

Which of the following metals will react with hydrochloric acid to produce hydrogen gas, based on the activity series?

Accepted Answer

Zinc (Zn)

Question 2

A solution contains 1.46 moles of $$C_6H_{12}O_6$ in 1.00 L of solution. What is the molarity of the solution?

Accepted Answer

$$1.46\ \mathrm{M}$$

Question 3

Which statement best describes a single displacement reaction?

Accepted Answer

An element replaces another element in a compound, forming a new element and a new compound.

Question 4

What is the correct formula to calculate the molarity ($$M) of a $$solution?

Accepted Answer

$$M = \dfrac{	ext{moles of solute}}{	ext{volume of solution in liters}}$$

Question 5

A student wants to prepare 500.0 mL of 2.80 M KI solution. What mass of KI is required? (Molar mass of KI = 166 g/mol)

Accepted Answer

$$232\ \mathrm{g}$$

Question 6

Which of the following statements about dilution is correct?

Accepted Answer

The number of moles of solute remains the same after dilution.

Question 7

How many moles of $$NO_3$$^-$$ ions are present in 1.00 L of 1.00 M Ba$$($$NO_3)_2$ solution?

Accepted Answer

2.00 mol

Question 8

You have a stock solution of 4.00 M $$HNO_3. $$How many milliliters of this stock solution are needed to prepare 60.0 mL of 0.200 M $$HNO_3$$?

Accepted Answer

3.00 mL

Question 9

In an acid-base titration, 42.00 mL of 0.150 M NaOH is required to neutralize 50.00 mL of HCl. What is the molarity of the HCl solution?

Accepted Answer

$$0.196\ \mathrm{M}$$

Question 10

Which of the following best explains why copper does not react with hydrochloric acid to produce hydrogen gas?

Accepted Answer

Copper is below hydrogen in the activity series and cannot displace hydrogen ions.

Question 11

A solution is prepared by dissolving 1.00 mol of $$KCl in $$enough water to make 1.00 L of solution. What is the concentration of $$K^+$$ ions?

Accepted Answer

$$1.00\ \mathrm{M}$$

Question 12

Which equation correctly represents the neutralization reaction between sulfuric acid and sodium hydroxide?

Accepted Answer

$$H_2SO_4(aq) + 2NaOH(aq) \rightarrow 2H_2O(l) + Na_2SO_4(aq)$$

Question 13

If 42.00 mL of 0.150 M NaOH is required to neutralize 50.00 mL of $$H_2SO_4$$, what is the molarity of the $$H_2SO_4$$ solution?

Accepted Answer

$$0.0630\ \mathrm{M}$$

Question 14

Which of the following is true about the equivalence point in a titration?

Accepted Answer

It is the point where the reaction between acid and base is complete.

Question 15

Which of the following ions is produced in twice the concentration of the original salt when $$Ba(NO_3$)_2 is $$dissolved in water?

Accepted Answer

$$NO_3$$^-$$

Question 16

A reactive metal is placed in a solution containing ions of a less reactive metal. What will happen?

Accepted Answer

The reactive metal will be oxidized and the less reactive metal ions will be reduced.

Question 17

Which of the following best describes the role of an indicator in a titration?

Accepted Answer

It changes color at or near the equivalence point.

Question 18

Which of the following is the correct relationship for a dilution calculation?

Accepted Answer

$$M_i V_i = M_f V_f$$

Question 19

In a redox reaction, which species is oxidized?

Accepted Answer

The species that loses electrons.

Reactions in Aqueous Solution: Displacement Reactions, Activity Series, and Solution Concentrations

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