Q: Which of the following is the correct formula for calculating molarity ($M$)?

$M = \dfrac{\text{Amount of solute (mol)}}{\text{Volume of solution (L)}}$

Question 1

Which statement best explains why dissolving solid substances in water is a practical way to allow chemical reactions to occur?

Accepted Answer

Dissolving solids in water allows the reactant particles to mix thoroughly and collide more frequently.

Question 2

Which of the following best describes a solution?

Accepted Answer

A homogeneous mixture of two or more substances, consisting of a solvent and one or more solutes.

Question 3

A student prepares a solution by dissolving 36.5 g of NaCl in enough water to make 750.0 mL of solution. What is the molarity of the solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$0.833\ \mathrm{M}$

Question 4

Which of the following is the correct formula for calculating molarity ($M$)?

Accepted Answer

$M = \dfrac{	ext{Amount of solute (mol)}}{	ext{Volume of solution (L)}}$

Question 5

How many grams of NaCl are required to make 500.0 mL of a 0.250 M solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$7.31\ \mathrm{g}$

Question 6

A laboratory technician needs to prepare 100.0 mL of a solution that is 0.500 M in chloride ion using magnesium chloride ($\mathrm{MgCl_2}$). What mass of $\mathrm{MgCl_2}$ is required? (Molar mass of $\mathrm{MgCl_2}$ = 95.21 g/mol)

Accepted Answer

$2.38\ \mathrm{g}$

Question 7

Which equation correctly relates the concentrations and volumes before and after dilution?

Accepted Answer

$M_1V_1 = M_2V_2$

Question 8

What volume of 12.0 M HCl stock solution is required to prepare 500.0 mL of a 0.145 M HCl solution?

Accepted Answer

$6.04\ \mathrm{mL}$

Question 9

Which of the following statements about electrolytes is TRUE?

Accepted Answer

Strong electrolytes dissociate completely in water, resulting in high electrical conductivity.

Question 10

Which of the following compounds is a strong electrolyte when dissolved in water?

Accepted Answer

Sodium chloride ($\mathrm{NaCl}$)

Question 11

Which of the following is the net ionic equation for the reaction between $\mathrm{AgNO_3(aq)}$ and $\mathrm{NaCl(aq)}$?

Accepted Answer

$\mathrm{Ag^+(aq) + Cl^-(aq) \rightarrow AgCl(s)}$

Question 12

Which of the following ions is considered a spectator ion in the reaction between $\mathrm{AgNO_3(aq)}$ and $\mathrm{NaCl(aq)}$?

Accepted Answer

$\mathrm{Na^+}$

Question 13

Which of the following compounds is generally insoluble in water?

Accepted Answer

$\mathrm{PbSO_4}$

Question 14

Which of the following is a correct Arrhenius definition?

Accepted Answer

An Arrhenius acid produces $\mathrm{H^+}$ ions (as $\mathrm{H_3O^+}$) in water.

Question 15

Which of the following is a strong acid?

Accepted Answer

$\mathrm{HNO_3}$

Question 16

In a titration, what is the equivalence point?

Accepted Answer

The point at which stoichiometric amounts of reactants have been mixed.

Question 17

A student titrates 15.00 mL of $\mathrm{H_2SO_4}$ with 18.45 mL of 0.0973 M NaOH. What is the molarity of the $\mathrm{H_2SO_4}$ solution? (Reaction: $\mathrm{H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O}$)

Accepted Answer

$0.0598\ \mathrm{M}$

Question 18

Which of the following is a redox reaction?

Accepted Answer

$\mathrm{2Na(s) + Cl_2(g) \rightarrow 2NaCl(s)}$

Question 19

Which element is most easily oxidized?

Accepted Answer

Na

Chapter 5: Introduction to Solutions and Aqueous Reactions – Study Notes

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