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 of the following best describes an aqueous solution?

Accepted Answer

A solution in which water is the solvent.

Question 2

A student prepares a solution by dissolving 10.0 g of NaCl in enough water to make 500 mL of solution. What is the molarity of the solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$0.342\ \mathrm{M}$

Question 3

Which of the following statements about concentrated and dilute solutions is correct?

Accepted Answer

A dilute solution contains a small amount of solute compared to solvent.

Question 4

How many moles of solute are required to make $2.0\ \mathrm{L}$ of a $0.50\ \mathrm{M}$ solution?

Accepted Answer

$1.0\ \mathrm{mol}$

Question 5

A laboratory technician needs to prepare $250\ \mathrm{mL}$ of a $1.50\ \mathrm{M}$ KBr solution. What mass of KBr (molar mass = $119.00\ \mathrm{g/mol}$) is required?

Accepted Answer

$44.6\ \mathrm{g}$

Question 6

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 7

If you dilute $0.200\ \mathrm{L}$ of a $15.0\ \mathrm{M}$ NaOH stock solution to a final concentration of $3.00\ \mathrm{M}$, what is the final volume of the solution?

Accepted Answer

$1.00\ \mathrm{L}$

Question 8

A $0.125\ \mathrm{M}$ NaOH solution contains how many moles of NaOH in $2.00\ \mathrm{L}$ of solution?

Accepted Answer

$0.250\ \mathrm{mol}$

Question 9

Which of the following ions, when present in a compound, guarantees that the compound is soluble in water with no exceptions?

Accepted Answer

$\mathrm{NO}_3^-$

Question 10

Which of the following compounds is insoluble in water?

Accepted Answer

$\mathrm{BaSO}_4$

Question 11

When solutions of $\mathrm{K_2CO_3}$ and $\mathrm{NiCl_2}$ are mixed, which product will precipitate?

Accepted Answer

$\mathrm{NiCO}_3$

Question 12

Which of the following is a strong electrolyte?

Accepted Answer

$\mathrm{KBr}$

Question 13

What is the net ionic equation for the reaction between aqueous $\mathrm{HCl}$ and aqueous $\mathrm{NaOH}$?

Accepted Answer

$\mathrm{H}^+(aq) + \mathrm{OH}^-(aq) \rightarrow \mathrm{H_2O}(l)$

Question 14

A $10.00\ \mathrm{mL}$ sample of $0.200\ \mathrm{M}$ HBr is titrated with $0.200\ \mathrm{M}$ NaOH. What volume of NaOH is required to reach the equivalence point?

Accepted Answer

$10.00\ \mathrm{mL}$

Question 15

Which of the following is the correct net ionic equation for the gas-evolution reaction between $\mathrm{HNO_3}(aq)$ and $\mathrm{Na_2CO_3}(aq)$?

Accepted Answer

$2\ \mathrm{H}^+(aq) + \mathrm{CO_3}^{2-}(aq) \rightarrow \mathrm{H_2O}(l) + \mathrm{CO_2}(g)$

Question 16

Assign the oxidation state to sulfur in $\mathrm{SO_4^{2-}}$.

Accepted Answer

$+6$

Question 17

Which of the following reactions is a redox reaction?

Accepted Answer

$2\ \mathrm{Mg}(s) + \mathrm{O_2}(g) \rightarrow 2\ \mathrm{MgO}(s)$

Question 18

In the reaction $2\ \mathrm{Na}(s) + \mathrm{Cl_2}(g) \rightarrow 2\ \mathrm{NaCl}(s)$, which species is the reducing agent?

Accepted Answer

$\mathrm{Na}(s)$

Question 19

According to the activity series, which metal is most easily oxidized?

Accepted Answer

$\mathrm{K}$

Introduction to Solutions and Aqueous Reactions: Solution Concentration and Molarity

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