$$2\,\text{Ag}^+(aq) + \text{SO}_4$$^{2-}$$(aq) \rightarrow \text{Ag}_2\text{SO}_4(s)$$

$$\text{HCl}(aq) + \text{NaOH}(aq) \rightarrow \text{NaCl}(aq) + \text{H}_2\text{O}(l)$$

$$\text{H}^+(aq) + \text{OH}^-(aq) \rightarrow \text{H}_2\text{O}(l)$$

$$\text{KI}(aq) + \text{Pb(NO}_3)_2(aq) \rightarrow \text{PbI}_2(s) + 2\,\text{KNO}_3(aq)$$

$$\text{CO}_3$$^{2-}$$(aq) + 2\,\text{H}^+(aq) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(l)$$

Question 1

Which of the following best describes the difference between a concentrated solution and a dilute solution, as shown in the image?

Accepted Answer

A concentrated solution contains more solute particles per unit volume than a dilute solution.

Question 2

What is the molarity of a solution prepared by dissolving 25.5 g of KBr (molar mass = 119.00 g/mol) in enough water to make 1.75 L of solution?

Accepted Answer

$$0.122\,	ext{M}$$

Question 3

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

Accepted Answer

$$M_1V_1 = M_2V_2$$

Question 4

A student needs to prepare 1.00 L of a 1.00 M NaCl solution. Which of the following steps is correct?

Accepted Answer

Weigh out 1.00 mol of NaCl, add to a flask, add water to dissolve, and fill to the 1-L mark.

Question 5

How many liters of a 0.125 M NaOH solution are required to provide 0.255 mol NaOH?

Accepted Answer

$$2.04\,	ext{L}$$

Question 6

Which of the following statements about electrolytes is correct?

Accepted Answer

A strong electrolyte completely dissociates into ions in water and conducts electricity well.

Question 7

Which compound is insoluble in water according to the solubility rules?

Accepted Answer

AgCl

Question 8

What is the net ionic equation for the reaction between aqueous solutions of K$$_2SO$_4$$ and AgNO$$_3$$?

Accepted Answer

$$2\,	ext{Ag}^+(aq) + 	ext{SO}_4$$^{2-}$$(aq) ightarrow 	ext{Ag}_2	ext{SO}_4(s)$$

Question 9

Which of the following best describes what happens when NaCl dissolves in water?

Accepted Answer

Na$$^+$$ and Cl$$^-$$ ions are surrounded by water molecules and become free to move.

Question 10

A solution is prepared by diluting 0.200 L of a 15.0 M NaOH stock solution to a final concentration of 3.00 M. What is the final volume?

Accepted Answer

$$1.00\,	ext{L}$$

Question 11

Which of the following is a correct balanced molecular equation for the reaction between HCl(aq) and NaOH(aq)?

Accepted Answer

$$	ext{HCl}(aq) + 	ext{NaOH}(aq) ightarrow 	ext{NaCl}(aq) + 	ext{H}_2	ext{O}(l)$$

Question 12

Which of the following is the net ionic equation for the neutralization of a strong acid with a strong base?

Accepted Answer

$$	ext{H}^+(aq) + 	ext{OH}^-(aq) ightarrow 	ext{H}_2	ext{O}(l)$$

Question 13

A titration requires 12.54 mL of 0.100 M NaOH to neutralize 10.00 mL of HCl. What is the concentration of the HCl solution?

Accepted Answer

$$0.125\,	ext{M}$$

Question 14

Which of the following reactions is a precipitation reaction?

Accepted Answer

$$	ext{KI}(aq) + 	ext{Pb(NO}_3)_2(aq) ightarrow 	ext{PbI}_2(s) + 2\,	ext{KNO}_3(aq)$$

Question 15

Which of the following best describes a strong acid in aqueous solution?

Accepted Answer

It ionizes completely to produce H$$^+$$ ions.

Question 16

Which of the following is a correct net ionic equation for the reaction of Na$$_2CO$_3(aq) $$with HCl(aq)?

Accepted Answer

$$	ext{CO}_3$$^{2-}$$(aq) + 2\,	ext{H}^+(aq) ightarrow 	ext{CO}_2(g) + 	ext{H}_2	ext{O}(l)$$

Introduction to Solutions and Aqueous Reactions: Solution Concentration and Stoichiometry

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