Q: Which of the following is the correct formula for calculating the mass of solute required to prepare a solution of known volume and molarity?

$$\text{mass} = \text{molarity} \times \text{volume} \times \text{molar mass}$$

Question 1

Which of the following best explains why water is an effective solvent for ionic compounds?

Accepted Answer

Water is polar, so its partial charges attract and surround ions, separating them from the crystal lattice.

Question 2

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

Accepted Answer

KClO4 (potassium perchlorate)

Question 3

A solution is prepared by dissolving 0.50 mol of NaCl in enough water to make 1.0 L of solution. What is the concentration of chloride ions in the solution?

Accepted Answer

$$1.0\ \mathrm{M}$$

Question 4

Which of the following best describes a precipitation reaction?

Accepted Answer

A reaction in which an insoluble solid forms when two solutions are mixed.

Question 5

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

Accepted Answer

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

Question 6

Which of the following is a nonelectrolyte in water?

Accepted Answer

C$$_6H$_{12}O$_6 ($$glucose)

Question 7

How many grams of NaCl (molar mass = 58.44 g/mol) are required to prepare 250 mL of a 0.200 M NaCl solution?

Accepted Answer

$$2.92\ \mathrm{g}$$

Question 8

A 10.00-mL sample of vinegar (acetic acid) is titrated with 0.5062 M NaOH. If 16.58 mL of NaOH is required to reach the equivalence point, what is the molarity of acetic acid in the vinegar?

Accepted Answer

$$0.840\ \mathrm{M}$$

Question 9

Which of the following statements about strong and weak electrolytes is correct?

Accepted Answer

Strong acids and soluble ionic compounds are strong electrolytes.

Question 10

What is the final concentration when 50.0 mL of 6.0 M HCl is diluted to a total volume of 300.0 mL?

Accepted Answer

$$1.0\ \mathrm{M}$$

Question 11

Which of the following best describes the process of hydration?

Accepted Answer

Water molecules surround and interact with solute ions or molecules, stabilizing them in solution.

Question 12

A solution contains 0.65 M $$\mathrm{Ca}_3(\mathrm{PO}_4)_2. $$What is the concentration of $$\mathrm{PO}_4$$^{3-}$$ ions?

Accepted Answer

$$1.95\ \mathrm{M}$$

Question 13

Which of the following is NOT a type of chemical reaction discussed in solution chemistry?

Accepted Answer

Polymerization reaction

Question 14

What is the limiting reactant when 0.10 mol of Na$$_2CO$_3$$ reacts with 0.15 mol of AgNO$$_3$$ according to the equation: $$\mathrm{Na}_2\mathrm{CO}_3 + 2\mathrm{AgNO}_3 \rightarrow \mathrm{Ag}_2\mathrm{CO}_3 + 2\mathrm{NaNO}_3$$?

Accepted Answer

AgNO$$_3$$

Question 15

Which of the following best describes the role of water in an acid-base reaction?

Accepted Answer

Water acts as a solvent and often as a product (as in neutralization).

Question 16

A student mixes solutions of FeSO$$_4$$ and Pb(NO$$_3$$)$$_2. $$What is the precipitate formed, if any?

Accepted Answer

PbSO$$_4$$

Question 17

Which of the following is the correct formula for calculating the mass of solute required to prepare a solution of known volume and molarity?

Accepted Answer

$$	ext{mass} = 	ext{molarity} 	imes 	ext{volume} 	imes 	ext{molar mass}$$

Question 18

Which of the following best describes a net ionic equation?

Accepted Answer

An equation that shows only the ions that participate directly in the reaction.

Question 19

Which of the following is a weak electrolyte in water?

Accepted Answer

NH$$_3$$

Question 20

A solution is prepared by dissolving 4.25 g of Ca metal in enough water to make 225 mL of solution. The reaction is $$\mathrm{Ca}(s) + 2\mathrm{H}_2\mathrm{O}(l) \rightarrow \mathrm{Ca(OH)}_2(aq) + \mathrm{H}_2(g). $$What is the molarity of hydroxide ions in the solution?

Accepted Answer

$$0.40\ \mathrm{M}$$

Chapter 4: Solution Chemistry and Precipitate Reactions

Study Guide - Practice Questions

Study Guide - Flashcards