Question 1

Which of the following best describes a homogeneous mixture?

Accepted Answer

A mixture in which the composition is uniform throughout at the molecular level.

Question 2

What is the role of water in an aqueous solution?

Accepted Answer

Water acts as the solvent, dissolving the solute.

Question 3

Which statement correctly describes a concentrated solution?

Accepted Answer

A solution with a relatively large amount of solute compared to solvent.

Question 4

Why is water considered a good solvent for ionic and polar compounds?

Accepted Answer

Because water has a dipole moment, allowing it to interact with charged and polar species.

Question 5

Which of the following is a strong electrolyte?

Accepted Answer

NaCl(aq)

Question 6

What is the net ionic equation for the reaction between KOH(aq) and Mg(NO3)2(aq)?

Accepted Answer

$$2OH^- (aq) + Mg$$^{2+}$$ (aq) \rightarrow Mg(OH)_2 (s)$$

Question 7

Which of the following compounds is insoluble in water according to the solubility rules?

Accepted Answer

AgCl

Question 8

A solution is prepared by dissolving 12.0 g of FeSO4 (molar mass = 151.91 g/mol) in enough water to make 500 mL of solution. What is the molarity of the solution?

Accepted Answer

$$0.158\ \mathrm{mol/L}$$

Question 9

Which of the following statements about electrolytes is correct?

Accepted Answer

Strong electrolytes completely dissociate into ions in water.

Question 10

If you dilute 100.0 mL of a 2.00 M NaCl solution to a final volume of 500.0 mL, what is the final concentration?

Accepted Answer

$$0.400\ \mathrm{M}$$

Question 11

Which ions are considered spectator ions in the reaction: $$2KOH(aq) + Mg(NO_3$)_2(aq) \rightarrow 2KNO_3(aq) + Mg(OH)_2(s)$$?

Accepted Answer

$$K^+$$ and $$NO_3$$^-$$

Question 12

Which of the following will result in a precipitation reaction when mixed?

Accepted Answer

Pb(NO3)2(aq) and KI(aq)

Question 13

What is the molarity of a solution prepared by dissolving 5.00 g of NaCl (molar mass = 58.44 g/mol) in enough water to make 250 mL of solution?

Accepted Answer

$$0.342\ \mathrm{mol/L}$$

Question 14

Which of the following is a nonelectrolyte when dissolved in water?

Accepted Answer

Sugar (C12H22O11)

Question 15

A student mixes solutions of AgNO3(aq) and NaCl(aq). What is the solid product formed?

Accepted Answer

AgCl(s)

Question 16

Which equation correctly represents the relationship for solution dilution?

Accepted Answer

$$M_1V_1 = M_2V_2$$

Question 17

Which of the following is true about the dissolution of ionic compounds in water?

Accepted Answer

The compound dissociates into its component ions, which are stabilized by water molecules.

Question 18

How many moles of ions are produced when 1 mole of Na2SO4 dissolves in water?

Accepted Answer

3 moles (2 Na$$^+$$ and 1 SO$$_4$$^{2-}$$)

Question 19

Which of the following best explains why strong acids are considered strong electrolytes?

Accepted Answer

They completely ionize in water, producing a high concentration of ions.

Question 20

A solution contains 0.250 mol of solute in 0.500 L of solution. What is its molarity?

Accepted Answer

$$0.500\ \mathrm{mol/L}$$

Aqueous Solutions, Electrolytes, and Solution Concentration

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