Solutions and Concentrations of Solutions

The total concentration of ions in a 0.250 M solution of HCl is __________.

• essentially zero

• 0.125 M

• 0.250 M

• 0.500 M

Of the following elements, __________ is the only one that cannot be found in nature in its elemental form.

• Mercury (Hg)

• Gold (Au)

• Silver (Ag)

• Sodium (Na)

What is the concentration (M) of KCl in a solution made by mixing 25.0 mL of 0.100 M KCl with 50.0 mL of 0.100 M KCl?

• 0.100

• 0.0500

• 0.0333

• 0.0250

How many grams of NaOH are there in 500.0 mL of a 0.175 M NaOH solution?

• 2.19 x 10^-3 g

• 3.50 g

• 114 g

• 14.0 g

As more salt is dissolved in water, what will happen to the boiling point of that solution?

• it will not be measurable

• it will decrease

• it will increase

• it will stay the same

What is the concentration (M) of CH₃OH in a solution prepared by dissolving 11.7 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

• 11.9

• 1.59 x 10^-3

• 0.0841

• 1.59

What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?

• 18

• 0.16

• 0.45

• 27

Which one of the following statements is true?

• A dilute solution has a small amount of solute dissolved in a small amount of solvent.

• A concentrated solution has a large amount of solute dissolved in a large amount of solvent.

• A concentrated solution has a small amount of solute dissolved in a large amount of solvent.

• A dilute solution has a small amount of solute dissolved in a large amount of solvent.

What is the freezing point of an aqueous 1.00 m NaCl solution? (K_f =1.86 ^oC/m) (Assume complete dissociation of the salt.)

• -1.86 ^oC

• -3.72 ^oC

• +1.86 ^oC

• -0.93 ^oC

Consider the three statements below. Which statement(s) is(are) true?

I. Hydration is a special case of solvation in which the solvent is water.

II. The oxygen end of water molecules is attracted toward Ca²⁺ ions.

III. The hydrogen end of water molecules is attracted toward Cl^- ions.

• I only

• II and III only

• II only

• I, II and III