Unit 9: Solutions

Misc.

100

Determine if the following compound is soluble or insoluble. 

BaCO₃

Insoluble 

200

Why is an aqueous solution considered to be homogenous? 

Uniform throughout 

300

Draw a diagram of NaCl dissolving into ions in water in the correct orientation. 

Na+ next to oxygen

Cl- next to hydrogen 

400

What is the measure of the amount of solute present in a unit of solution referred to as? 

Concentration 

500

In a saturated solution of NaNO_3, equilibrium exists between what? 

The dissolved NaNO₃ ions in solution and the solid NaNO₃ crystals at the bottom of the container; meaning the rate at which NaNO₃ dissolves is equal to the rate at which it precipitates out of solution.

Solubility

100

Using your reference table, identify the grams of solute where NH₃ would be unsaturated, saturated, and supersaturated at 40C. 

Un = under 35

S = 35

Sup = above 35

200

According to the reference table, which of these substances is most soluble at 60C? 

a. NaCl

b. KCl

C. KClO₃

d. NH₄Cl

D. NH₄Cl

- Highest line 

300

Tell how many grams of each solute precipitate. Assume the solution is saturated and in 100 grams of water. 

KCl (aq) is cooled from 55C to 30C

9 grams 

400

According to reference table G, how many grams of KNO₃ would be needed to saturate 200 grams of water at 70C?

268 g

500

Based on Table G, which sample, when added to 100. grams of water and thoroughly stirred, produces a heterogenous mixture at 20C? 

a. 20 g KCl

b. 20 g KI

c. 80 g KCl

d. 80 g KI

C. 80 g KCl

-supersaturated solution 

Factors Influencing Solubility

100

What does the saying like dissolves like mean? 

Polar dissolves polar

Nonpolar dissolves nonpolar 

200

Describe the impact temperature has on the solubility of a solid.

Increase temp = increase solubility 

300

Potassium iodide is a ionic compound. What type of solution will it dissolve best in? 

Polar solution 

400

Determine the impact each factor below has on the solubility of a gas and a solid. 

-Temp

-Pressure 

-Surface Area 

- Solvent

-Temp; high for solids, low for gas

-Pressure; high for gas, no effect solids

-Surface Area; no effect gas, increase for solids

- Solvent; like dissolves like 

500

What conditions would give soda the most amount of dissolved CO₂ (g)? 

Low temperature and high pressure 

Molarity/ppm/%mass

100

Calculate the molarity of a solution of NaOH if 2 liters of the solution contains 4 moles of NaOH? 

2 M 

200

A 2,400 gram sample of an aqueous solution contains 0.012 g of NH₃. What is the concentration of NH₃ in the solution, expressed as parts per million. 

5.0 ppm 

300

Calculate the percent by mass of a 25 g solution containing 3.0 g CsOH.

12% 

400

How many moles of NaOH are required to give 3000 mL of a 6.4 M solution? 

19.2 moles 

500

Two solutions were made, calculate the molarity of each and determine which solution is more concentrated. 

Solution A - 2.5 L with 0.5 mols CuSO₄

Solution B - 2.5 L with 1.4 mols CuSO₄

A - 0.2 M

B - .56 M

Solution B

Colligative Properties

100

What is an electrolyte? 

Substance that dissolves into ions in solution and conducts electricity 

200

Which substance is an electrolyte? 

a. KI

b. CH₃CH₂OH

c. C₆H₆

a. KI

300

I have an aq. solution of MgCl₂, what will happen to the boiling point and freezing point of the solution? 

bp - increase

fp - decrease 

400

Which solution has the highest boiling point? 

a. 1 M NaCl

b. 1 M MgBr₂

c. 2 M NaCl

d. 2 M MgBr₂

d. 2 M MgBr₂

500

Put the following compounds in order of increasing change in freezing point. 

NaI

K₂SO₄

C₆H₁₄

Li₃PO₄

C₆H_14; NaI; K₂SO₄; Li₃PO₄