Chemistry Jeopardy Unit 6Solutions &

SolubilityI’m

ConcentratingColligative Properties

Equal What? Special K’s

10 10 10 10 10

20 20 20 20 20

30 30 30 30 30

40 40 40 40 40

50 50 50 50 50

The ingredient of a solution present in the greatest

amount.

A. IonsB. LiquidC. SoluteD. Solvent

This factor has the largest effect

of the solubility of solid

compounds.

A. Pressure

B. Temperature

C. Rate of Stirring

D. Amount of solvent

A solution that contains the maximum amount of solute

possible.

A. Unsaturated B. SaturatedC. Supersaturated D. Megasaturated

To maximize the solubility of gases in solutions a student

should.

A. Increase the temperatureB. Decrease the temperatureC. Decrease the pressure D. Increase the amount of solvent

What saying allows us to predict if a solvent will dissolve a solute?

A. Likes dissolve likesB. Polar dissolves nonpolarC. Nonpolar dissolves polarD. All solvents dissolve all solutes

Molarity has units of

A. grams/moleB. moles/kilogramC. liters/moleD. moles/liter

What is the concentration of a solution made by dissolving 1.5 mol of NaCl

to a volume of 500. mL

A. 1.5 M B. 0.0030 M C. 3.0 MD. 2.0 M

The product of concentration times volume.

A. MolesB. MolarityC. KeqD. Dilution

Proper solution preparation requires what piece of equipment.

A. BeakerB. Erlenmeyer FlaskC. Graduated CylinderD. Volumetric Flask

What is the resulting concentration when 20. mL of a 2.0M solution

is diluted to 40. mL?

A. 1.0 MB. 0.50 MC. 2.0 MD. 4.0 M

Colligative Properties depend on the number of

A. Chemists WorkingB. Particles in solutionC. Beakers usedD. Readings taken

A liquid reaches its boiling point when

A. It feels like itB. When bubbles start formC. The vapor pressure of the

liquid equals the pressure of the atmosphere

D. Cannot be determined

Adding a solute to a solvent

A. Raises the freezing pointB. Lowers the boiling pointC. Lowers the freezing pointD. Does not change the boiling point

What is the advantage of using AlCl3 to melt ice on sidewalks as opposed to

NaCl

A. The freezing point change will be 2x largerB. The freezing point change will be 4x largerC. The freezing point change will be 10x largerD. There is no advantage

When ΔTf = 3.4 ºC for an aqueous solution of NaCl the new freezing

point of the solution is

A. 3.4 ºCB. -3.4 ºCC. 103.4 ºCD. 96.6 ºC

When a reaction reaches equilibrium the forward and reverse reactions

A. Occur at different ratesB. Occur at the same rateC. Stop D. Make the same amount of chemical

The only stress that can change the equilibrium constant is

A.ConcentrationB.TemperatureC.PressureD.Final Exams

A large equilibrium constant mean the reaction is

A.Product favoredB.Reactant favoredC.NeutralD.Happens very fast

Ksp expressions are written for

A. Chemical equilibriumB. Force equilibriumC. Solubility equilibriumD. Balance Equilibrium

When a common ion is added to an equilibrium the equilibrium shifts

A. Toward the added ionB. Away from the added ionC. Toward the heat in the reactionD. Toward the higher pressure

What is the equilibrium expression for the following equation?3A(g) + 2B(g) A3B2(g)

A. Keq = [A3B2] / ([A]3[B]2)B. Keq = [A]3 [B]2 / [A3B2] C. Keq = [A] [B] / [A3B2]D. Keq = [A3] [B2] / [A3B2]

How can the following reaction bemade to favor the product side

of the reaction?3A(g) + 2B(g) A3B2(g) + heat

A. Add more productB. Increase the pressureC. Increase the temperatureD. Add a catalyst

What is the Ksp expression for the following reaction

BaSO4(s) Ba+2 + SO4-2

A. Ksp = [BaSO4] / ([Ba+2] [SO4-2])

B. Ksp = [Ba+2] [SO4-2] / [BaSO4]

C. Ksp = [BaSO4] / [Ba]2 [SO4] -2

D. Ksp = [Ba+2] [SO4-2]

Which of the following will have no effect on the reaction?

A (g) + B (g) AB (g) + heat

A. Increasing the amount of AB. Decreasing the temperature C. Increasing the amount of A2B2

D. Increasing the pressure

How could you lower the concentration of Ba+2 for the following reaction?

BaSO4(s) Ba+2 + SO4-2

A. Add solid Na2SO4

B. Increase the pressureC. Add solid Ba(NO3)2

D. The concentration cannot be changed