[Chemistry] Unit 6: Solutions

Henry's law

At a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid

Graham's law of effusion

The rate of effusion of a gas is inversely proportional to the square root of the gas's molar mass; this relationship is also true for the diffusion of gases

A

The relationship between pressure and volume of a gas is A. inverse B. direct C. incomplete D. none of the choices

D

There are 3 solutions. Solution 1 has a mole of sugar, solution 2 has a mole of NaCl, and solution 3 has a mole of CaCl2. Which solution would have the lowest freezing point? A. no way to tell B. solution 2 C. solution 1 D. solution 3

B

True or False? Any pressure, temperature, and volume for gases will always give you the same constant.

True

True or False? The variables in Charles's Law are directly related.

False

True or False? The variables in Gay-Lussac's Law are inversely related.

Charles's Law

V1/T1=V2/T2

R

What is the symbol for the ideal gas constant?

C

What is the term for something that depends on the amount and not the type of particles? A. freezing point B. none of these choices C. colligative D. boiling point

C

What temperature units must be used for Charles's law? A. Farenheit B. Celsius C. Kelvin D. temperature isn't used in Charles's law

C, D

What two variables are controlled (held constant) in Gay-Lussac's law? A. Pressure B. Temperature C. Amount (mass) D. Volume

A, D

What two variables are explored in Gay-Lussac's law? A. Pressure B. Volume C. Number of moles D. Temperature

A

What units should the temperature be in? A. Kelvin B. Celsius C. Farenheit D. The units don't matter for temperature in combined gas law

A

What variable(s) are held constant? A. Number of moles B. Temperature C. Pressure D. Volume

A, B, C

What variable(s) are involved in the combined gas law? (Check all that apply) A. Temperature B. Pressure C. Volume D. Number of moles

A, B

What variables have to be held constant in Boyle's law? A. number of moles B. temperature C. pressure D. volume

D

When a nonvolatile solute is added to a pure solvent, the vapor pressure will __. A. remain the same B. raise C. first raise then lower D. lower

A

When the pressure above a solution is high, the solubility of a gas is high. A. True B. False

C, D

When you calculate these colligative properties, you should be aware of: A. adding the change in temperature to the original freezing point B. subtracting the change in temperature from the boiling point C. the dissociation of ions from an ionic compound D. grams to moles of solute

A, B

Which two variables are examined using Charles's law? A. Volume B. Temperature C. Amount (mass) D. Pressure

A, D

Which two variables must be controlled (held constant) during Charles's law? A. Amount (mass) B. Volume C. Temperature D. Pressure

C

Which variable determines which ideal gas constant is used? A. Temperature B. Volume C. Pressure D. Number of moles

A, C

Why is a real gas not ideal? (Check all that apply) A. Non zero volume B. Pressure is not related to collisions C. Intermolecular forces exist D. Temperature has no connection with movement of gas particles

C, D

Why is a real gas not ideal? (Check all that apply) A. Pressure is not related to collisions B. Temperature has no connection with movement of gas particles C. Non zero volume D. Intermolecular forces exist

A

You add 70g ammonium chloride to 100g of water at 850C. This solution is saturated. You let the solution cool to 450C and NO crystals form out of solution. You have created a(n) A. super saturated solution B. immiscible solution C. unsaturated solution D. saturated solution

B

You are given a small beaker of solution at room temperature. You add a bit of solute to the solution and it dissolves into the solution. The solution was: A. saturated B. unsaturated C. warm D. concentrated

C

You have two beakers in front of you. Beaker A contains pure solvent. Beaker B contains a nonvolatile solute dissolved in the same solvent. How do the freezing points of the two samples compare? A. Sample A has a lower freezing point than sample B B. Samples A and B have the same freezing point C. Sample B has a lower freezing point than sample A D. There is not enough information to tell

B

You place 100 g of sodium nitrate in 100 g of water at 550C. The solubility for sodium nitrate at 550C is 120 g. You have created a(n) A. saturated solution B. unsaturated solution C. immiscible solution D. super saturated solution

Solution

a homogeneous mixture; consists of solutes dissolved in a solvent

Compressibility

a measure of how much the volume of matter decreases under pressure

Concentration

a measurement of the amount of solute that is dissolved in a given quantity of solvent; usually expressed as mol/L

colligative property

a physical property of a solution that depends only upon the number of solute particles, and not upon their identities; boiling-point elevation, freezing-point depression, and vapor-pressure lowering are colligative properties

Concentrated solution

a solution containing a large amount of solute

Saturated solution

a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure; an equilibrium exists between undissolved solute and ions in solution

Dilute solution

a solution that contains a small amount of solute

Unsaturated solution

a solution that contains less solute than a saturated solution at a given temperature and pressure

Supersaturated solution

a solution that contains more solute than it can theoretically hold at a given temperature; excess solute precipitates if a seed crystal is added

Molal boiling point elevation constant

the change in boiling point for a 1-molal solution of a nonvolatile molecular solute

Molal freezing-point depression constant

the change in freezing point for a 1-molal solution of a nonvolatile molecular solute

Molarity

the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 liter of solution

ideal gas constant

the constant in the ideal gas law with the symbol R and the value 8.31 (L·kPa)/(K·mol)

partial pressure

the contribution each gas in a mixture of gases makes to the total pressure

Boiling point elevation

the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent

Freezing point depression

the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent

Combined Gas Law

the law that describes the relationship among the pressure, temperature, and volume of an enclosed gas

Gay-Lussac's Law

the pressure of a gas is directly proportional to the Kelvin temperature if the volume is constant

Dilution

the process of adding solvent to lower the concentration of solute in a solution

effusion

the process that occurs when a gas escapes through a tiny hole in its container

Ideal gas law

the relationship PV=nRT, which describes the behavior of an ideal gas

Diffusion

the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout

Charles's Law

the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant

A, C

A real gas behaves ideally unless it is under _ conditions. (Check all that apply) A. high pressure B. high temperature C. low temperature D. high volume E. low pressure

D

Crystals of alum, sugar, or copper (II) sulfate are made by hanging a string in a solution of the substance. This solution must be: A. warm B. unsaturated C. solvent D. saturated

B, A

If you add a solute to a pure solvent, the freezing point will _____ and the boiling point will _____. A. Raise (elevate) B. Lower (depress)

B

If you are looking at gases that are in the same mixture, when using the ideal gas law, the following variable(s) will cancel out. A. volume and pressure B. volume and temperature C. pressure only D. number of moles only E. temperature only F. pressure and temperature

A

In order to find the total pressure of a mixture of gases you would: A. add together each individual gas pressure B. subtract each individual gas pressure from each other C. divide each individual gas pressure from each other D. multiply together each individual gas pressure

A

In the following problem, the combined gas law is not necessary and is better solved by __ 's law: A given mass of air has a volume of 6 L at 101.3 kPa and OoC. What will the pressure be if the temperature increases to 100oC with the volume held constant? A. Gay-Lussac B. Charles C. Boyle D. Avogadro

A

Kb is the __. A. molal boiling point constant B. Freezing point C. molal freezing point constant D. boiling point

C

Kf is the __. A. molal boiling point constant B. freezing point C. molal freezing point constant D. boiling point

B

Molality is the ratio of the moles of the solute to the __. A. kilograms of solution B. kilograms of solvent C. liters of solution D. liters of solvent

Gay-Lussac's Law

P1/T1=P2/T2

Combined Gas Law

P1V1/T1=P2V2/T2

Boyle's Law

P1V1=P2V2

Ideal gas law

PV=nRT

Dalton's Law of Partial Pressures

Ptotal = P1 + P2 + P3...

Graham's law of effusion

Rate A/Rate B = the square root of molar mass B/molar mass A

Solubility

The amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution

Molality

The concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kilogram (1000 g) of solvent

D

The equation for finding the __ is ΔTb = Kbm. A. molarity B. freezing point depression C. vapor pressure D. boiling point elevation

D

The ideal gas law has one more variable than the combined gas law. This variable is A. P - pressure B. T - Temperature in Kelvin C. R - ideal gas constant D. n - moles

Dalton's Law of Partial Pressures

at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases

Immiscible

describes liquids that are insoluble in one another; oil and water are examples

Miscible

describes liquids that dissolve in one another in all proportions

Boyle's Law

for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure