47 terms

Chem. Chapter 16

STUDY
PLAY

Terms in this set (...)

Section 1: Describes the liquids that are insoluble in one another
immiscicble
Sections 1: solution containing maximum amount of solute
saturated solution
Section 1: solution containing more solute than can theoretically dissolve at a given temperature
supersaturated
Section 1: At a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid
Henry's law
Section 1: measure of the amount of solute dissolved in a specified quantity of solvent.
concentration
Section 1: Which of the following usually makes a substance dissolve faster in a solvent?
agitating the solution
Section 1:What is the maximum amount of KCl that can dissolve in 200 g of water?
68 g
Section 1: What is the solubility of silver nitrate if only 11.1 g can dissolve in 5.0 g of water at 20 degrees Celsius?
22.2 g over 100 g H20 at 20 degrees Celsius
Section 1: which of the following epressions is generally used for solubility?
grams of solute per 100 grams of solvent.
Section 1: which of the following pairs of factors affect the solubility of a particular substance?
temperature and the nature of solute and solvent.
Section 1: If a crystal added to an aqueous solution causes many particles to come of the solution, the original solution was
supersaturated
Section 1: Which of the following substances is less soluble in hot water than cold water?
CO2
Section 1: Which of the following occurs as temperature increases?
solubility increases.
Section 1: The solubility of a gas in a liquid is
directly proportional to the pressure of the gas above the liquid
Section 1: If the solubility of a particular solute is 10 g at 20 degrees Celsius, which of the following solution concentrations would represent a supersaturated aqueous solution of that solute?
11 g over 100 g H2O at 20 degrees Celsius
Section 1: what happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid decreases?
the solubility decreases
Section 1: to increases the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to
2.7 atm
Section 2: In a concentrated solution there is
a large amount of solute
Section 2: What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
3 m
Section 2: Which of the following operations yields the number of moles of solute?
molarity X liters of solution
Section 2: What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
12 m
Section 2: What is the molarity of 200 mL of sulution in which 2.0 moles of sodium bromide is dissolved?
10 m
Section 2: What is the number of moles of solute in 250 mL of a 0.4 M solution?
0.1 mol
Section 2: What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (Molar mass of solute dissolved= 26 g/mol)
2.2 m
Section 2: What does NOT change when a solution is diluted by the addition of solvent?
number of moles of solute
Section 2: How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
50 mL
Section 2: The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is
362 mL
Section 2: If 2.0 mL og 6.0M HCl is used to make a 500.0 mL aqueous solution, what is the molarity of the addition solution?
0.024 m
Section 2: To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution?
0.18M
Section 2: If the percent by volume is 2.0% and the volume of the solution is 250 mL, what is the volume of solute in solution?
5.0 mL
Section 2: In which of the following is concentration expressed in percent by volume?
10% (v/v)
Section 2: The volume of alcohol present in 620 mL of a 40.% (v/v) solution of alocohol is
248 mL
Section 3: Which of the following is NOT a colligative preoperty of a solution?
supersaturation
Section 3: Colligative properties depend upon the
number of solute particles in a solution
Section 3: A solute depresses the freezing point because the solute
disrupts crystal formation of the solvent
Section 3: The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is
1.7 m
Section 3: Which of the following is an expression of molality?
10 mol of solute over 1 kg of solvent
Section 3: What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?
0.375
Section 3: What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute= 24 g)
0.87m
Section 3: What is the number of kilograms of solvent in a 0.70 molal solution containging 5.0 grams of solute? (molar mass of solue= 30 g)
0.24 kg
Section 3: To which of the following variables is change in boiling point directly proportional?
molality of solution
Section 3: What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water? (Kf= 1.86 degrees Celsius/m)
-3.72 degrees Celsius
Section 3:The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is
-3.33 degrees Celsius
Section 3: What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb= 0.512 degrees Celsius/m)
101.4 degrees Celsius
Section 3: What is the molality of a solution of water and KCl if the freezing point of the solution is -3 degrees Celsius? (Kf= 1.86 degrees Celsius/m; molar mass of water = 18 g)
0.8 m
Section 3: What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (Kb= 0.512 degrees Celsius/m)
100.26 degrees Celsius
Section 3: What is the approximate molar mass of a molecular solute if 300 g of solute in 1000 g of water causes the solution to have a boiling point of 101 degrees Celsius? (Kb= 1.86 degrees Celsius/m; molar mass of water= 18 g)
150 amu
YOU MIGHT ALSO LIKE...
STUDY GUIDE