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Chapter 1516

chem
STUDY
PLAY
How does the surface tension of water compare with the surface tensions of most other liquids?
it is higher
What causes water's low vapor pressure?
hydrogen bonding
Which of the following is primarily responsible for holding water molecules together in the liquid state?
hydrogen bonds
Which atom in a water molecule has the greatest electronegativity?
the oxygen atom
The bonds between adjacent water molecules are called ____.
hydrogen bonds
What is primarily responsible for the surface tension of water?
hydrogen bonding
Which of the following is NOT a result of surface tension in water?
Water has an unusually low vapor pressure
Surface tension ____.
is the inward force which tends to minimize the surface area of a liquid
The fact that ice is less dense than water is related to the fact that ____.
ice has a molecular structure that is an open framework held together by hydrogen bonds.
Which is responsible for the high thermal energy required to melt ice?
hydrogen bonding
Which of the following substances is the most soluble in water?
sodium chloride
What occurs in solvation?
solvent molecules surround solute ions
Which of the following substances dissolves most readily in gasoline?
CH4
Which of these would you expect to be soluble in the nonpolar solvent carbon disulfide, CS ?
SnS2
Which of the following substances dissolves most readily in water?
NH3
What type of compound is always an electrolyte?
ionic
Which of the following compounds is a nonelectrolyte?
carbon tetrachloride
Which of the following compounds is an electrolyte?
sodium hydroxide
Which of the following compounds is a nonelectrolyte when pure, but an electrolyte when dissolved in water?
ammonia
Which of the following are weak electrolytes in water?
ionic compounds that partially dissociate in water
Which of the following compounds is a weak electrolyte?
NH3
Which of the following compounds is a strong electrolyte?
potassium sulfate
Which of the following compounds is NOT an electrolyte?
sugar
Which of the following usually makes a substance dissolve faster in a solvent?
agitating the solution
Which of the following expressions is generally used for solubility?
grams of solute per 100 grams of solvent
Which of the following pairs of factors affects the solubility of a particular substance?
particle size and temperature
If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.
supersaturated
Which of the following substances is less soluble in hot water than in cold water?
CO2
Which of the following occurs as temperature increases?
solubility increases
If the solubility of a particular solute is 10g/100gH20 at 20 C, which of the following solution concentrations would represent a supersaturated aqueous solution of that solute?
11g/100g h2o at 20 C
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
If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?
0.75 atm
What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
3M
In which of the following is the solution concentration expressed in terms of molarity?
10 mol of solute/ 1 L of solution
Which of the following operations yields the number of moles of solute?
molarity x liters of solution
What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
12M
What mass of Na2SO4 is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g)
710 g
What does NOT change when a solution is diluted by the addition of solvent?
number of moles of solute
How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
50 mL
The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____.
362 mL
If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution?
0.024M
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
In which of the following is concentration expressed in percent by volume?
10%(v/v)
If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of solute in solution?
8.0 g
The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.
????????:(
How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution?
142 mL
In which of the following is concentration expressed in percent by volume?
10mL solute/ 100mL SOLUTION
Which of the following is NOT a colligative property of a solution?
supersaturation
Colligative properties depend upon the ____.
number of solute particles in the solution
What is the number of kilograms of solvent in a 0.70 molal solution containing 5.0 grams of solute? (molar mass of solute = 30 g)
0.24kg
What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water? (K = 1.86 C/m)
-3.72 Celsius
The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is ____. (K = 1.86 C/m; molar mass of water = 18 g)
-3.33 Celsius
What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (K = 0.512 C/m; molar mass of water = 18 g)
101.4 Celsius
What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (K = 0.512 C/m)
100.26 Celsius