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How does the surface tension of water compare with the surface tensions of most other liquids? |
it is higher |
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What causes water’s low vapor pressure? |
hydrogen bonding |
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Which of the following is primarily responsible for holding water molecules together in the liquid state? |
hydrogen bonds |
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Which atom in a water molecule has the greatest electronegativity? |
the oxygen atom |
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The bonds between adjacent water molecules are called ____. |
hydrogen bonds |
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What is primarily responsible for the surface tension of water? |
hydrogen bonding |
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Which of the following is NOT a result of surface tension in water? |
Water has an unusually low vapor pressure |
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Surface tension ____. |
is the inward force which tends to minimize the surface area of a liquid |
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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. |
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Which is responsible for the high thermal energy required to melt ice? |
hydrogen bonding |
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Which of the following substances is the most soluble in water? |
sodium chloride |
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What occurs in solvation? |
solvent molecules surround solute ions |
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Which of the following substances dissolves most readily in gasoline? |
CH4 |
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Which of these would you expect to be soluble in the nonpolar solvent carbon disulfide, CS ? |
SnS2 |
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Which of the following substances dissolves most readily in water? |
NH3 |
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What type of compound is always an electrolyte? |
ionic |
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Which of the following compounds is a nonelectrolyte? |
carbon tetrachloride |
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Which of the following compounds is an electrolyte? |
sodium hydroxide |
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Which of the following compounds is a nonelectrolyte when pure, but an electrolyte when dissolved in water? |
ammonia |
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Which of the following are weak electrolytes in water? |
ionic compounds that partially dissociate in water |
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Which of the following compounds is a weak electrolyte? |
NH3 |
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Which of the following compounds is a strong electrolyte? |
potassium sulfate |
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Which of the following compounds is NOT an electrolyte? |
sugar |
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Which of the following usually makes a substance dissolve faster in a solvent? |
agitating the solution |
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Which of the following expressions is generally used for solubility? |
grams of solute per 100 grams of solvent |
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Which of the following pairs of factors affects the solubility of a particular substance? |
particle size and temperature |
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If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____. |
supersaturated |
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Which of the following substances is less soluble in hot water than in cold water? |
CO2 |
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Which of the following occurs as temperature increases? |
solubility increases |
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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 |
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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 |
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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 |
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What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution? |
3M |
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In which of the following is the solution concentration expressed in terms of molarity? |
10 mol of solute/ 1 L of solution |
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Which of the following operations yields the number of moles of solute? |
molarity x liters of solution |
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What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution? |
12M |
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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 |
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What does NOT change when a solution is diluted by the addition of solvent? |
number of moles of solute |
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How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr? |
50 mL |
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The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____. |
362 mL |
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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 |
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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 |
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In which of the following is concentration expressed in percent by volume? |
10%(v/v) |
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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 |
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The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____. |
????????:( |
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How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution? |
142 mL |
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In which of the following is concentration expressed in percent by volume? |
10mL solute/ 100mL SOLUTION |
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Which of the following is NOT a colligative property of a solution? |
supersaturation |
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Colligative properties depend upon the ____. |
number of solute particles in the solution |
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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 |
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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 |
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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 |
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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 |
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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 |
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