Colligative Properties Practice Test - WW

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When 200.0 mL of 0.200 M H2SO4 is diluted with 155.0 mL of water, what is the molarity of the solution? A) 0.258 M B) 0.155 M C) 0.124 M D) 0.113 M E) none of these

D) 0.113 M

What is the approximate Na+ ion concentration in a 0.75 M Na2CO3 solution? A) 0.375 M B) 0.75 M C) 1.25 M D) 1.50 M E) 2.25 M

D) 1.50 M

Determine the molarity of a solution containing 2.00 g of sodium hydroxide in 250.0 mL of solution.

0.200 M

Plasma is the fluid portion of blood. The concentration of acetylsalicylic acid (aspirin, C9H8O4, molar mass = 180. g/mol) in your plasma is found to be 2.99 × 10^-4 M after you take two tablets of aspirin. If the volume of your plasma is 5.85 L, how many grams of aspirin are in your blood? (Assume that the density of plasma is 1.00 g/mL.)

0.315 g

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

0.513 g

Calculate the molarity of the solution made by dissolving 100.0 g of calcium nitrate in 450.0 mL of aqueous solution.

1.354 M

You dissolve 15.71 g of NH4NO3 in 150.0 mL of solution (call this solution A). You take 20.0 mL of solution A and add water until the total volume is 75.0 mL (call this solution B). You take 15.0 mL of solution B and add 25.0 mL of water to it (call this solution C). You mix 10.0 mL of solution B and 10.0 mL of solution C (call this solution D). What is the concentration of ammonium nitrate in solution D? A) 0.240 M B) 0.190 M C) 0.131 M D) 0.279 M E) none of these

A) 0.240 M

When 271.0 mL of 0.828 M HCl is diluted with 161.6 mL of water, the molarity of the solution (assuming the volumes are additive) is A) 0.519 M. B) 0.111 M. C) 0.00191 M. D) 0.309 M. E) 1.39 M.

A) 0.519 M.

What volume of 0.25 M HNO3 is necessary to react exactly with 7.4 g of Ca(OH)2? A) 8.0 × 10^2 mL B) 1.2 × 10^2 mL C) 4.0 × 10^2 mL D) 2.5 × 10^2 mL E) 2.0 ×10^2 mL

A) 8.0 × 10^2 mL

The concentration of a 300.0-mL sample of a calcium chloride solution is 0.256 M. What is the mass of the solute? A) 8.52 g B) 5.80 g C) 2.70 g D) 95 g E) 28.4 g

A) 8.52 g

1.00 mL of a 3.50 × 10^-4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. How many grams of oleic acid are in 5.00 mL of solution B? (molar mass for oleic acid = 282 g/mol) A) 9.87 × 10^-6 g B) 4.94 × 10^-5 g C) 4.94 × 10^-4 g D) 1.97 × 10^-6 g E) 7.00 × 10^-6 g

A) 9.87 × 10^-6 g

Which of the following solutions contains the greatest total ion concentration? A) One mole of sodium phosphate dissolved in 1.0 L of solution. B) One mole of potassium hydroxide dissolved in 1.0 L of solution. C) One mole of iron(II) nitrate dissolved in 1.0 L of solution. D) One mole of potassium chloride dissolved in 1.0 L of solution. E) At least two of these solutions have an equal number of ions, and these contain the greatest total ion concentration.

A) One mole of sodium phosphate dissolved in 1.0 L of solution.

A solute added to a solvent raises the boiling point of the solution because A) the solute particles lower the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. B) the temperature to cause boiling must be great enough to boil not only the solvent but also the solute. C) the solute increases the volume of the solution, and an increase in volume requires an increase in the temperature to reach the boiling point (derived from PV = nRT). D) the solute particles raise the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. E) Two of the above are correct.

A) the solute particles lower the solvent's vapor pressure, thus requiring a higher temperature to cause boiling.

How many grams of Na2SO4 are required to make 150.0 mL of a 0.180 M sodium sulfate solution? A) 3.40 g B) 3.84 g C) 3.21 g D) 2.78 g E) none of these

B) 3.84 g

You mix 50.0 mL of 2.00 M lead(II) nitrate with 50.0 mL of 2.00 M sodium chloride. What mass of lead(II) chloride should you form? A) 12.1 g B) 13.9 g C) 27.8 g D) 24.3 g E) none of these

B) 13.9 g

You dissolve a 1.28-g sample of NaCl in a total volume of 125.0 mL of solution. Your lab partner has 1.50 M aqueous NaCl and wants to make a solution with the same concentration and volume as yours. How much of the solution does your lab partner need to use? A) 1.83 mL B) 14.6 mL C) 125 mL D) 107 mL E) none of these

B) 14.6 mL

A 230.-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.10 M. What volume of solvent has evaporated from the 0.275 M solution? (Assume volumes are additive.) A) 288 mL B) 172 mL C) 63.3 mL D) 230. mL E) 58.0 mL

B) 172 mL

An aqueous solution contains 144.0 g of NaCl per liter. What is the molarity of the solution? A) 2.879 M B) 2.464 M C) 0.1682 M D) 0.1440 M E) 2.154 M

B) 2.464 M

In the reaction 2MnO4- + 5H2O2 + 6H+ → 2Mn2+ + 8H2O + 5O2 what volume of 0.150 M MnO4- solution is needed to react with 75.0 mL of a 0.150 M H2O2 solution? A) 75.0 mL B) 30.0 mL C) 45.0 mL D) 15.0 mL E) none of these

B) 30.0 mL

What volume of 12.0 M HCl is required to prepare 16.0 L of 0.250 M hydrochloric acid? A) 768 mL B) 333 mL C) 585 mL D) 130. mL E) none of these

B) 333 mL

You have 120.0 mL of a 0.245 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it has a concentration of 0.348 M. How much water must have evaporated? (Assume volumes are additive.) A) 84.5 mL B) 35.5 mL C) 120. mL D) 204 mL E) 119 mL

B) 35.5 mL

How much water must be added to 20.0 mL of a 9.50 M sulfuric acid solution to make a 0.480 M solution? (Assume volumes are additive.) A) 81.0 mL B) 376 mL C) 396 mL D) 101 mL E) none of these

B) 376 mL

What volume of 0.504 M barium nitrate solution is needed to prepare 218.0 mL of a solution that is 0.244 M in nitrate? A) 4.50 × 10^2 mL B) 5.28 × 10^1 mL C) 3.52 × 10^1 mL D) 1.06 × 10^2 mL E) 2.11 × 10^2 mL

B) 5.28 × 10^1 mL

Mixing 40.0 mL of a 4.00 M sodium chloride solution with 20.0 mL of a 5.00 M calcium chloride solution results in a solution with a chloride ion concentration of A) 4.33 M. B) 6.00 M. C) 4.50 M. D) 7.00 M. E) none of these

B) 6.00 M.

Adding salt to water decreases the freezing point of the water because it lowers the vapor pressure of the ice. A) True B) False

B) False

Consider five solutions that all have the same mass of solute in 100.0 mL of solution. Which has the highest concentration as measured in molarity? A) Na2SO4 B) NaF C) KCl D) CaCl2 E) NaCl

B) NaF

Which of the following aqueous solutions has the lowest freezing point? A) 0.18 m KCl B) 0.15 m Na2SO4 (ethylene glycol) C) 0.12 m Ca(NO3)2 D) pure water E) 0.20 m C2H6O2

B) and C)

Magnesium metal reacts with hydrochloric acid to form aqueous magnesium chloride and hydrogen gas. When 3.65 g of magnesium is added to 50.0 mL of 3.00 M hydrochloric acid, what mass of hydrogen is produced, assuming a complete reaction? A) 0.302 g B) 0.246 g C) 0.151 g D) 0.123 g E) none of these

C) 0.151 g

Calculate the concentration of NaOH if 26.2 mL reacts exactly with 24.4 mL of 0.311 M HCl. A) 0.145 M B) 0.334 M C) 0.290 M D) 0.579 M E) 0.311 M

C) 0.290 M

An aqueous solution contains 48.6 g of KNO3 in 290.6 mL of solution. What is the molarity of the solution? A) 0.140 M KNO3 B) 0.167 M KNO3 C) 1.65 M KNO3 D) 0.00716 M KNO3 E) 0.0591 M KNO3

C) 1.65 M KNO3

Reacting 42.8 mL of 0.320 M AgNO3 with 55.8 mL of 0.580 M K2CrO4 results in what mass of solid formed? A) 3.27 g B) 7.25 g C) 2.27 g D) 3.07 g E) 10.74 g

C) 2.27 g

What volume of 6.60 M potassium hydroxide is required to prepare 53.6 mL of 0.450 M KOH? A) 786 mL B) 0.0554 mL C) 3.65 mL D) 6.31 mL E) 1.35 mL

C) 3.65 mL

A 51.24-g sample of Ba(OH)2 is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 molar Ba(OH)2? A) 278 mL B) 333 mL C) 400. mL D) 249 mL E) 1.20 × 10^3 mL

C) 400. mL

Dissolving a solute such as KOH in a solvent such as water results in A) an increase in the melting point of the liquid. B) a decrease in the boiling point of the liquid. C) a decrease in the vapor pressure of the liquid. D) no change in the boiling point of the liquid.

C) a decrease in the vapor pressure of the liquid.

How many milliliters of 12.4 M HNO3 are needed to prepare 360.6 mL of 0.20 M HNO3? A) 2.2 × 10^1 mL B) 0.349 mL C) 0.034 mL D) 5.8 mL E) 35 mL

D) 5.8 mL

With what volume of 2.5 M HF will 6.4 g of calcium hydroxide react completely, according to the reaction 2HF + Ca(OH)2 → CaF2 + 2H2O? A) 1.6 × 10^1 mL B) 2.6 × 10^1 mL C) 1.6 × 10^2 mL D) 6.9 × 10^1 mL E) 3.5 × 10^1 mL

D) 6.9 × 10^1 mL

What volume of 2.0 M HCl can be prepared from 2.00 L of 9.00 M HCl? A) 444 mL B) 4.50 L C) 2.25 L D) 9.00 L E) none of these

D) 9.00 L

A saturated solution A) contains more solute than solvent. B) contains more solvent than solute. C) contains equal moles of solute and solvent. D) contains the maximum amount of solute that will dissolve in that solvent at that temperature. E) contains a solvent with only sigma bonds and no pi bonds (i.e. only single bonds, with no double or triple bonds).

D) contains the maximum amount of solute that will dissolve in that solvent at that temperature.

To calculate the concentration in molarity of a salt solution, you need to know A) the molar mass of the salt and the total volume of the solution. B) the mass of the salt added, the molar mass of the salt, the volume of water added, and the total volume of the solution. C) the mass of the salt added to the solution and the volume of water added to the solution. D) the mass of the salt added, the molar mass of the salt, and the total volume of the solution. E) the mass of the salt added to the solution and the total volume of the solution.

D) the mass of the salt added, the molar mass of the salt, and the total volume of the solution.

T

E

Consider a 0.90 M Al(NO3)3 solution. This solution has a nitrate ion concentration of A) 0.30 M. B) 0.90 M. C) 0.0 M. D) 8.1 M. E) 2.7 M.

E) 2.7 M.

A 16.2-g sample of HF is dissolved in water to give 2.6 × 10^2 mL of solution. The concentration of the solution is A) 6.2 M B) 0.21 M C) 4.2 M D) 0.81 M E) 3.1 M

E) 3.1 M

If a student needs to make a 0.10 M solution of NaHCO3, how many milliliters of solution can be made using a 0.35-g sample of NaHCO3? A) 4.2 mL B) 1.0 × 10^2 mL C) 35 mL D) 3.5 mL E) 42 mL

E) 42 mL

Which of the following aqueous solutions has the highest boiling point? A) 0.2 m KCl B) 0.2 m Na2SO4 C)0.2 m Ca(NO3)2 D) A and B. E) B and C.

E) B and C.

50.0g of pure sand (silica) is poured into 1 L of water where it immediately sinks to the bottom and remains undissolved. Which of the following is true? A) The freezing point of the water will go down. B) The boiling point of the water will go up. C) The boiling point of the water will go down. D) A and B E) None of the above

E) None of the above

What volume of 0.350 M KOH is required to react completely with 24.0 mL of 0.650 M H3PO4? A) 52.0 mL B) 156 mL C) 26.0 mL D) 104 mL E) none of these

E) none of these

Automobile radiators usually carry a sticker that indicates that they must contain an antifreeze solution for proper operation, winter or summer. Why should you not use ordinary water during the summer?

The antifreeze will lower the vapor pressure of the fluid or elevate the boiling point of the radiator solution so that the cooling system of your car will be able to operate at higher temperatures without generating excessive pressure.