Chem Final Chapter 13

A sample of salt water will freeze at a higher temperature than a sample of pure water.

false

A semipermeable membrane allows only half the amount of a substance to pass through it.

false

Colligative properties are independent of the amount of solute in solution.

false

Ionic solutes typically dissolve in nonpolar solvents

false

Molality is calculated by dividing grams of solute by kilograms of solution.

false

Osmotic pressure is the pressure required to completely reverse the direction of solvent movement in osmosis.

false

The major component is a solution is called the solute

false

The terms "molarity"and "molality" are considered identical and can always be used interchangeably

false

The tragedy at Lake Nyos in Cameroon, West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water.

false

The tragedy at Lake Nyos in Cameroon, West Africa, was due to the sudden release of excessive amounts of carbon monoxide dissolved in the lake water.

false

When a chunk of gold is melted and poured into the shape of an ingot, an aqueous solution of gold has been created.

false

If 50 grams of salt dissolves into 250 grams of water, the resulting solution must have a mass of 300 grams.

true

If you put a living cell into seawater containing a higher concentration of sodium chloride, the cell loses water through osmosis.

true

a solution that is 35 percent by mass NaCl contains 35 grams of NaCl dissolved in 100 grams of water

false

a surgar solution is an example of a weak electrolyte solution

false

one liter of 6.0 M HNO3 contains the same number of H+ ions as does one liter of 6.0 M H2SO4

false

solubility is formally defined as the amount of a compound that can be dissolved in water

false

sugar solutions conduct electricity because the dissolved particles are molecules

false

the molarity of a solution prepared by dissolving 150 grams of NacL in 1000 mL water is 0.15 M

false

One liter of a 2.0 M NaOH (aq) solution contains the same number of Na+ ions as does one liter of a 1.0 M Na2CO3 (aq) solution.

true

Osmosis is the process in which a solvent moves from an area of low solute concentration to an area of high solute concentration.

true

Upon completing a dilution from a stock solution, you will always have more volume of solution than you started with and it will have a lower concentration than the stock solution.

true

a saturated solution holds the maximum amount of solute under the solution conditions

true

a solution that is 13.58 percent by mass of sugar contains 13.75 grams of sugar dissolved in 87.5 grams of water

true

a supersaturated solution is unstable and crystallization usually occurs

true

it would be expected that methanol CH3OH would be more soluble in water than methane CH4 would be

true

molarity is defined as moles of solute per liter of solution

true

salt water is an example of a strong electrolyte solution

true

steel is an example of a solid solution

true

tap water contains dissolved nitrogen and oxygen

true

the fact that the oceans contain salt water shows that polar solvents dissolve in solutes

true

the minor component in a solution is called a solvent

true

the solubility of gases in water decreases with increasing temperature

true

the solubility of gases in water increases with pressure above the water

true

the solubility of solids in water generally increases with increasing temperature

true

vitamin c is water soluble vitamin so it is likely that this vitamin is polar

true

warm beer goes flat quicker than cold beer

true

What is the concentration of sodium chloride in the final solution if of BaC completely reacts and the total volume of the reaction is , given the reaction: Ba(aq) + NS(aq) → BaS(s) + 2NaCl (aq) A) 0.226 B) 0.0259 C) 0.0519 D) 0.667 E) none of the above

0.0519

What is the change in the boiling point of a solution made by dissolving 14.7 g of C6H12O6 into of water? The density of water is and . A) 0.502°C B) 5.22°C C) 0.0418°C D) 0.279°C E) none of the above Answer: D

0.279

What is the final concentration of a solution prepared by diluting of HCl to a final volume of ? A) 0.504 M B) 3.50 M C) 0.420 M D) 0.350 M E) none of the above

0.350

What is the final concentration of a solution prepared by diluting of HCl to a final volume of ? A) 0.504 M B) 3.50 M C) 0.420 M D) 0.350 M E) none of the above

0.350 M

A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters. The molarity of the final solution is ________. A) 0.500 M B) 0.750 M C) 1.00 M D) 2.25 M E) none of the above

0.750 M

What is the change in the freezing point of a solution made by dissolving of C6H12O6 into of water? The density of water is and A) 0.152°C B) 1.01°C C) 18.97°C D) 1.82°C E) none of the above

1.01

We dissolve 2.45 g of sugar in 200.0 g water. What is the mass percent of sugar in the solution? A) 1.21% B) 1.23% C) 2.42% D) 123% E) none of the above

1.21%

Given that you wished to use exactly 0.325 mole of NaCl to prepare a 2.50 M NaCl solution, how many milliliters of solution must you prepare? A) 130. mL B) 0.130 mL C) 7.69 mL D) 0.813

130 mL

Determine the volume (liters) of 0.500M NaOH solution required to neutralize 1.50L of 0.750M H2SO4. The neutralization reaction is: H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + 2 H2O (l) A) 2.25 B) 1.13 C) 2.00 D) 4.50 E) none of the above

4.50

How many milliliters of 0.755 M H2SO4 solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq) + H2SO4 (aq) → 2 H2O (l) + K2SO4 (aq) A) 51.9 mL B) 182 mL C) 91.1 mL D) 17200 mL E) none of the above

91.1 mL

Oftentimes solubility of a compound limits the concentration of the solution that can be prepared. Use the solubility data given with each compound shown below to determine which compound would allow the preparation of a 10.0 Molar solution. A) AgNO3 (solubility = 122 g/100 g H2O) B) KCl (solubility = 34.0 g/100 g H2O) C) NaNO3 (solubility = 89.0 g/100 g H2O) D) NH4Cl (solubility = 41.1 g/100 g H2O) E) none of the above

NaNO3 (solubility = 89.0 g/100 g H2O)

Why is it NOT a good idea to drink seawater when people are lost at sea? A) The high concentration of salt forces water out of the cells lining your stomach and intestine. B) The osmotic pressure builds up in the cells of your intestine until they potentially rupture. C) The semipermeable membrane protecting your stomach is ruptured during osmosis. D) The seawater has fish urine in it and who wants to drink that? E) none of the above

The high concentration of salt forces water out of the cells lining your stomach and intestine.

After you have completed the task of diluting a solution, which statement below must be TRUE? A) The new solution has more volume but has a lower concentration than before. B) The new solution has more volume but has a higher concentration than before. C) The new solution has less volume but has a lower concentration than before. D) The new solution has less volume but has a higher concentration than before. E) none of the above

The new solution has more volume but has a lower concentration than before.

Which of the following statements about colligative properties is FALSE? A) The boiling point of a solution is increased by the addition of salt. B) The freezing point of a solution is lowered by the addition of salt. C) The change in temperature is proportional to the molality. D) The identity of the solute is not a factor. E) All of the above statements are true.

all of the above statements are true

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker, the solution would be considered ________. A) unsaturated B) saturated C) supersaturated D) thermally saturated E) none of the above

saturated

A 0.10 molality solution of the sugar glucose (molecular weight = 180.10 g/mol) and a 0.10 molality solution of sucrose (molecular weight = 342.34 g/mol) would both boil at the same temperature.

true

A solution is a homogeneous mixture of two or more substances.

true

A stock solution is a more concentrated form than what is typically used in a lab. It often requires further dilution.

true

Adding a nonvolatile solute to a liquid will cause boiling point depression and freezing point elevation.

true

Air is an example of a gaseous solution

true