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