Adv. Chemistry Ch. #16 Review
Solutions.....ch. #16 review before taking the test.
Terms in this set (53)
Another word for stirring or shaking.
True or false? Stirring will increase the rate at which a substance will dissolve.
True or False? Heating a solution will decrease the rate at which a substance will dissolve.
True or False? Increasing the surface area of a solute will cause a substance to dissolve faster.
True or False? There is no limit on the amount of solute that a solvent will hold.
The maximum amount of solute per given quantity of solvent at a constant temperature and pressure.
The amount of solute that dissolves in a given amount of solvent at specified temperatures and pressures to produce a saturated solution is called this.
Usual unit of solubility.
grams solute/100 grams solvent
A solution that contains less solute than a saturated solution at a given temperature and pressure.
Two liquids are this if they dissolve in each other in all proportions.
Liquids that are insoluble in one another are __________________.
Raising the temperature of the solvent will usually _____________ the solubility of most solid substances.
Raising the temperature of the liquid solvent will usually ______________ the solubility of most gaseous substances.
This term means the solution contains more solute than it can theoretically hold at a given temperature.
If a ____________ is added to a supersaturated solution, then the excess solute will crystallize out of solution and grow into a larger crystal.
Formula for Henry's Law.
S1/P1 = S2/P2
Solubility of a gas _________ as you add more pressure to the system.
The solubility of a gas is 0.16 g/L at an unknown pressure. If the pressure is increased to 288 kPa, the new solubility is 0.44 g/L. What is the original pressure?
If the new pressure is 2.6 atmospheres and the new solubility is 9.5 g/L what was the original solubility at 1.0 atmospheres pressure?
The solubility of a gas is 0.58 g/L at a pressure of 104 kPa. What is new pressure if the new solubility is 1.4 g/L?
A measure of the amount of of solute that is dissolved in a given amount of solvent.
A solution with only a small amount of solute per solvent.
A solution with large amount of solute per solvent.
The number of moles of solute dissolved in a liter of solution.
A solution has a volume of 4.0-L and contains 500.0 g of glucose (C6H12O6). If the molar mass is 180 g/mol, what is the molarity of the solution?
A solution contains 1.75 mol NaCl in 250.0-mL of solution. What is the molarity?
How many moles of NH4NO3 are in 335-mL of 0.500M solution?
How many grams of solute are in 250-mL of 2.0M CaCl2?
Diluting a solution reduces the number of moles of solute per unit of volume, but the total number of moles of solute in solutions ______________________.
does not change
The dilution formula is -______________.
M1 x V1 = M2 x V2
How many milliliters of a solution of 1.0M KI are needed to prepare a 250.0-mL of 0.250M KI?
How would you prepare 250 mL of 0.20M NaCl using only a solution of 1.0M NaCl and water?
Transfer 5.0x10^1 mL of the 1.0 M solution to a 250.0 mL volumetric flask and add enough water to the mark.
Percent by volume has what formula?
volume of solute/volume of solution x 100%
If 25 mL of propanone (C3H6O) is diluted with water to a total solution volume of 250 mL, what is the percent by volume of propanone in the solution?
A bottle of antiseptic hydrogen peroxide (H2O2) is labeled 3.0% (v/v). How many mL of H2O2 are in a 500.0 mL bottle of this solution?
15 mL H2O2
What is the formula for the percent by mass (%m/m)?
mass of solute/mass of solution x 100%
Suppose you want to make 2500-g of a glucose solution in water that has a 7.0% (m/m). How much grams of glucose (C6H12O6) should you use?
How many grams of K2SO4 would you need to prepare 1500-g of a 5.0% solution K2SO4 (m/m) solution?
What is the concentration, in percent (v/v), of a solution containing 50 mL of diethyl ether (C4H10O) in 2.5 L of solution?
2.0% v/v diethyl ether
How many mL of a stock solution of 2.00M KNO3 would you need to prepare 100.0 mL of 0.150M KNO3?
How many moles of solute are present in 50.0 mL of 0.20M KNO3?
Calculate the molarity of a solution containing 400.0-g of CuSO4 in 4.00-L of solution.
If you dilute a solution, how does the moles of solute compare with the moles of solute after the dilution.
They are the same, you just added more solvent.
A property that depends only on the number of solute particles, and not upon their identity is called ______________.
Three important ____________ properties are vapor-pressure lowering, boiling-point elevation, and freezing point depression.
The decrease in a solution's vapor pressure is proportional to the _______________ the solute makes in solution.
number of particles
The difference in temperature between the freezing point of a solution and the freezing point of the pure substance is called the __________________.
freezing point depression
The magnitude of the freezing point depression is proportional to the number of solute particles dissolved in the solvent and (does/does not) depend upon their identity.
The difference in temperature between the boiling points of the solution and the boiling points of the pure solvent is the _________________.
The boiling point elevation is a colligative property that depends on the __________ of particles, not their identity.
The magnitude of the boiling-point elevation is _______________ to the number of solute particles.
The ______________ in a solution's vapor pressure is proportional to the number of particles the solute makes in solution.
Would a dilute or concentrated solution of sodium fluoride have a higher boiling point?
concentrated sodium fluoride
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