Chemistry Quiz: An Amazing Quiz On Solutions.

45 Questions | By Verdun | Updated: Mar 21, 2022 | Attempts: 213

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Hey fella, this is Chemistry time! Are you a high school student? Or a Chemist? Or in college preparing for your chemistry finals? Well, since you are here, I would like to challenge you to take this quiz up and score as much right as you can! Note: This quiz is based on Solutions in Chemistry. Are you ready?

Questions and Answers

1.

What does the picture of the sugar cube suspended in water tell you about where on a solid sample the solution process takes place?
- A.
  
  The solution process takes place at the bottom of a solid.
- B.
  
  The solution process takes place at the surface of a solid.
- C.
  
  The solution process takes place at the side of a solid.
2.

The conditions that cause sugar to dissolve faster in water are
- A.
  
  Solute is molecular,solvent in kilograms, middle temperature.
- B.
  
  The freezing point ,boiling-point elevation, and lower temperature.
- C.
  
  In granulated form, when stirred, and at a higher temperature.
3.

Finely ground particles dissolve more rapidly than larger particles because finer particles expose a greater surface area to the colliding solvent molecules.
- A.
  
  Quantity of solvent
- B.
  
  Sodium chloride.
- C.
  
  Solvent molecules.
4.

Three factors that influence the rate at which a solute dissolves in a solvent are
- A.
  
  Agitation (stirring or shaking), temperature, particle size.
- B.
  
  Solute is molecular,solvent in kilograms, middle temperature.
- C.
  
  In granulated form, when stirred, and at a higher temperature.
5.

Finely ground particles dissolve more rapidly than larger particles because finer particles expose a greater surface area to the ___________________.
- A.
  
  Non colliding solvent molecules.
- B.
  
  colliding solvent molecules.
- C.
  
  Semi- colliding solvent molecules.
6.

The amount of a substance that dissolves in a given quantity of solvent at a constant temperature is called the substance’s ______________________ .
- A.
  
  Solubility
- B.
  
  Dissolved
- C.
  
  Saturated
7.

If a solution contains the maximum amount of solute for a given quantity of solvent at a constant temperature, it is called a(n) ______________________ solution.
- A.
  
  Solubility
- B.
  
  Dissolved
- C.
  
  Saturated
8.

The total amount of dissolved solute remains constant. The total mass of undissolved crystals remains constant. When the rate of solvation equals the rate of crystallization, a state of dynamic equilibrium exists.
- A.
  
  Those sentences are true about a vapor pressure equilibrium
- B.
  
  Those sentences are true about a given quantity of solvent .
- C.
  
  Those sentences are true about a saturated solution.
9.

If two liquids dissolve each other, they are said to be ______________________ .
- A.
  
  Miscible
- B.
  
  Immiscible
- C.
  
  Decreased
10.

Vinegar is water-based, and oil and water are ________________. The less dense oil floats on the water-based solution.
- A.
  
  Immiscible
- B.
  
  Miscible
- C.
  
  Decreased
11.

The solubility of sodium chloride in water _________________ to 39.2 g per 100 g of water at 100 °C from 36.2 g per 100 g of water at 25 °C.
- A.
  
  Stays the same
- B.
  
  Decreases
- C.
  
  Increases
12.

How does the solubility of solid substances change as the temperature of the solvent increases?
- A.
  
  The solubility increases for all solids.
- B.
  
  The solubility increases for most solids.
- C.
  
  The solubility remains constant.
13.

_________ is the solid substance that is nearly insoluble at any temperature?
- A.
  
  Barium sulfate
- B.
  
  Sodium sulfate
- C.
  
  Lithium sulfate
14.

How does the solubility of a gas change with an increase in temperature?
- A.
  
  As the temperature increases, the solubility of a gas remains the same.
- B.
  
  As the temperature increases, the solubility of a gas increases.
- C.
  
  As the temperature increases, the solubility of a gas decreases.
15.

The directly proportional relationship between the solubility of a gas in a liquid and the pressure of the gas above the liquid is known as ___________________________.
- A.
  
  Howard's Law
- B.
  
  Henry's Law
- C.
  
  Harvard's Law
16.

In the closed bottle, the pressure is high and lots of CO2 is dissolved in the carbonated beverage. Once the cap is removed, the___________________, allowing more CO2 in the carbonated beverage to escape.
- A.
  
  Vapor pressure stays the same
- B.
  
  Vapor pressure decreases
- C.
  
  Vapor pressure increases
17.

The greater the pressure and _____________and the lesser the pressure and ______________.
- A.
  
  Less solubility, greater solubility
- B.
  
  greater solubility , less solubility
- C.
  
  Stable solubility , unstable solubility
18.

How does a solution become supersaturated?
- A.
  
  When the temperature of a solution with a small excess of solid solute is raised, the solute does not dissolve. If the solution is then allowed to slowly cool, the excess solute may stay dissolved at a temperature above the temperature at which it would ordinarily crystallize.
- B.
  
  When the temperature of a solution with a small excess of solid solute is raised, the solute does not dissolve. If the solution is then allowed to slowly cool, the excess solute may stay dissolved at a temperature below the temperature at which it would ordinarily crystallize.
- C.
  
  When the temperature of a solution with a small excess of solid solute is raised, the solute dissolves. If the solution is then allowed to slowly cool, the excess solute may stay dissolved at a temperature below the temperature at which it would ordinarily crystallize.
19.

A measure of the amount of solute dissolved in a given quantity of solvent is the ______________________ of a solution.
- A.
  
  Miscible
- B.
  
  Supersaturated
- C.
  
  Concentration
20.

The most important unit of concentration in chemistry is ______________________ .
- A.
  
  Solubility
- B.
  
  Molarity
- C.
  
  Solidify
21.

Molarity is the number of ________ of solute dissolved in one liter of solution.
- A.
  
  Meters
- B.
  
  Ounces
- C.
  
  Moles
22.

The best procedure for making a 0.50-molar (0.50M) solution in a 1.0-L volumetric flask is
- A.
  
  Add distilled water exactly to the 1.0-L mark, add 0.50 mol of solute, and then agitate to dissolve the solute.
- B.
  
  Place 0.50 mol of solute in the flask, add distilled water to the 1.0-L mark, and then agitate to dissolve the solute.
- C.
  
  Fill the flask with distilled water until it is about half full, add 0.50 mol of solute, agitate to dissolve the solute, and then carefully fill the flask with distilled water to the 1.0-L mark.
23.

List the information needed to find the molarity of a 2.0-L solution containing 0.50 mol of sodium chloride. Known __________ of solution __________of sodium chloride ___________________________ molarity (M) ___________________ liters of solution
- A.
  
  (known)1.0 liters, 0.20 mol, ( molarity) moles of solvent
- B.
  
  (known)2.0 liters, 0.50 mol, ( molarity) moles of solute
- C.
  
  (known)4.0 liters, 1.00 mol, ( molarity) moles of solultion
24.

How do you make a solution less concentrated?
- A.
  
  Dilute it with ice.
- B.
  
  Dilute it with gas.
- C.
  
  Dilute it with solvent.
25.

What happens to the number of moles of solute present in the solution when the volume doubles?
- A.
  
  The number of moles of solute remains decreases .
- B.
  
  The number of moles of solute increases.
- C.
  
  The number of moles of solute remains constant.