Question 1

The solvent is the most abundant component of a mixture.

Accepted Answer

This statement is true. The solvent is the component of a mixture that dissolves other components, and it is typically present in a greater amount than the solutes.

Question 2

What mass of ethanol,C₂H₅OH,is required to decrease the freezing point of 2.000 L of water to -10.00^° C? (The freezing point depression constant for water is 1.86^° C/m)

Accepted Answer

The answer of What mass of ethanol,C₂H₅OH,is required to decrease...

Question 3

Explain why the solubility of gases decreases with increasing temperature.

Accepted Answer

The answer of Explain why the solubility of gases decreases...

Question 4

A sulfuric acid solution that is 34.0 % by mass has a density of 1.25 g/mL.
What is the molarity of the solution?

Accepted Answer

The answer of A sulfuric acid solution that is 34.0...

Question 5

A solution has a lower vapor pressure than the pure solvent,therefore,it will have a lower boiling point.

Accepted Answer

A solution has a lower vapor pressure than the pure solvent, which means it requires more heat to achieve the vapor pressure necessary for boiling, thus it will have a higher boiling point.

Question 6

Calculate the mass of the precipitate formed when 250.mL of a 0.100 M aqueous solution of silver nitrate reacts with 200.mL of a 0.150 M aqueous solution of sodium chloride. AgNO₃(aq)+ NaCl(aq) AgCl(s)+ NaNO₃(aq)

Accepted Answer

The answer of Calculate the mass of the precipitate formed...

Question 7

Calculate the volume (in mL)of a 0.300 M aqueous NaOH solution required to react completely with 32.5 mL of a 0.200 M aqueous solution of H₂SO₄. H₂SO₄(aq)+ 2 NaOH(aq) Na₂SO₄(aq)+ 2 H₂O(l)

Accepted Answer

The answer of Calculate the volume (in mL)of a 0.300...

Question 8

A solution of 5.36 g of a molecular compound dissolved in 76.8 g of benzene has a boilingpoint of 81.48^° C.The boiling point of pure benzene is 80.10^° C and the boiling point elevation constant for benzene is 2.53^°C/m.What is the molar mass of the solute?

Accepted Answer

The answer of A solution of 5.36 g of a...

Question 9

An ethylene glycol,C₂H₄(OH)₂,solution contains 500.g of ethylene glycol dissolved in 600.g of water.(The boiling point elevation constant for water is 0.512^° C/m. ) A.What is the molality of the solution? B.What is the boiling point of the solution?

Accepted Answer

The answer of An ethylene glycol,C₂H₄(OH)₂,solution contains 500.g of ethylene...

Question 10

Polar molecules tend to be soluble in water.

Accepted Answer

Polar molecules have a positive and negative end, which allows them to interact with the partial charges in water molecules. This makes them soluble in water.

Question 11

As particle size increases,surface area increases,and the rate of dissolving increases.

Accepted Answer

As particle size increases, the surface area decreases, and the rate of dissolving decreases. This is because there is less surface area available for the solvent to come into contact with and dissolve the solute.

Question 12

Freezing point depression,boiling point elevation,and osmotic pressure are all colligative properties.

Accepted Answer

Colligative properties are properties that depend on the number of solute particles present in a solution, not their identity or chemical nature. Freezing point depression, boiling point elevation, and osmotic pressure are examples of colligative properties.

Question 13

What mass of ethylene glycol,C₂H₄(OH)₂,is required to raise the boiling point of 1.400 kg of water to 103.50^° C? (The boiling point elevation constant for water is 0.512^° C/m. )

Accepted Answer

The answer of What mass of ethylene glycol,C₂H₄(OH)₂,is required to...

Question 14

When a solution is diluted by adding more solvent,the number of moles of solute remains constant.

Accepted Answer

When a solution is diluted by adding more solvent, the number of moles of solute remains constant. This is because the amount of solute present in the solution does not change, only the volume of the solution increases, leading to a decrease in concentration. Since the number of moles of solute is directly proportional to the concentration of the solution, it remains constant when the solution is diluted.

Question 15

A solution made by dissolving 20.g of NaCl in 100.0 mL of water has the same % by mass as a solution made by dissolving 10.0 g of NaCl in 50.0 mL of water.

Accepted Answer

Both solutions have a mass of 20.0 g of NaCl + water. Therefore, the % by mass of NaCl is the same in both solutions.

Question 16

As more solute is added to a saturated solution,the concentration of the solution increases.

Accepted Answer

A saturated solution has reached its maximum capacity of solute that can be dissolved at a given temperature and pressure, so adding more solute does not increase its concentration; the excess solute will not dissolve.

Question 17

A cup of coffee has a volume of 250.mL,a mass of 250.g,and contains 125 mg of caffeine,C₈H₁₀N₄O₂. A.What is the molarity of the caffeine in the coffee? B.What is the mass percent of the caffeine in the coffee?

Accepted Answer

The answer of A cup of coffee has a volume...

Question 18

A sample of a compound with a mass of 90.10 g is dissolved in 250.0 g of water. The freezing point of the resulting solution is -3.72^° C.The freezing point depression constant for water is 1.86^° C/m. Upon analysis the compound is found to consist of 39.99 % carbon,6.727 % hydrogen,and 53.28 % oxygen. What is the molecular formula of this compound?

Accepted Answer

The answer of A sample of a compound with a...

Question 19

Salt water has a higher freezing point than pure water.

Accepted Answer

Salt water has a lower freezing point than pure water because the dissolved salt disrupts the formation of ice crystals, thus requiring a colder temperature to freeze.

Question 20

Ammonium chloride is the most soluble salt at 20°C.

Accepted Answer

Ammonium chloride is the most soluble salt at 20°C, with a solubility of 29.7 g per 100 mL of water.

Quiz 14: Solutions

The solvent is the most abundant component of a mixture.

What mass of ethanol,C2H5OH,is required to decrease the freezing point of 2.000 L of water to -10.00° C? (The freezing point depression constant for water is 1.86° C/m)