Chemistry Unit 9 - Solutions

A 1-gram sample of a compound is added to 100 grams of H2O(l) and the resulting mixture is stirred thoroughly. Some of the compound is then separated from the mixture by filtration. Based on Table F, the compound could be? A) AgCl B) CaCl2 C) NaCl D) NiCl2

A

A decrease in pressure has the greatest effect on a solution that contains A) A gas in a liquid B) A liquid in a liquid C) A solid in a solid D) A solid in a liquid

A

A small quantity of a salt is stirred into a liter of water until it dissolves. In the resulting mixture, the water is A) The solvent B) The solute C) Dispersed material D) A precipitate

A

A solution consists of 0.50 mole of CaCl2 dissolved in 100. g of H2O at 25 C. Compared to the boiling point and freezing A) A higher boiling point and a lower freezing point B) A higher boiling point and a higher freezing point C) A lower boiling point and a lower freezing point D) A lower boiling point and a higher freezing point

A

According to SOLUBILITY CURVES reference table, which solution is saturated at 30 C? A) 12 grams of KClO3 in 100 grams of water B) 12 grams of KClO3 in 200 grams of water C) 30 grams of NaCl in 100 grams of water D) 30 grams of NaCl in 200 grams of water

A

After being thoroughly stirred at 10.⁰C, which substance will produce a heterogeneous mixture with 100. g of water? A) 25.0 g of KNO3 B) 25.0 g of KCl C) 25.0 g of NaCl D) 25.0 g of NaNO

A

As the temperature of liquid water decreases, its vapour pressure A) Decreases B) Increases C) Remains the same D) Disappears

A

As the temperature rises, the solubility of all gases in water A) Decreases B) Increases C) Remains the same

A

At standard pressure, how do the boiling point and freezing point of NaCl(aq) compare to that of H2O(l)? A) The boiling point of NaCl(aq) is higher, and the freezing point of NaCl(aq) is lower. B) The boiling point of NaCl(aq) is lower, and the freezing point of NaCl(aq) is higher. C) Both the boiling point and the freezing point of NaCl(aq) are lower. D) Both the boiling point and the freezing point of NaCl(aq) are higher.

A

Based on the SOLUBILITY CURVES chemistry reference table, when 100 grams of water saturated with KNO3 at 70 C is cooled to 25 C, the total number of grams of KNO3 that will precipitate is A) 90 B) 40 C) 45 D) 80

A

How many moles of solute are contained in 200 milliliters of a 1 M solution? A) 0.2 B) 0.8 C) 200 D) 1

A

Water boils at 90 C when the pressure exerted on the liquids equal A) 65 kPa B) 90 kPa C) 101.3 kPa D) 120 kPa

A

What volume of a 2.0M solution is needed to provide 0.50 mol of NaOH? A) 0.25 L B) 0.5 L C) 1.0 L D) 2.0 L

A

Which compound becomes less soluble in water as the temperature of the solution is increased? A) HCl B) KCl C) NaCl D) NH4Cl

A

Which diagram but illustrate the ion-molecule attractions that occur when the ions of NaCl(s) are added to water? A) H2O+Na and Cl+H2O B) OH2+Na and Cl+OH2 C) H2O+Na and Cl+OH2 D) OH2+Na and Cl+H2O

A

Which of the following substances is least soluble in 100. g of water at 50⁰C? A) NaCl B) KCl C) NH4Cl D) HCl

A

Carbon dioxide gas has a solubility of 0.0972 g/100g H2O at 40⁰C. Expressed in parts per million, this concentration is closest to A) 0.972 ppm B) 9.72 ppm C) 97.2 ppm D) 972 ppm

D

How many grams of the compound potassium chloride (KCl) must be dissolved in 200. g of water to make a saturated solution at 60⁰C? A) 30 g B) 45 g C) 56 g D) 90 g

D

If 100. mL of a 1.0M solution is evaporated to a volume of 25mL, what will be the concentration of the resulting solution? A) 0.25 M B) 0.50 M C) 2.0 M D) 4.0 M

D

In a true solution the dissolved particles A) Are visible to the eye B) Will settle out on standing C) Are always solid D) Cannot be removed by filtration

D

Most ionic substances are soluble in water because water molecules are A) Nonpolar B) Inorganic C) Ionic D) Polar

D

Of the following solutions, the one that will boil at the HIGHEST temperature contains 1 mole of nonvolatile solute dissolved in A) 1,000 g of solvent B) 750 g of solvent C) 500 g of solvent D) 250 g of solvent

D

What is the molarity of a solution of NaOH if 2 liters of the solution contains 4 moles of NaOH? A) 0.5 M B) 80 M C) 8 M D) 2 M

D

Which sample of matter is a mixture? A) H2O(s) B) H2O(l) C) NaCl(l) D) NaCl(aq)

D

A nonpolar solvent would most easily dissolve which of the following substances? A) NH3 B) CCl4 C) NaCl D) H2SO4

B

A solution A) Will separate on standing B) May have colour C) Can be cloudy D) Can be heterogenous

B

An aqueous solution has a mass of 490 grams, and contains 8.5 x 10-³ grams of calcium ions. The concentration of calcium ions in this solution is A) 4.3 ppm B) 17 ppm C) 8.5 ppm D) 34 ppm

B

As the temperature of a liquid decreases, the amount of a gas that can be a gas A) Decreases B) Increases C) Remains the same

B

At which temperature can water contain the MOST dissolved oxygen at a pressure of 1 atmosphere? A) 40 C B) 10 C C) 30 C D) 20 C

B

Nonpolar solvents will most easily dissolve solids that are A) Ionic B) Covalent C) Metallic D) Colored

B

Salt water is classified as A) Mixture, with fixed composition B) Mixture, with variable composition C) Compound, with fixed composition D) Compound, with variable composition

B

What happens when KI(s) is dissolved in water? A) I- ions are attracted to the oxygen atoms of the water B) K+ ions are attracted to the oxygen atoms of the water C) K+ ions are attracted to the hydrogen atoms of the water D) No attractions are involved; the crystal just falls apart.

B

What happens when NaCl(s) is dissolved in water? A) Cl- ions are attracted to the oxygen atoms of the water. B) Cl- ions are attracted to the hydrogen atoms of the water. C) Na+ ions are attracted to the hydrogen atoms of the water. D) No attractions are involved; the crystal just falls apart.

B

What happens when a crystal of a salt is dropped into an unsaturated solution of the same salt? A) Excess solute crystals form B) The crystal dissolves C) The crystal drops to the bottom, unchanged. D) The solution becomes colourless.

B

What happens when a crystal of solute is dropped into a supersaturated solution of the salt? A) The crystal dissolves. B) Excess solute crystals form. C) The crystal drops to the bottom, unchanged. D) The solution begins to boil.

B

What is the molarity of a KF(aq) solution containing 116g of KF in 1.00L of solution? A) 1.00 M B) 2.00 M C) 3.00 M D) 4.00 M

B

What is the molarity of a solution that contains 40. g of NaOH is 0.50L of solution? A) 1.0 M B) 2.0 M C) 0.5 M D) 0.25 M

B

When a teaspoon of sugar is added to water in a beaker, the sugar dissolves. The resulting mixture is A) A compound B) A homogeneous solution C) A heterogeneous solution D) An emulsion

B

Which amount of compound dissolved in 100. g of water at the stated temperature represents a solution that is saturated? A) 20 g KClO3 at 80⁰C B) 40 g KNO3 at 25⁰C C) 40 g KCl at 60⁰C D) 60 g NaNO3 at 40⁰C

B

Which compound's solubility decreases most rapidly as the temperature changes from 10⁰C to 70⁰C? A) NH4Cl B) NH3 C) HCl D) KCl

B

Which ion combines with Ba²+ to form a compound that is most soluble in water? A) S²- B) OH- C) Co3²- D) SO4²-

B

Which of the following compounds is LEAST soluble in water? A) Copper(II) chloride B) Iron(III) hydroxide C) Potassium sulfate D) Aluminum acetate

B

Which substance increases in solubility as the temperature decreases? A) KClO3 B) NH3 C) KNO3 D) NaCl

B

A saturated solution of potassium chloride at 10 C is heated to 30 C. As the solution is heated in a closed container, the total mass of the solution A) Decreases B) Increases C) Remains the same

C

A solution contains 14 g of KCl in 100. g of water at 40⁰C. What is the minimum amount of KCl that must be added to make this a saturated solution? A) 14 g B) 19 g C) 25 g D) 44 g

C

A student drops a crystal of NaCl into a beaker of NaCl(aq) and the crystal dissolves. The original solution must have been A) Supersaturated B) Saturated C) Unsaturated D) Heterogeneous

C

According to Table F, which ions combine with chloride ions to form an insoluble compound? A) Fe²+ ions B) Ca²+ ions C) Ag+ ions D) Li+ ions

C

An aqueous solution of copper sulfate is powered into a filter paper cone. What passes through the filter paper? A) Only the solvent B) Only the solute C) Both solvent and solute D) Neither the solute nor solvent

C

Based on the SOLUBILITY CURVES chemistry reference table, what is the maximum number of grams of KCl(s) that will dissolve in 200 grams of water at 50 C to produce a saturated solution ? A) 42 g B) 38 g C) 84 g D) 58 g

C

Hexane (C6H14) and water do NOT form a solution. Which statement explains this phenomenon? A) Hexane is nonpolar and water is ionic B) Hexane is polar and water is nonpolar C) Hexane is nonpolar and water is polar D) Hexane is ionic and water is polar

C

If 100. g of water at 80 C contains 45 g of KCl and 45g of NaNO3, the solution is A) Saturated with respect to both KCl and NaNO3 B) Saturated with respect to KCl and unsaturated with respect to NaNO3 C) Unsaturated with respect to both KCl and NaNO3 D) Supersaturated with respect to both KCl and NaNO3

C

If solutions of barium nitrate and sodium sulfate are mixed and then poured into a filter, the solid remaining on the filter will be A) Barium nitrate B) Sodium nitrate C) Barium sulfate D) Sodium sulfate

C

In an aqueous solution of potassium chloride, the solute is A) Cl- only B) K+ only C) K+Cl- D) H2O

C

The depression of the freezing point is dependent on A) The nature of the solute B) The formula mass of the solute C) The concentration of dissolved particles D) Hydrogen bonding

C

Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as A) An element B) A compound C) A homogeneous mixture D) A heterogeneous mixture

C

Under which conditions are gases most soluble in water? A) High temperature and high pressure B) High temperature and low pressure C) Low temperature and high pressure D) Low temperature and low pressure

C

What is the molarity of an H2SO4 solution of 0.25L of the solution contains 0.75 mol of H2SO4? A) 0.33 M B) 0.75 M C) 3.0 M D) 6.0 M

C

What is the percent by mass of a solution in which 60. g of NaOH are dissolved in sufficient water to make 100g of solution? A) 16% B) 40% C) 60% D) 67%

C

What is the percent by mass of a solution in which 60. g of acetic acid are added to 90. g of water? A) 20% B) 30% C) 40% D) 67%

C

What is the total number of moles of the solute H2SO4 needed to prepare 5.0L of a 2.0M solution of H2SO4? A) 2.5 mol B) 5.0 mol C) 10. mol D) 20. mol

C

Which compound is soluble in water? A) PbS B) BaS C) Na2S D) Fe2S3

C

Why is salt (NaCl) put on icy roads and sidewalks in the winter? A) It is ionic and raises the freezing point of water. B) It is covalent and raises the freezing point of water. C) It is ionic and lowers the freezing point of water. D) It is covalent and lowers the freezing point of water.

C