Deck 8: Solutions

Question 1

In which of the following pairs of ionic compounds are both members of the pair soluble in water?

A) AgNO₃ and AgCl
B) LiOH and Li₂SO₄
C) PbSO₄ and BaCO₃
D) NH₄I and Sn₃(PO₄)₂

Answer 1

LiOH and Li₂SO₄

Question 2

If 145 mL of 2.00 M KOH is diluted to 1.15 L, the resulting solution contains

A) 0.334 moles of KOH
B) 2.30 moles of KOH
C) 3.34 moles of KOH
D) 23.0 moles of KOH

Answer 2

0.334 moles of KOH

Question 3

If two solutions with concentrations of 0.4 M sugar and 0.7 M sugar respectively are separated by a semipermeable membrane, during osmosis there is a net flow of

A) sugar molecules from the concentrated to the dilute solution
B) sugar molecules from the dilute to the concentrated solution
C) water molecules from the concentrated to the dilute solution
D) water molecules from the dilute to the concentrated solution

Answer 3

water molecules from the dilute to the concentrated solution

Question 4

Which of the following statements concerning factors that affect solute solubility is incorrect?

A) Most solid solutes become more soluble in water with increasing temperature.
B) Most solid solutes become less soluble in water with decreasing pressure.
C) Gaseous solutes become less soluble in water with increasing temperature.
D) Gaseous solutes become more soluble in water with increasing pressure.

Question 5

The solubility rule "like dissolves like" is not adequate for predicting solubilities when the solute is a(n)

A) nonpolar gas
B) ionic compound
C) nonpolar liquid
D) polar gas

Question 6

A 0.300 M solution of LiOH that contains 0.500 mole of solute would have a volume, in milliliters, of

A) 30.0 mL
B) 60.0 mL
C) 6.00 * 10² mL
D) 1.67 * 10³ mL

Question 7

What is the freezing point for a solution containing 1.00 mole of NaCl (an ionic component) dissolved in 1.00 kg of water?

A) +1.86^oC
B) -1.86^oC
C) +3.72^oC
D) -3.72^oC

Question 8

What volume, in milliliters, of 4.0 M NaOH is needed to prepare 145 mL of 0.15 M NaOH by dilution?

A) 3.9 * 10³ mL
B) 5.4 mL
C) 2.6 *10^-4 mL
D) 0.18 mL

Question 9

Compared to pure water, a 1 M sugar-water solution will have a

A) lower vapor pressure, lower boiling point and lower freezing point
B) higher vapor pressure, higher boiling point and higher freezing point
C) lower vapor pressure, higher boiling point and lower freezing point
D) lower vapor pressure, lower boiling point and higher freezing point

Question 10

Crenation of red blood cells occurs when the cells are placed in a(n)

A) hypotonic solution
B) isotonic solution
C) hypertonic solution
D) physiological saline solution

Question 11

A solution may contain

A) only one solvent but many solutes
B) many solvents but only one solute
C) only one solvent and one solute
D) many solvents and many solutes

Question 12

A colloidal dispersion differs from a suspension in that colloidal particles

A) tend to settle at an appreciable rate
B) are large enough to scatter light
C) are large enough to be seen with the naked eye
D) are large enough to be seen with a microscope

Question 13

In a solution, the solvent is

A) the substance being dissolved
B) always a liquid
C) the substance present in the greatest amount
D) always water

Question 14

Calculate the concentration in % (m/m) of a solution containing 20.5 g of LiF dissolved in 340.0 g of H₂O.

A) 1.14% (m/m)
B) 5.69% (m/m)
C) 6.03% (m/m)
D) 6.42% (m/m)

Question 15

A solution is made by dissolving 0.35 mole of LiI in enough water to give a final volume of 260.0 mL. What is the molarity of the solution?

A) 0.091 M
B) 0.67 M
C) 1.3 M
D) 2.6 M

Question 16

Calculate the grams of NaOH present in 9.0 mL of a 8.0% (m/v) NaOH solution.

A) 0.72 g
B) 0.80 g
C) 7.2 g
D) 8.0 g

Question 17

What is the molarity of a solution containing 16.7 grams of NH₃ in 1.50 liters of solution?

A) 0.0653 M
B) 0.653 M
C) 1.53 M
D) 11.1 M

Question 18

Which of the following solutions is hypertonic with respect to blood?

A) 0.5% (m/v) NaCl
B) 0.7% (m/v) NaCl
C) 4.5% (m/v) glucose
D) 7.6% (m/v) glucose

Question 19

For which of the following types of ionic compounds are most examples insoluble in water?

A) nitrates
B) sulfates
C) hydroxides
D) chlorides

Question 20

Which of the following statements concerning a saturated solution is incorrect?

A) Undissolved solute must be present.
B) Undissolved solute may or may not be present.
C) Undissolved solute, if present, is continually dissolving.
D) Undissolved solute, if present, is in equilibrium with dissolved solute.

Question 21

Which of the following solute amounts, when dissolved in 1.00 kg of water. Would produce a solution with a freezing point of -1.86^oC?

A) 0.500 mole NaCl
B) 1.00 mole glucose
C) 2.00 mole KBr
D) more than one correct response
E) no correct response

Question 22

In which of the following pairs of properties are both members of the pair colligative properties?

A) density, boiling point
B) vapor pressure, osmotic pressure
C) solubility, freezing point
D) more than one correct response
E) no correct response

Question 23

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) A solution of concentration 7.6 %(m/m) contains 7.6 grams of solute per 1 liter of solution.
(2) The use of antifreeze in car radiators in the winter and the use of rock salt in making homemade ice cream are based on the same chemical principle.
(3) One mole of any molecular solute raises the boiling point of one kilogram of water by 1.86^oC..

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 24

Which of the following solutions has an osmolarity of 3.0?

A) 4.0 M glucose
B) 2.0 M NaCl
C) 1.0 M Na₃PO₄
D) more than one correct response
E) no correct response

Question 25

Which of the following statements about solutions is correct?

A) A solution is a homogeneous mixture.
B) It is possible to have solutions in which both solute and solvent are solids.
C) Solutions readily separate into solute and solvent if left undisturbed for 24 hours.
D) More than one correct response.
E) No correct response.

Question 26

In which of the following sets of ionic compounds are all members of the set insoluble in water?

A) AgCl, PbCl₂, NH₄Cl
B) CuCO₃, CaCO₃, MgCO₃
C) PbSO₄, FeSO₄, BaSO₄
D) more than one correct response
E) no correct response

Question 27

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) Equal volumes of two solutions of the same molarity contain the same number of grams of solute.
(2) Hemolysis and crenation are "opposite" processes.
(3) The solubility rule "like dissolves like" is not adequate for predicting the solubility of ionic compounds in water.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 28

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) To find the molarity of a solution, both solution volume and the number of moles of solute must be known.
(2) Osmosis involves the passage of solvent from a dilute solution (or pure solvent) into a more concentrated solution.
(3) 5.0 %(m/v) glucose solution and 0.9 %(m/v) sodium chloride solution have the same osmolarity and are hypotonic relative to red blood cells.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 29

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) A colloidal dispersion is a homogeneous mixture and a suspension is a heterogeneous mixture.
(2) The selectivity of a semipermeable membrane is based on polarity differences among molecules.
(3) For dilute aqueous solutions, %(m/m) and %(m/v) concentration units have almost the same magnitude because the density of water is 1.00 g/mL and the solution is almost entirely water.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 30

A crystal of solid NaCl is placed into an aqueous NaCl solution. It is observed that most, but not all, of the crystal dissolves. This means the original solution was

A) supersaturated
B) unsaturated
C) dilute
D) more than one correct response
E) no correct response

Question 31

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) The Tyndall effect involves light-scattering by colloidal-sized particles.
(2) Aqueous solutions of 0.1 M KCl and 0.1 M glucose would have the same freezing point because the solvent is water in both cases.
(3) Percent by volume is a concentration unit used when both solute and solvent are liquids.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 32

Which of the following amounts of solution contain 20.0 g of solute?

A) 100.0 g of 20.0% (m/m) NaCl solution
B) 500.0 g of 4.00% (m/m) NaCl solution
C) 200.0 g of 10.0% (m/m) NaCl solution
D) more than one correct response
E) no correct response

Question 33

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) A saturated solution always contains excess undissolved solute.
(2) In aqueous solution, Ba²⁺ ion combines with NO₃^- ion to produce an insoluble salt.
(3) Addition of a nonvolatile solute to a solvent produces a solution with lower vapor pressure, freezing point, and boiling point than that of pure solvent.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 34

Which of the following solutions would always contain 10.0 g of solute per 40.0 g of solvent?

A) 20.0% (m/m) solution
B) 25.0% (m/v) solution
C) 25.0% (v/v) solution
D) more than one correct response
E) no correct response

Question 35

Which of the following types of interparticle attractions must be overcome in order for a solute to dissolve in a solvent?

A) solute-solute
B) solvent-solvent
C) solute-solvent
D) more than one correct response
E) no correct response

Question 36

Consider the following substances and their polarities: A - polar, B - polar, C - nonpolar, D - nonpolar. It is true that:

A) A is more soluble in C than in B.
B) C is more soluble in D than in A.
C) D is more soluble in B than in C.
D) More than one correct response.
E) No correct response.

Question 37

In which of the following pairings are the terms closely related?

A) hemolysis, hypotonic solution
B) hypertonic, higher osmotic pressure than within cells
C) isotonic solution, crenation
D) more than one correct response
E) no correct response

Question 38

Which of the following solutions has a molarity of 1.0?

A) 0.050 mole of solute in 25.0 mL of solution
B) 2.0 moles of solute in 500.0 mL of solution
C) 3.0 moles of solute in 1.5 L of solution
D) more than one correct response
E) no correct response

Question 39

Which of the following solutions will have a molarity of less than 1.0 after 50.0 mL of solvent is added to it?

A) 50.0 mL of 3.0 M solution
B) 10.0 mL of 5.0 M solution
C) 575 mL of 1.2 M solution
D) more than one correct response
E) no correct response

Question 40

Particles of the dispersed phase in a colloidal dispersion are

A) small enough that they cannot be seen by the naked eye
B) large enough that they settle out under the influence of gravity
C) small enough that they cannot be filtered out using filter paper
D) more than one correct response
E) no correct response

Question 41

Choose the correct numerical value for the molarity from the response list for a solution prepared from 0.25 mole solute in 2500 mL of solution.

A) 0.10 M
B) 0.20 M
C) 1.0 M
D) 2.0 M

Question 42

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) Addition of 40.0 mL of water to 10.0 mL of 8.0 M NaOH would produce a 2.0 M NaOH solution.
(2) Henry's law is a pressure-solubility relationship for gases in liquids.
(3) Boiling points are the basis for the solubility rule "like dissolves like."

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 43

Choose the correct numerical value for the molarity from the response list for a solution prepared from 0.50 mole solute in 500.0 mL of solution.

A) 0.10 M
B) 0.20 M
C) 1.0 M
D) 2.0 M

Question 44

For a solution composition of 10.0 g solute in 100.0 g solution; choose the correct numerical concentration of % (m/m).

A) 1.00
B) 5.00
C) 10.0
D) 11.1

Question 45

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) The osmolarity of a 3.0 M NaCl solution is greater than the osmolarity of a 2.0 M Na₂SO₄ solution.
(2) A solution with just two components must always be a liquid.
(3) Red blood cells will shrink in size when placed in an isotonic solution.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 46

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) Fat-soluble vitamins have polar molecular structures.
(2) Increased temperature decreases gas solubility, and increased pressure increases gas solubility.
(3) The mechanism for controlled-release medications involves encapsulation with particle coatings of varying thickness.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 47

For the set of ionic compounds, LiCl, AgCl, MgCl₂, choose the correct characterization of their solubilities in water from the response list.

A) All three salts are soluble.
B) Two of the three salts are soluble.
C) One of the three salts is soluble.
D) None of the three salts are soluble.

Question 48

Choose the correct numerical value for the molarity from the response list for a solution prepared from 0.40 mole solute in 2.0 L of solution.

A) 0.10 M
B) 0.20 M
C) 1.0 M
D) 2.0 M

Question 49

Choose the correct numerical value for the molarity from the response list for a solution prepared from 0.10 mole solute in 1.0 L of solution.

A) 0.10 M
B) 0.20 M
C) 1.0 M
D) 2.0 M

Question 50

For a solution composition of 5.00 g solute in enough solvent to give 50.0 g solution; choose the correct numerical concentration of % (m/m).

A) 1.00
B) 5.00
C) 10.0
D) 11.1

Question 51

For a solution composition of 10.0 g solute in enough solvent to give 1.00 L solution; choose the correct numerical concentration of % (m/v).

A) 1.00
B) 5.00
C) 10.0
D) 11.1

Question 52

For a solution composition of 5.00 mL solute in enough solvent to give 100.0 mL solution; choose the correct numerical concentration of % (v/v).

A) 1.00
B) 5.00
C) 10.0
D) 11.1

Question 53

For the set of ionic compounds, AlPO₄, Al(OH)₃, Al(NO₃)₃, choose the correct characterization of their solubilities in water from the response list.

A) All three salts are soluble.
B) Two of the three salts are soluble.
C) One of the three salts is soluble.
D) None of the three salts are soluble.

Question 54

For a solution composition of 10.0 g solute and 90.0 g solvent; choose the correct numerical concentration of % (m/m).

A) 1.00
B) 5.00
C) 10.0
D) 11.1

Question 55

For the set of ionic compounds, NaNO₃, KNO₃, NH₄NO₃, choose the correct characterization of their solubilities in water from the response list.

A) All three salts are soluble.
B) Two of the three salts are soluble.
C) One of the three salts is soluble.
D) None of the three salts are soluble.

Question 56

For the set of ionic compounds, CaSO₄, CaBr₂, CaCO₃, choose the correct characterization of their solubilities in water from the response list.

A) All three salts are soluble.
B) Two of the three salts are soluble.
C) One of the three salts is soluble.
D) None of the three salts are soluble.

Question 57

For the set of ionic compounds, BaSO₄, BaCO₃, Ba(OH)₂, choose the correct characterization of their solubilities in water from the response list.

A) All three salts are soluble.
B) Two of the three salts are soluble.
C) One of the three salts is soluble.
D) None of the three salts are soluble.

Question 58

For a solution composition of 10.0 g solute in 100.0 g solution; choose the correct numerical concentration of % (m/m).

A) 1.00
B) 5.00
C) 10.0
D) 11.1

Question 59

Choose the correct numerical value for the molarity from the response list for a solution using 10.0 g of solute whose molar mass is 50.0 g in 100.0 mL solution.

A) 0.10 M
B) 0.12 M
C) 0.25 M
D) 0.30 M

Question 60

Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices. (1) 2.0 liters of a 6.0 M solution would contain 12.0 moles of solute, independent of the identity of the solute.
(2) For liquid-liquid solutions, volume of the solution is always greater than the sum of the volumes of solute and solvent because of solute-solvent repulsion effects.
(3) Osmotic pressure is the amount of pressure needed to prevent the process of osmosis from occurring.

A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question 61

Using the response list, characterize the osmotic pressure for a 2.0% (m/v) glucose with respect to cells.

A) isotonic solution
B) hypertonic solution
C) hypotonic solution
D) saturated solution

Question 62

Using the response list, characterize the osmotic pressure for a 0.50% (m/v) NaCl solution with respect to cells.

A) isotonic solution
B) hypertonic solution
C) hypotonic solution
D) saturated solution

Question 63

Using the response list, characterize the osmotic pressure for a 5.0% (m/v) glucose with respect to cells.

A) isotonic solution
B) hypertonic solution
C) hypotonic solution
D) saturated solution

Question 64

Choose the correct numerical value for the molarity from the response list for a solution using 50.0 mL of a 0.30 M solution to which 75.0 mL of solvent has been added.

A) 0.10 M
B) 0.12 M
C) 0.25 M
D) 0.30 M

Question 65

Using the response list, characterize the osmotic pressure for a 0.80% (m/v) MgCl₂ with respect to cells.

A) isotonic solution
B) hypertonic solution
C) hypotonic solution
D) saturated solution

Question 66

Using the response list, characterize the osmotic pressure for a 5.0% (m/v) NaCl with respect to cells.

A) isotonic solution
B) hypertonic solution
C) hypotonic solution
D) saturated solution

Question 67

Choose the correct numerical value for the molarity from the response list for a solution using 75.0 mL of 0.20 M solution that has been concentrated to 60.0 mL.

A) 0.10 M
B) 0.12 M
C) 0.25 M
D) 0.30 M

Question 68

Choose the correct numerical value for the molarity from the response list for a solution using 50.0 mL of 0.40 M solution diluted to a final volume of 0.20 L.

A) 0.10 M
B) 0.12 M
C) 0.25 M
D) 0.30 M

Question 69

Choose the correct numerical value for the molarity from the response list for a solution using 50.0 mL of 0.40 M solution diluted to a final volume of 0.20 L.

A) 0.10 M
B) 0.12 M
C) 0.25 M
D) 0.30 M