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Solutions Flashcards

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1
Q

A mixture that cannot be separated by a semipermeable membrane.

A

Solution.

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2
Q

A mixture that settles upon standing.

A

Suspension.

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3
Q

A mixture that contains particles that are small enough to pass through filters but are too large to pass through semipermeable membranes.

A

Colloid.

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4
Q

True or False:

A mixture can be classified as heterogeneous or homogeneous.

A

True.

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5
Q

True or False:

All solutions, by definition, are liquids.

A

False.

14 Kt gold is a solid solution (copper and silver). They can be solids, liquids or gasses.

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6
Q

A solution has 50.0 mL of ethanol and 10.0 mL of water. Which is the solute and which is the solvent?

A

Water solute, ethanol solvent.

Usually the higher volume component is the solvent.

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7
Q

A solution has 10.0 g of NaCl in 100.0 g of water. Which is the solute and which is the solvent?

A

NaCl solute, water solvent.

When a gas or solid is dissolved in water it is considered the solute and the water is the solvent.

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8
Q

A solution has 0.20 L of O2 and 0.80 L of N2. Which is the solute and which is the solvent?

A

O2 solute, N2 solvent.

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9
Q

Water is an excellent polar solvent and carbon tetrachloride (CCl4) is a nonpolar solvent. In which solvent is NaNO3 more likely to be soluble?

A

Water.

NaNO3 is an ionic compound, so it will be more soluble in water.

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10
Q

Water is an excellent polar solvent and carbon tetrachloride (CCl4) is a nonpolar solvent. In which solvent is I2 more likely to be soluble?

A

Carbon tetrachloride (CCl4).

I2 is non polar so would dissolved in non polar solvent.

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11
Q

Water is an excellent polar solvent and carbon tetrachloride (CCl4) is a nonpolar solvent. In which solvent is sucrose (table sugar) which is polar, more likely to be soluble?

A

Water.

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12
Q

Water is an excellent polar solvent and carbon tetrachloride (CCl4) is a nonpolar solvent. In which solvent is gasoline, which is nonpolar, more likely to be soluble?

A

Carbon tetrachloride.

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13
Q

True or False:

Ionic compounds will not be soluble in water, a molecular compound.

A

False.

Water is very polar so it is able to dissolve most ionic compounds! This is due to ion-dipole interactions.

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14
Q

If a crystal is added to a solution and it does not change size is it a saturated or unsaturated solution?

A

Saturated.

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15
Q

If a sugar cube completely dissolves when it is added to hot coffee is it a saturated or unsaturated solution?

A

Unsaturated.

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16
Q

Determine whether the following solution will be saturated or unsaturated at 20°C (the solubility of KCl is 34g/100mL at this temperature): adding 25 g of KCl to 100 g of water.

A

Unsaturated.

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17
Q

Determine whether the following solution will be saturated or unsaturated at 20°C (the solubility of NaNO3 is 68g/100mL at this temperature): addding 11 g of NaNO3 to 25 g of water.

A

Unsaturated.

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18
Q

Determine whether the following solution will be saturated or unsaturated at 20°C (the solubility of sugar is 82g/100mL at this temperature): adding 400 g of sugar to 125 g of water.

A

Saturated.

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19
Q

What role does temperature play in solubility?

A

Solids that are more soluble at higher temperatures form a supersaturated solution. This means the solution will have even more solute dissolved than if it were saturated.

These are unstable and will percipatate when disturbed.

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20
Q

A solution containing 80 g KCl in 200 g H2O at 50°C is cooled to 20°C. How many grams of KCl will remain in solution at 20°C?

Solubility data for KCl:

Solubility at 20°C = 34g KCl/100 g H2O

Solubility at 50°C = 43g KCl/100 g H2O

A

68 g of KCl.

Since 34g KCl can dissolve in 100g of H2O,

We have 200 g of water, therefore;

100 x 2 = 200 g
34 g x 2 = 68 g KCl.

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21
Q

A solution containing 80 g KCl in 200 g H2O at 50°C is cooled to 20°C. How many grams of KCl crystallized after cooling?

Solubility data for KCl:

Solubility at 20°C = 34g KCl/100 g H2O

Solubility at 50°C = 43g KCl/100 g H2O

A

12 g KCl.

Since we know that 68g of KCl can dissolve in 200 g of water at 20 degrees Celsius and we have 80 g of KCl when we started at 50 degree;

80 - 68 = 12 g.

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22
Q

True or False:

LiCl is soluble in water.

A

True.

It is an ionic compound.

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23
Q

True or False:

AgCl is soluble in water.

A

False.

Silver is insoluble. (PHAC Bud: Pb, Hg, Ag, Ca and Ba).

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24
Q

True or False:

BaCO3 is soluble in water.

A

False.

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25
Q

True or False:

K2O is soluble in water.

A

True.

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26
Q

True or False:

Fe(NO3)3 is soluble in water.

A

True.

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27
Q

True or False:

The solubility of most solids increases with increasing temperature.

A

True.

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28
Q

A sugar cube completely dissolves when it is added to hot coffee. Therefore the solubility of sugar ___________ with _________ temperature.

A

Increases, increasing.

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29
Q

True or False:

The solubility of all gases decreases with increasing temperature.

A

True.

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30
Q

True or False:

Pressure has no effect on the solubility of liquids or solids.

A

True.

It does affect the solubility of gas.

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31
Q

In general, the solubility of ________ in water decreases as temperature increases.

A

Gas.

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32
Q

Calculate the concentration of
nitrogen gas in water with a nitrogen gas at a partial pressure of 0.826 atm
above it. Henry’s law constant for
nitrogen in water is 6.8 × 10-4 mol/L-atm.

A

(0.826 atm)(.8 × 10-4 mol/L-atm) =

5.6 x 10^ -4

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33
Q

Calculate the mass percent (m/m) for the solute in the following solution:

25 g KCl and 125 g water.

A

Solution = 125 g + 25 g = 150 g

(m/m) % = [ solute (g)/solution (g) ] x 100

= 25/150 = 0.17 x 100 = 17%

34
Q

Calculate the mass percent (m/m) for the solute in the following solution:

12 g of sucrose in 225 g tea solution.

A

Solute = 12 g sucrose
Solution = 225 g tea

= 12/225 = 5.3%

35
Q

Calculate the mass percent (m/m) for the solute in the following solution:

8.0 g of CaCl2 in 80 g CaCl2 Solution

A

10% m/m CaCl2 solution.

36
Q

Calculate the m/v percent of the following solution:

75 g of NaSO4 in 250 mL of NaSO4 solution.

A

30% m/v Na2SO4 solution.

37
Q

Calculate the m/v percent of the following solution:

39 g of sucrose in 355 mL of Coke.

A

11% m/v sucrose solution.

38
Q

Calculate the number of mg of solute required to prepare the following solution:

50 g of a 5.0% (m/m) KCl solution.

A

2.5 g KCl.

39
Q

Calculate the number of mg of solute required to prepare the following solution:

1250 mL of a 4.0% (m/v) NH4Cl solution.

A

50 g NH4Cl.

40
Q

Calculate the number of mg of solute required to prepare the following solution:

250 mL of a 10% (m/v) acetic acid solution.

A

25 mL acetic acid.

41
Q

A mouthwash contains 22.5 % (v/v) alcohol. If the bottle of mouthwash contains 355 mL, what is the volume, in mL, of alcohol?

A

79.9 mL alcohol.

42
Q

A patient receives 100 mL of a 20% (m/v) mannitol solution every hour. How many grams of mannitol will the patient receive after 12 hours?

A

240 g of mannitol.

43
Q

A patient needs 100 g of glucose in the next 12 h. How many litres of a 5% (m/v) glucose solution must be given?

A

2 L.

44
Q

Calculate the grams of 25% (m/m) LiNO3 solution that contains 5.0 g of LiNO3.

A

20 g LiNO3.

45
Q

Calculate the mL of 10% (m/v) KOH solution that contains 40.0 g KOH.

A

400 mL KOH solution.

46
Q

Calculate the molarity of the following solution:

2.0 moles of glucose in 4.0 L of a glucose solution.

A

0.50 M glucose solution.

47
Q

Calculate the number of grams of KCl required to prepare 4.00 L of a 0.200 M KCl solution.

A

59.6 g KCl.

.200 M = mol? / 4 L
(4)(.200) = 0.8 mol

= 0.8 mol x ( 74.55 g KCl/1 mol KCl)
= 59.6 g KCl.

48
Q

Calculate the molarity of the following solution:

4.00 g of KOH in 2.00 L of a KOH solution.

A

0.0356 M KOH.

49
Q

Calculate the molarity of the following solution:

5.85 g of NaCl in 400 mL of a KOH solution.

A

.250 M NaCl.

50
Q

Calculate the number of grams of HCl required to prepare 25.0 mL of a 6.00 M HCl solution.

A

5.47 g HCl.

51
Q

Calculate the number of litres of a 2.00 M KBr solution to obtain 3.00 mol KBr.

A

1.50 L of KBr solution.

52
Q

Calculate the number of litres of a 1.50 M NaCl solution to obtain 15.0 mol NaCl.

A

10 L of NaCl solution.

53
Q

Calculate the number of mL of a 0.800 M Ca(NO3)2 solution to obtain 0.0500 mol Ca(NO3)2.

A

62.5 mL.

54
Q

What is the final concentration when 2.0 L of a 6.0 M HCl solution is added to water so the final volume is 6.0 L?

A

2 M.

55
Q

What is the final concentration when water is added to 0.50 L of a 12.0 M NaOH solution to make 3.0 L of a diluted NaOH solution?

A

2 M NaOH.

56
Q

What is the final concentration when a 10 mL sample of a 25% (m/v) KOH solution is diluted with water so the final volume is 100 mL?

A

2.5% (m/v) KOH.

57
Q

What is the final concentration when a 50.0 mL sample of a 15% (m/v) H2SO4 solution is added to water to give a final volume of 250 mL?

A

3.0 % (m/v) H2SO4.

58
Q

Determine the final volume, in mL, when 1.5 M HCl solution is prepared from 20.0 mL of a 6.0 M HCl solution.

A

80 mL.

59
Q

Determine the final volume, in mL, when a 2.0% (m/v) LiCl solution is prepared from 50.0 mL of a 10.0% (m/v) (m/v) LiCl solution.

A

250 mL.

60
Q

What is the final volume, in mL, when a 0.500 M H3PO4 solution is prepared from 50.0 mL of a 6.00 M H3PO4 solution?

A

600 mL.

61
Q

What is the final volume, in mL, when a 5.0% (m/v) glucose solution is prepared from 75 mL of a 12% (m/v) glucose solution?

A

180 mL.

62
Q

Adding solute to a solution increases each of the following except

A) Boiling point
B) Molality.
C) Osmotic pressure
D) Freezing point

A

C) Osmotic pressure.

63
Q

True or False:

Colligative properties depend on the chemical identity of the solute.

A

False.

They depend on the concentration of the dissolved solute.

64
Q

Which is the correct balanced equation when the following strong electrolyte dissociates in water: CaCl2.

A

CaCl2(s) → Ca2+(aq) + 2Cl–(aq).

65
Q

Which is the correct balanced equation when the following strong electrolyte dissociates in water: K3PO4.

A

K3PO4(s) → 3K+(aq) + PO43–(aq).

66
Q

Which is the correct balanced equation when the following strong electrolyte dissociates in water: Fe(NO3)3.

A

Fe(NO3)3(s) → Fe3+(aq) + 3NO3–(aq).

67
Q

what are the equivalents for the following ion quantities:

1 mole of K+
3 moles of OH–
1 mole of Ca2+
3 moles of CO32–

A

1 mole of K+ = 1 Eq
3 moles of OH– = 3 Eq
1 mole of Ca2+ = 2 Eq
3 moles of CO32– = 6 Eq

68
Q

A physiological saline solution contains 154 mEq/L each of Na+ and Cl–. How many moles each of Na+ and Cl– are in 1.00 L of saline solution?

A

0.154 mol Na+ and 0.154 mol Cl–.

69
Q

Define what happens when a strong electrolyte dissolves in water.

A

Breaks down to ions only.

70
Q

Define what happens when a weak electrolyte dissolves in water.

A

Some ions form and some molecules.

71
Q

Define what happens when a nonelectrolyte dissolves in water.

A

Molecules only form.

72
Q

A solution contains 40 mEq/L of Cl– and 15 mEq/L of HPO42–. If Na+ is the only cation in solution, what is the Na+ concentration in mEq/L?

A

55 mEq/L.

73
Q

If “A” contains 2% NaCl
and is separated by a semipermeable membrane from “B” which contains
10% NaCl, which event will occur?

A

Water will flow from “A” to “B”.

74
Q

For each mole of solute added, the boiling point of 1kg of water is:

A

Raised by 0.51°C.

75
Q

1 mole of iron(III) chloride would raise the boiling point of 1kg of water by:

A

2.04°C.

FeCl3 -> 4 moles = 4 x 0.51°C

76
Q

1 mole of aluminum chloride would lower the freezing point of 1kg of water by:

A

7.44°C.

77
Q

A 10% (m/v) starch solution is separated from a 1% (m/v) starch solution by a semipermeable membrane. (Starch is a colloid). Which compartment has the higher osmotic pressure?

A

10% (m/v) starch solution.

A more concentrated solution will have a higher osmotic pressure.

78
Q

A 10% (m/v) starch solution is separated from a 1% (m/v) starch solution by a semipermeable membrane. (Starch is a colloid). In which direction will water flow initially?

A

From the 1% (m/v) starch solution to the 10% (m/v) starch solution.

79
Q

Dialysis is best described as a process which mimics the function of the:

A

Kidneys.

80
Q

True or False: The pores in a dialysis are smaller than those in an osmotic membrane in an effort to retain more nutrients.

A

False.

Pores in dialysis are bigger than those of osmosis.

81
Q

What is removed during hemodialysis?

A

Urea.

PSC: Chemistry (9 decks)

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