Honors - Unit 7 - Solutions

Question 1

Intermolecular Forces

Answer 1

Attractive forces BETWEEN molecules.

Van Der Waals or London Dispersion Forces are the weakest type of intermolecular force and hydrogen bonds are the strongest.

Question 2

Intramolecular Forces

Answer 2

Attractive forces WITHIN a molecule (Ionic & Covalent Bonds)

These bonds are stronger than intermolecular forces.

Question 3

Solution

Answer 3

Solute + Solvent

Question 4

The Dissolving Process

Answer 4

1. The solvent surrounds the outer surface of the solute.
2. Individual Solute Ions are “stripped” away from the surface due to their attraction to the solvent particles.
3. This exposes more particles to the solvent and thus the process continues.

Question 5

How can you make things dissolve faster?

Answer 5

1. Agitation (stirring)
2. Temperature
3. Increase Surface Area (Grind or Crush)

Question 6

“Like Dissolves Like”

Answer 6

Not everything will dissolve in everything. Polar solvents dissolve polar solutes. Nonpolar solutes dissolve nonpolar solutes. Water is polar so it dissolves polar solutes.

Question 7

Solvent

Answer 7

The component doing the dissolving.

The component in the largest amount.

Water is the universal solvent.

Question 8

Solute

Answer 8

The component being dissolved.

The component in the smallest amount.

Question 9

Unsaturated

Answer 9

Contains less solute than it can at that temperature.

Question 10

Saturated

Answer 10

Contains as much solute as it can at that temperature.

If you add more solute it will not dissolve.

Question 11

Supersaturated

Answer 11

Contains more solute than it should at that temperature. Ussually the solution is heated to allow that much solute to dissolve and then cooled back down.

If you add solute to a supersaturated solution the “super” part (amount over the saturation point) will crystallize out of solution.

Question 12

Concentrated

Answer 12

A relatively large amount of solute.

Question 13

Dilute

Answer 13

Relatively small amount of solute.

Question 14

Solubility Curve

Answer 14

Used to determine the mass of solute in 100g (100ml) of water at a given temperature.

Question 15

What is the solubility of Potassium Nitrate at 50 C?

Answer 15

86 g Potassium Nitrate

Question 16

How to determine if a solution is unsaturated, saturated, or supersaturated.

Answer 16

Add more solute and observe the results.

Question 17

Is the solution unsaturated, saturated, or supersaturated, if I have 30 g of Potassium Nitrate in 100 g of Water at 30 C?

Answer 17

Unsaturated

Question 18

Is the solution unsaturated, saturated, or supersaturated, if I have 60g of Potassium Nitrate in 100g of Water at 30 C?

Answer 18

Supersaturated

Question 19

How much solute will not dissolve if I have 80g of Potassium Nitrate in 100g of Water at 30C?

Answer 19

35g Potassium Nitrate

Question 20

How much more solute could I dissolve if I have 10g of Potassium Nitrate in 100g of Water at 30C?

Answer 20

~32g of Potassium Nitrate

Question 21

How much solute would crystallize out of solution once a solution of 85g of Potassium Nitrate in 100g of Water at 50C is cooled to 20C?

Answer 21

55g Potassium Nitrate

Question 22

What is the molarity of a solution made by dissolving 2.5g of NaCl in enough water to make 125 ml of solution?

Answer 22

Question 23

Molarity

Answer 23

Expression of Concentration ( [] )

Question 24

Percent Mass

Answer 24

Question 25

Calculate the concentration of the solute in the diluted solution: 1.00mL of 0.50M NH4Cl diluted to 250.0mL

Answer 25

M₁V₁ = M₂V₂ M₁ = (M₂V₂)/(V₁) M₁ = (0.5 M x 1 ml)/(250 ml) M₁ = 0.0020M

Question 26

Calculate the volume required to prepare the diluted solution: Given 6.0M NaOH; need 5.0L of 0.10M NaOH.

Answer 26

M₁V₁ = M₂V₂ V₁ = (M₂V₂)/(M₁) V₁ = 0.083L

Question 27

## Footnote What is the molarity of a solution in which 58 g of NaCl are dissolved in 1.0 L of solution?

Answer 27

## Footnote 1.0 M

Question 28

## Footnote What is the molarity of a solution in which 10.0 g of AgNO₃ is dissolved in 500 ml of solution?

Answer 28

## Footnote 0.118 M AgNO₃

Question 29

## Footnote How many grams of KNO₃ should be used to prepare 2.00 L of a .500 M solution?

Answer 29

## Footnote 101 g KNO₃

Question 30

## Footnote To what volume should 5.0 g of KCl be made in order to prepare a .25 M solution?

Answer 30

## Footnote 0.27 L KCl

Question 31

Colligative Properties

Answer 31

properties that depend on the concentration of solute, but not on the chemical identity of the solute. (Vapor Pressure Lowering, Boiling Point Elevation, Freezing Point Depression, and Osmotic Pressure)

Question 32

How to determine if a solution is unsaturated, saturated, or supersaturated.

Answer 32

Add more solute and observe the results.

Question 33

How much solute will not dissolve if I have 80g of Potassium Nitrate in 100g of Water at 30C?

Answer 33

35g Potassium Nitrate

Question 34

Is the solution unsaturated, saturated, or supersaturated, if I have 60g of Potassium Nitrate in 100g of Water at 30 C?

Answer 34

Supersaturated

Question 35

Is the solution unsaturated, saturated, or supersaturated, if I have 30 g of Potassium Nitrate in 100 g of Water at 30 C?

Answer 35

Unsaturated

Question 36

What is the solubility of Potassium Nitrate at 50 C?

Answer 36

86 g Potassium Nitrate

Question 37

What is the effect of pressure on solubility?

Answer 37

Question 38

What is the effect of temperature on solubility?

Answer 38

Question 39

immiscible

Answer 39

Will not dissolve in water.

Question 40

miscible

Answer 40

Will dissolve in water.