unit 4

Question 1

solution

Answer 1

Homogeneous mixture of two or more substances

Question 2

Aqueous solution

Answer 2

A solution in which water is the solvent

Question 3

solvent

Answer 3

The substance that does the dissolving

Question 4

solute

Answer 4

The substance that is dissolved

Question 5

concentration

Answer 5

ratio of solute to solution or solvent

Question 6

concentrated solution

Answer 6

Solution with large quantity of solute in solvent

Question 7

dilute solution

Answer 7

solution with small quantity of solute in solvent

Question 8

saturated solution

Answer 8

no more solute can dissolve

Question 9

supersaturated solution

Answer 9

More than maximum amount of solute is present, if one more crystal is added, the solute will precipitate out

Question 10

unsaturated solution

Answer 10

A solution that is not yet saturated

Question 11

solubility

Answer 11

The amount of solute which will be dissolved in a given volume of solvent at a specific temperature

Question 12

insoluble

Answer 12

Solubility less than 0.1 g in 100 mL

Question 13

Slightly soluble

Answer 13

Solubility between 0.1 g and 1 g in 100 mL

Question 14

soluble

Answer 14

Solubility is 1 g or greater in 100 mL

Question 15

dissociation

Answer 15

processed by which compounds separate into smaller molecules when in water
ex. CaCl2 —> Ca2+ (aq) + 2Cl - (aq)

Question 16

ionization

Answer 16

The formation of ions from polar covalent compounds when placed in water

Question 17

miscible

Answer 17

substances able to combine with each other in any proportion

Question 18

immiscible

Answer 18

substance is not able to combine with each other

Question 19

why water is the universal solvent

Answer 19

1) polarity
2) hydrogen bonding (water molecule is bent)
3) small molecule

Question 20

generalization of solubility

Answer 20

solids -high solubility at high temps
gases- high solubility at low temps
liquids- cannot generalize

Question 21

factors that affect solubility

Answer 21

1) increase surface area (large solids are harder to dissolve)
2) agitation (stir the solution)
3) increase temperature of solution

Question 22

how do you solve for solubility

Answer 22

g/mL = g/mL
then cross multiply

Question 23

solving for concentration

Answer 23

c = n/v
*volume must be in litres
1) find MM of solution
2) find moles using n= m/MM
3) find c

Question 24

how else can you represent concentration

Answer 24

square brackets

Question 25

what are the two ways to prepare a solution

Answer 25

from a solid: n = c x v 1) find n 2) find m or dilution: C1V1 = C2V2

Question 26

what is a total ionic equation

Answer 26

includes every ion

Question 27

what is a net ionic equation

Answer 27

simplified version

Question 28

what are spectator ions

Answer 28

does not change chemical reaction

Question 29

what does pH stand for

Answer 29

potential of hydrogen

Question 30

what are the pH levels

Answer 30

pH 7 is neutral pH less than 7 is acidic pH more than 7 is basic

Question 31

how do you do sig figs for concentration

Answer 31

the number of decimal places in pH is equal to the number of sig figs in concentration

Question 32

how to calculate pH

Answer 32

pH = -log [H+(aq)]

Question 33

how to calculate concentration

Answer 33

[H+(aq)] = 10^-pH

Question 34

what are the methods of measuring pH

Answer 34

pH paper- not precise pH meter- digital reading computer- pH probe

Question 35

what are the methods of measuring pH

Answer 35

pH paper- not precise pH meter- digital reading computer- pH probe