Unit 3: Solutions Outcome 1

Question 1

What is a pure substance?

Answer 1

Only 1 type of particle

Question 2

What is a mixture?

Answer 2

Contain 2/more pure substances

Question 3

What does homogenous mean?

Answer 3

Look the same throughout

Question 4

What does heterogenous mean?

Answer 4

Can see different components

Question 5

What is an element?

Answer 5

Made up of 1 type of atom

Question 6

What is a compound?

Answer 6

Made up of two or more elements

Question 7

What is a solution?

Answer 7

Homogenous mixtures composed of a solute and a solvent

Question 8

What is a solute?

Answer 8

A substance that is dissolved

Question 9

What is a solvent?

Answer 9

The medium a solute is disoled in

Question 10

What does acqueous(aq) mean?

Answer 10

Dissolved in water

Question 11

What are the two ways to classify aqueous solution?

Answer 11

1- electrolytes (polar) or non-electrolytes (non-polar)
2- acid, base, or neutral

Question 12

What are electrolytes?

Answer 12

Compounds that conduct electricity in solution

Question 13

What is non-electrolytes?

Answer 13

Compounds that don’t conduct electricity in solution

Question 14

What are acids?

Answer 14

A compound that contains hydrogen acting as metal and dissolves in water to make a solution with a pH less than 7

Question 15

What are the traits of acids?

Answer 15

• state is (aq)
• has H at front or COOH at end
• turns litmus red

Question 16

What are the traits of bases?

Answer 16

A compound taht dissolves in water water to make a solution with pH more than 7

Question 17

What are the traits of bases?

Answer 17

• state is (aq)
• has OH at the end
• turns litmus blue

Question 18

What are the generalizations about electrolytes?

Answer 18

Acids, Bases, Ionic Compounds = electrolytes

Molecular Compounds = non=electrolytes

Question 19

What is dissociation?

Answer 19

Seperation of an ionic compound into its ions in water

Question 20

What is ionization?

Answer 20

Process by which a molecule i s converted into ion (s)

Question 21

What occurs when bonds break?

Answer 21

When bonds break, energy must be absorbed from surroundings (endothermic reaction where the surroundings cool down)

Question 22

What occurs when bonds form?

Answer 22

When bonds form, energy is released into surroundings (exothermic reaction where surroundings heat up)

Question 23

What is concentration?

Answer 23

Ratio of quantity of teh solute to the quantity of the solution

Question 24

What is a dilute solution?

Answer 24

Relatively small quanitty of solute when compared to volume of solution

Question 25

What is concentrated solution?

Answer 25

Relatively large quantity of solute when compared to volume of solution

Question 26

What are the different ways of expressing concentration?

Answer 26

- percentage (v/v, w/v, w/w) - parts per million concentration - amount concentration

Question 27

What is saturated solubility?

Answer 27

A solution in which no more solute can be dissolved at a specific temp.

Question 28

What is solubility?

Answer 28

Concentration of a saturated solution (same unit as concentration but should be accompanied by a temp. value because solubility with temp)

Question 29

What is solubility in water with solids?

Answer 29

Have higher solubility in wataer at higher temp.s

Question 29

What is solubility in water with gases?

Answer 29

- higher solubility at lower temps - higher solubility at higher pressures

Question 29

What is solubility in water with liquids?

Answer 29

Hard to make generalizations (miscible or immiscible)

Question 30

What is miscible?

Answer 30

Liquids that mix with water

Question 31

What is immiscible?

Answer 31

Liquids that don't mix with water

Question 32

What is solubility in water with elements?

Answer 32

- have low solubility in water (not polar, can't ionize/dissoziate, in most stable form already)

Question 33

What is ion concentration?

Answer 33

A whole number multiple of the compound concentration

Question 34

What is a standard solution?

Answer 34

Solution that has a knonw, accurate concentration

Question 35

What are the two ways to make a standard solution?

Answer 35

- by dissolving a solid - by diluting a more concentrated solution

Question 36

What are the steps to preparing a standard solution from a solid?

Answer 36

1. Calculate what mass of solid is needed to make the required volume and concentration of solution (n= cv) (m= nM) 2. Measure out the mass of solid using an electronic scale 3. Dissolve the solid in half of the required volume water 4. Transfer the dissolved solid into a volumetric flask (make sure volumetric flask is the size needed) 5. Fill the volumetric flask to the marking for the volume of the solution needed 6. Place top on volumetric flask and invert to mix

Question 37

What is a stock solution?

Answer 37

An initial, usually concentrated, solution from which samples are taken for a dilution

Question 38

What are the steps to make a standard solution using dilution?

Answer 38

1. Calculate the volume of the stock solution needed to make the solution (C1V1= C2V2) 2. Measure the volume of the stock solution using a pipette 3. Add the volume of stock solution to the appropriate sized volumetric flask 4. Fill volumetric flask to line 5. Put on cap and invert to mix