Solutions

Question 1

Matter:

Answer 1

Anything with mass and volume.

Question 2

Substance:

Answer 2

Matter with constant composition. All particles have the same properties. Eg. Water, helium

Question 3

Mixture:

Answer 3

Matter with variable composition, made from two or more substances. Eg. Sand, soil

Question 4

Element:

Answer 4

A substance made of atoms with the same atomic number. Eg. Lead, sodium

Question 5

Compound:

Answer 5

A substance made from two or more elements chemically combined. Eg. Carbon dioxide

Question 6

Homogenous Mixture:

Answer 6

A mixture made up of particles that are uniformly distributed. Eg. Saltwater

Question 7

Heterogeneous Mixture:

Answer 7

A mixture made up of particles that are not uniformly distributed. Eg. Raisin bran

Question 8

Solution:

Answer 8

Formed by dissolving a solute into a solvent.

Question 9

Solute:

Answer 9

The dissolved substance in a solution which may be solid, liquid, or gas.

Question 10

Solvent:

Answer 10

The medium containing a solute which can be any state of matter.

Question 11

True or false: All mixtures are solutions but not all solutions are mixtures

Answer 11

False.

Question 12

True or False: Not all mixtures are solutions, but all solutions are mixtures.

Answer 12

True.

Question 13

Why is water a common solvent?

Answer 13

Because it is a polar molecule.

Question 14

Hydration:

Answer 14

When H2O molecules gradually surround the ions.

Question 15

Dissociation:

Answer 15

The separation of ions from each other.

Question 16

Solvation:

Answer 16

The surrounding of solute particles by solvent.

Question 17

The dissolving process:

Answer 17

Molecules become more spread out, energy is lost or gained.

Question 18

Is dissolving a chemical or physical change?

Answer 18

Physical

Question 19

The steps of dissolving:

Answer 19

The solute breaks (endothermic), the solvent breaks (endothermic), the particles of both attract and create solvent bonds (exothermic).

Question 20

Miscible:

Answer 20

Liquids that dissolve in each other in all proportions.

Question 21

Immiscible:

Answer 21

Liquids that do not dissolve in other liquids at all.

Question 22

What is saturation at a molecular level?

Answer 22

Ions are crystallizing at the same rate that solid crystals dissolve.

Question 23

Electrolytes:

Answer 23

Solutions that conduct electricity and must contain ions.

Question 24

Factors that affect the rate of dissolving:

Answer 24

Particle size, temperature, nature of the particle, agitation/stirring.

Question 25

Factors that affect the solubility of substances in a solvent:

Answer 25

Temperature, pressure, miscibility.

Question 26

What factor most affects the solubility of a solid?

Answer 26

Temperature.

Question 27

What factor most affects the solubility of a gas?

Answer 27

Pressure.

Question 28

High solubility ionic compounds and bases dissociation:

Answer 28

Will dissociate into two ions when placed in water.

Question 29

Low solubility ionic compounds and bases dissociation:

Answer 29

Will not dissolve or dissociate in water.

Question 30

Strong Acids:

Answer 30

The 6 strong acids ionize completely to produce hydrogen ions and an anion

Question 31

Weak acids:

Answer 31

Do not ionize completely in water.

Question 32

High solubility molecular compound solubility:

Answer 32

Dissolve in water but do not dissociate

Question 33

High solubility molecular compounds:

Answer 33

H bonded compounds and sugar, group 17 elements.

Question 34

Low solubility molecular compound solubility:

Answer 34

Do not dissolve in water and do not dissociate.

Question 35

Low solubility molecular compounds:

Answer 35

No h-bonds.

Question 36

How to calculate grams per litre:

Answer 36

mass of solute/volume of solute

Question 37

How to calculate percent by mass (%m/v):

Answer 37

mass of solute (g)/volume of solution (mL) x 100

Question 38

How to calculate parts per million (ppm):

Answer 38

mass of solute (g)/volume of solution (mL) x 1000000

Question 39

How to calculate molar concentration (mol/L):

Answer 39

moles of solute (mol)/volume of solution (L)

Question 40

How to calculate mole ratio:

Answer 40

moles of required/moles of given

Question 41

What are the steps for preparing a solution?

Answer 41

1. Calculate the required mass of solute 2. Weigh (x) grams of solute and put in a clean, dry beaker 3. Dissolve (x) grams with half the amount of the final volume of distilled water 4. Transfer the solution into a volumetric flask using a funnel and rinse everything out 5. Fill the volumetric flask up to the line with an eyedropper 6. Stopper and invert.

Question 42

What is the formula for dilution?

Answer 42

C1V1 = C2V2

Question 43

What are the steps for the preparation of a solution by the dilution of a solution of higher concentration?

Answer 43

1. Calculate the volume of concentrated solution required 2. Transfer the concentrated solution into a dry beaker. Use a graduated cylinder for measuring (x) millilitres of concentrated solution 3. Pipet the solution into a clean, dry 100 mL volumetric flask 4. Add distilled water to the line using an eyedropper 5. Stopper and invert

Question 44

When writing the equations for a chemical reaction, what are the three different steps?

Answer 44

Nonionic, total ionic, and net ionic.