solutions and solubility

Question 1

What is a mixture?

Answer 1

A substance made by combining elements or compounds physically, not chemically

Question 2

What are the two kinds of mixture?

Answer 2

Homogeneous and heterogeneous

Question 3

What is a homogeneous mixture?

Answer 3

A mixture where particles are evenly distributed throughout (cannot be separated physically)
also sometimes called solutions

Question 4

What is a heterogeneous mixture?

Answer 4

A mixture where particles are not evenly mixed and can be separated by physical means

Question 5

What is a soluble substance mean?

Answer 5

If a substance is soluble, it will completely dissolve in the solution

Question 6

What is an aqueous solution?

Answer 6

A solution where the solvent is water

Question 7

What is a precipitate?

Answer 7

an insoluble substance that separates from the solution

Question 8

What is solubility?

Answer 8

The ability of a solute to dissolve in a solvent

Question 9

What is a solute?

Answer 9

The substance that does the dissolving in a solution

Question 10

What is a solvent?

Answer 10

The substance that dissolves in a solution

Question 11

What is random molecular motion?

Answer 11

The unpredictable movement and breaking apart of molecules or atoms within a solution

Question 12

If NaCl mixes with H2O, which one is the solute and why?

Answer 12

H2O is the solute because the concentration of water rin the ocean is much higher than the concentration of salt.

Question 13

What is a saturated solution?

Answer 13

A solution that contains the maximum amount of solute possible. No more solute added will dissolve

Question 14

What is an unsaturated solution?

Answer 14

A solution that contains less than the maximum amount of solute possible
ie if you added more solute, it would dissolve

Question 15

What is a supersaturated solution?

Answer 15

A solution that holds more solute than normally possible (the solution was heated to a high temp and more solute was added to saturate the hot solution and then the solution is cooled quickly)

Question 16

What is a colloid?

Answer 16

A homogeneous solution that is made of larger particles but the substance is still evenly distributed throughout

Question 17

List the 4 types of colloids

Answer 17

• sol
• emulsion
• foam
• aerosol

Question 18

What is a suspension?

Answer 18

A mixture that looks uniform when stirred or shaken but settles into different layers

Question 19

What is a sol?

Answer 19

A colloidal suspension (looks uniform when stirred, separates into layers) that has solid particles in a liquid

Question 20

What is an emulsion?

Answer 20

A colloidal suspension (looks uniform when stirred, separates into layers) that is formed between two liquids

Question 21

What is a foam?

Answer 21

A colloidal suspension (looks uniform when stirred, separated into layers) that is formed when multiple gas particles are trapped in a solid or liquid

Question 22

What is an aerosol?

Answer 22

A colloidal suspension that has small solid or liquid particles spread evenly throughout a gas

Question 23

Ionic compounds dissolve in what kind of solvent?

Answer 23

Aqueous solvents

Question 24

Why do ionic compounds dissolve well in aqueous solvents? What is the process called?

Answer 24

The water is polar and pulls on the different charges in the ionic compound, causing the ionic crystal bonds to separate and break up into their original ions. This process is called “dissociation of ions”

Question 25

what kind of reaction is one of the most common types of chemical reaction to occur in an aqueous solution?

Answer 25

a precipitation reaction. where an insoluble liquid called a precipitate is formed.

Question 26

What is a spectator ion?

Answer 26

An ion that is not involved in the formation of a precipitate in an aqueous solution. not chemically changed over the course of a reaction

Question 27

What is a net ionic equation

Answer 27

a chemical equation that only shows the ions taking part in the reaction and ignores the spectator ions. only includes ions that are chemically changed in the overall reaction

Question 28

All ____ and ____ are soluble (one type of metal and one type of salt)

Answer 28

alkali metals

ammonium salts

Question 29

All ___, _____, and ____ are soluble (all end in -ate)

Answer 29

nitrates
chlorates
per chlorates
(all -ates contain an oxygen)

Question 30

All ___, ____, and ____ are insoluble

Answer 30

silver, lead 2+, and mercury + salts are insoluble

Question 31

All ____, ____, and ______ are soluble (all contain a halogen)

Answer 31

chloride
bromide
iodide

Question 32

What is an electrolyte?

Answer 32

A substance that will conduct electricity when dissolved in water

Question 33

What is a nonelectrolyte?

Answer 33

A substance that will not conduct electricity when dissolved in water

Question 34

What factors affect solubility and why? (2)

Answer 34

Temperature (increases solubility for solids as temp increases and decreases solubility for gases as temp increases), and pressure (affects gases when mixed with liquids, as pressure increases, the solubility of gases increases too)

Question 35

What is molarity?

Answer 35

Mol/L, mols of solute/liters of solution(or solvent - bc the solvent is dissolving the solute, just put the liters of solvent), or n/v

Question 36

What is molality?

Answer 36

The number of moles of solute dissolvent in 1 kg of solvent (mol/kg)

Question 37

When is molality important?

Answer 37

When you are adding solute to a solvent in an experiment and figuring out the colligative properties

Question 38

What is a colligative property? Give some examples

Answer 38

A physical property of a solution that depends on the ratio of the amount of solute to the solvent
freezing point depression, boiling point elevation

Question 39

Which is temperature-dependent, molarity or molality, and why?

Answer 39

Molarity is temperature-dependent because when the temp of a solution increases, so does the volume, and molarity is n/v

Question 40

When is molality used?

Answer 40

When the mass of a solvent must be known for a given calculation.

Question 41

What is the equation for calculating the overall charge in a covalent compound?

Answer 41

-(number of valence electrons - number of non-bonding electrons - (number of sharing electrons * 1/2))

Question 42

How is solubility measured?

Answer 42

Grams per liter, or the mass of the solute in grams/ the volume of the solvent in liters

Question 43

What is a dilution?

Answer 43

When the concentration of a solution is decreased

Question 44

When does dilution occur?

Answer 44

When more solvent is added to a fixed amount of solute

Question 45

What kind of lab equipment is used for dilutions?

Answer 45

Volumetric flasks

Question 46

What is the dilution formula and what does it tell you?

Answer 46

How much solvent to add to dilute a solution
M1V1=M2V2
(m1 =concentration/molarity of the starting solution, v1 = volume of starting solution, m2 = concentration/molarity of ending solution, v2 = volume of ending solution)