Unit 4 - Acids and Bases & Solubility

Question 0

What is an amphiprotic compound?

Answer 0

A compound that acts as both an acid and base

Question 1

Difference between monoprotic, diprotic, and polyprotic acids

Answer 1

Monoprotic acids can donate 1 proton (H+), diprotic acids can donate up to 2 protons, polyprotic acids can donate more than 2 protons

Question 2

T/F: Solutions are homogenous.

Answer 2

True, there is only one visible phase.

Question 3

Is the solute dissolved in the solvent or the solvent dissolved in the solute?

Answer 3

The solute is dissolved in the solvent.

Question 4

Define dissociation.

Answer 4

the separation of ions that occurs when an ionic compound dissolves in water

Question 5

How do you prepare a standard solution (from a solid)?

Answer 5

1. Calculate and measure the mass of solid needed using concentration equation (C = n/V)
2. Dissolve solid in small amount of pure water.
3. Transfer the solution into a volumetric flask and add pure water until desired volume is reached.

Question 6

How do you perform a dilution?

Answer 6

1. Calculate the volume of standard solution (vi, Ci) required to prepare the desired concentration and volume (Cf, vf) of diluted solution.
2. Add a small amount of pure water into a volumetric flask.
3. Measure and transfer the appropriate amount of initial solution into the flask.
4. Add the remaining water to reach desired volume.

Question 7

Define concentration.

Answer 7

The quantity of a given solute in a solution.

Question 8

Another term for molar concentration

Answer 8

Molarity - the number of moles that can be dissolved in 1L solution

Question 9

T/F: Solid ions do not dissociate into ions.

Answer 9

True

Question 10

What is the purpose of ionic equations?

Answer 10

Ionic equations show the dissociation of soluble ionic compounds in solution.

Question 11

What is a net ionic equation?

Answer 11

Ionic equations without the spectator ions

Question 12

Level of saturation is the point on the solubility curve is a) above the curve, b) below the curve, c) directly on the curve

Answer 12

a) supersaturated
b) unsaturated
c) saturated

Question 13

miscible & immiscible

Answer 13

Liquids that mix well are miscible.

Liquids that do not mix well are immiscible.

Question 14

Properties of acids

Answer 14

• pH lower than 7
• sour taste
• form hydronium ions (H3O+ or H+=H2O) in aqueous solutions
• react with many metals to form hydrogen gas
• electrolytes
• form H+ ions or protons in solution

Question 15

Properties of bases

Answer 15

• bitter taste
• feel slippery
• form hydroxyl ions (OH-) in solution
• pH higher than 7

Question 16

Define titration

Answer 16

A titration is a technique where a solution of known concentration is used to determine the concentration of an unknown solution.

Question 17

Svante Arrhenius theory of acids and bases

Answer 17

Acids: any compound which produces hydrogen ions (H+) in solution
Bases: any compound which produces hydroxide ions (OH-) in solution

Question 18

Bronsted-Lowry definition of acids and bases

Answer 18

Acids: a proton (H+) donor
Bases: a proton (H+) acceptor

Question 19

Lewis definition of acids and bases

Answer 19

Acids: electron pair donors
Bases: electron pair acceptors

Question 20

Define electrolyte

Answer 20

A compound that conducts electricity in aqueous solution