Chemistry Test 3

Question 1

The quantitative way to express solutions

Answer 1

Molarity = moles solute/liter solution (M=mol/L)

Question 2

Molarity

Answer 2

The quantitative way to express solution concentration

Question 3

How many mL of a 0.125 M NaOH solution contain 0.255 mol of NaOH?

Answer 3

2040mL

Question 4

How many grams of NaOH is required to make 1L of 0.5M NaOH?

Answer 4

20g NaOH

Question 5

Dilution

Answer 5

The process of lowering the concentration of a solution by adding more solvent

Question 6

Equation used to calculate dilutions

Answer 6

Volume(initial) * Molarity(initial) = volume(final) * molarity(final)

Question 7

What is the final molarity of a NaCl solution when 1.03L of 1.50M NaCl is diluted to 10.0L?

Answer 7

0.155M

Question 8

What volume of 1.00M CuSO4 is needed to make 250.0mL 0.100M CuSO4 solution?

Answer 8

0.025L

Question 9

Non-electrolyte

Answer 9

Compounds that remain intact when dissolved (molecules except acids)

Question 10

Electrolytes

Answer 10

Compounds that dissociate into ions and conduct electricity in water (ionic compounds and acids)

Question 11

Strong electrolyte

Answer 11

Any compound that COMPLETELY dissociate when dissolved in water

Question 12

Weak electrolyte

Answer 12

Most acids that PARTIALLY dissociate when dissolved in water

Question 13

Double displacement

Answer 13

Type of reaction in which the ions of two ionic compounds exchange places to form two new compounds. Like ions swap places with each other

Question 14

A reaction in solution where all reactants and products and reactants are written as neutral compounds

Answer 14

molecular equation

Question 15

Ions that are identical on both sides of the reaction

Answer 15

spectator ions

Question 16

Write the total ionic and net ionic equations:
Li2SO4(aq)+Ca(NO3)2(aq) —> 2LiNO3(aq)+CaSO4(s)

Answer 16

Li+(aq) + SO42-(aq) + Ca2+(aq) + 2NO3-(aq) –> 2Li+(aq) + 2NO3-(aq) + CaSO4(s)

Ca2+(aq) + SO42-(aq) –> CaSO4(s)

Question 17

Write the total ionic and net ionic equations:
2(NH4)3PO4(aq)+3Na2SO4(aq) —> 2Na3PO4(aq)+3(NH4)2SO(aq)

Answer 17

6NH4+(aq) + 2PO43-(aq) + 6Na+(aq) + 3SO42-(aq) –> 6Na+(aq) + 2PO43-(aq) + 6NH4+(aq) + 3SO4-2(aq)

They all cancel each other out = no net equation

Question 18

Does a chemical reaction occur when ammonium phosphate and sodium sulfate are mixed?

Answer 18

no; because the products and reactants are the same

Question 19

A precipitate forms when aqueous solutions of ammonium sulfate and calcium chloride are mixed. Write the net ionic equation for the reaction and identify any spectator ions present.

Answer 19

(NH4)2SO4(aq) + CaCl2(aq) —> 2NH4Cl(aq) + CaSO4(s)

Ca2+(aq) + SO42-(aq) —> CaSO4(s) (Net)

NH4+, Cl- spectator ions

Question 20

Acids are molecular compounds that ionize to produce what?

Answer 20

hydronium (H3O+) in water

Question 21

Acids that ionize completely

Answer 21

strong acids

Question 22

What are the 6 strong acids?

Answer 22

Hydrochloric acid (HCl)(aq)
Hydrobromic acid (HBr)(aq)
Hydroiodic acid (HI)(aq)
Sulfuric acid (H2SO4)(aq)
Nitric acid (HNO3)(aq)
Perchloric acid (HClO4)(aq)

Question 23

What is the name of the acids that contain more than one ionizable proton (H+) and release them sequentially

Question 24

What do Arrhenius bases produce

Answer 24

hydroxide in water

Question 25

What is the most common weak base?

Answer 25

Ammonia

Question 26

An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a …

Answer 26

transfer of electrons between compounds

Question 27

Numerical value given to an atom in a molecule or compound

Answer 27

oxidation number/state

Question 28

6 rules for determining oxidation numbers

Question 29

What are the two forms of energy?

Answer 29

potential and kinetic