Exam 4

Question 1

Solute

Answer 1

a substance that’s present in a smaller amount

Question 2

Solvent

Answer 2

present in greatest abundance

Question 3

Aqueous solutions

Answer 3

solutions where water is the solvent

Question 4

molarity

Answer 4

describes how much solute is dissolved per volume of solution

Question 5

Equation for molarity

Answer 5

M= moles of solute/volume of solution L

Question 6

Example: Calculate the molarity of a solution made by dissolving 23.4g of solution sulfate (Na2SO4) in enough water to form 125ml solution.

Answer 6

1.33 M Na2SO4 (reference notes for worked out problem)

Question 7

True or False: The number of moles of solute remains the same in the concentrated and diluted forms of the solution

Answer 7

True

Question 8

Dilution equation

Answer 8

(MB)(VB)=(MA)(VA) or (Mconc.)(Vconc.)= (Mdilute)(Vdilute)

Question 9

Example: How many millimeters of 3.0 M H2SO4 are needed to make 450mL of 0.10 H2SO4?

Answer 9

V1=15mL

Question 10

Example: How many grams of Cu are required to react with 1.5L of 0.10M AgNO3?

Answer 10

4.8g Cu

Question 11

True or false: Ionic compounds don’t dissolve in water

Answer 11

False: Ionic compounds generally dissolve in water

Question 12

What happens to ionic compounds in solutions?

Answer 12

ionic compounds don’t dissociate into ions in solution
(Example: NaCl (s)–> Na(aq) + Cl(aq)

Question 13

True or False: Molecular compounds may dissolve in water

Answer 13

true

Question 14

What happens to molecular compounds in solutions?

Answer 14

Molecular compounds don’t dissociate in solution
(Example: C12H22O11(l) –> C12H22O11(aq)

Question 15

Are electrolytes strong or weak?

Answer 15

Electrolytes are both strong and weak

Question 16

What are electrolytes?

Answer 16

compounds that break into ions when dissolved in water, and they conduct electricity

Question 17

What are nonelectrolytes?

Answer 17

compounds that don’t break into ions when dissolved in water, and don’t conduct electricity

Question 18

Compounds Containing the following Ions are generally soluble with NO exceptions

Answer 18

Li, Na, K, NH4, NO3, C2H3O2

Question 19

Compounds Containing the following Ions are generally soluble with exceptions

Answer 19

Cl, Br, I, SO4

Question 20

What are the exceptions for soluble ions: Cl, Br, and I

Answer 20

When these ions pair with Ag, Hg2, or Pb, the resulting compounds are insoluble

Question 21

What are the exceptions for soluble ions: SO4

Answer 21

When SO4 pairs with Sr, Ba, Pb, Ag, or Ca, the resulting compounds are insoluble

Question 22

Is NaCl soluble or insoluble?

Answer 22

Always soluble

Question 23

Is AgCl soluble or insoluble?

Answer 23

insoluble exception

Question 24

Compounds that are generally insoluble and their exceptions:

Answer 24

OH and S
Exceptions for both: Li, Na, K, NH4
Exception for S : Ca, Sr, Ba
Exception for OH: Ca, Sr, Ba however when OH is paired with these ions the result is slightly soluble

Question 25

Is Fe2S3 soluble or insoluble?

Answer 25

always insoluble

Question 26

Is CaS souble or insoluble?

Answer 26

soluble exception

Question 27

What happens when two water-soluble compounds are mixed?

Answer 27

it produces an insoluble product (Example: Pb(NO3)2 (aq) + 2KI (aq) --> PbI2 (s) + 2KNO3 (aq)

Question 28

What do exchange/ double replacement reactions involve?

Answer 28

swapping ions in a solution (the cation from the first compound gets paired with the anion from the second compound) ( AX + BY --> AY + BX)

Question 29

Monoprotic acids

Answer 29

acids that ionize to form one H+ ion

Question 30

Diprotic acids

Answer 30

acids that ionize to form two H+ ions

Question 31

What are the 7 strong acids: (all other acids are weak acids)

Answer 31

1. hydroiodic (HI) 2. hydrobromic (HBr) 3. hydrochloric (HCl) 4. Sulfuric (H2SO4) 5. Nitric (HNO3) 6. Chloric (HClO3) 7. Perchloric (HClO4)

Question 32

Base

Answer 32

proton acceptors

Question 33

Strong bases: (all other bases are weak bases)

Answer 33

1. Alkali metals 2. Strontium (Sr(OH)2) 3. Calcium (Ca(OH)2 4. Barium (Ba(OH)2)