Ch 4 Solubility, Precipitation, Titration

Question 1

aqueous solution

Answer 1

liquid solution made with a solute and solvent

Question 2

aqueous solutions and electrolytes

Answer 2

some aqueous solutions form ions within a solution that are called electrolytes; others are called nonelectrolytes

Question 3

electrolytes

Answer 3

can be observed with lightbulbs; ions in the solution are conductors’ electrolytes are either strong, weak, or non

Question 4

ionic compounds in water

Answer 4

when an ionic compound dissolves it’s component ions disassociate; because Oxygen in water is slightly negative and Hydrogens are slightly positive, they separately attract the solute’s ions and disassociate them

Question 5

ions in a solution are…

Answer 5

stable, ions not in a solution aren’t really stable

Question 6

molecular compounds in water

Answer 6

molecules remain intact and disperse as nonelectrolytes; acids are the exceptions here

Question 7

writing aqueous solution equations

Answer 7

if weak electrolytes, the arrows flowing both ways indicate only small amounts of ions disassociated; if a strong electrolyte or nonelectrolyte, a one way arrow is used

Question 8

strong electrolyte reactants

Answer 8

ionic compounds and acids

Question 9

precipitation reaction

Answer 9

when two pairs of ionic compounds switch ions to form new ions; one of the new products is a compound

Question 10

soluble ionic compounds

Answer 10

all nitrates and acetates.
Chloride, Bromide, and Iodide are soluble except with Silver, Mercuriy and Lead.
Sulfates except with Strontium, Barium, Mercury, and Lead

Question 11

insoluble ionic compounds

Answer 11

Sulfide and Hydroxide except with ammonium, calcium, strontium, barium, and all alkalis.
Carbonate and Phosphate except with ammonium and all alkalis.

Question 12

how do you identify the precipitate?

Answer 12

the precipitate is identified using solubility rules, if one of the new ionic compounds are insoluble, that’s your precipitate

Question 13

ionic equations

Answer 13

complete ionic is when you pull all compounds apart and list all elements as ions; the net ionic equation identifies which ions created a new compound end excludes spectator ions

Question 14

acids and bases when dissolved

Answer 14

acids are dissolved into H ions and disassociate; bases accept H ions and disassociate into OH ions.

Question 15

strength of electrolytes

Answer 15

all ionic are strong, strong acids are strong; weak acids and bases are weak; no ionic compounds are weak; all other molecular compounds are nonelectrolytes and no ionic compounds are nonelectrolytes

Question 16

neutralization reactions

Answer 16

when an acid and base react they neutralize each other and the products don’t share any properties; one product is a salt

Question 17

salt formation

Answer 17

occurs in neutralization when the cation is from a base and the anion is from an acid; metal hydroxide and an acid always makes a salt

Question 18

gas formation from acids and bases

Answer 18

non hydroxide bases sometimes produce gases when reacted with an acid; carbonates and bicarbonates create carbonic acid (which is unstable) that then decomposes to water and CO2

Question 19

molarity

Answer 19

mol/Liter

Question 20

Dilution

Answer 20

the moles of solute never change, but the total volume increases by adding solvent.

Question 21

Strong Acids

Answer 21

HI
HBr
HClO4
HCl
HClO3
H2SO4
HNO3

Question 22

Strong Bases

Answer 22

NaOH
KOH
LiOH
RbOH
CsOH
Ca(OH)2
Ba(OH)2
Sr(OH)2