mini test 4

Question 1

Arrhenius acid

Answer 1

increase the H+ concentration in the solution

Question 2

Arrhenius base

Answer 2

increase the OH- concentration in the solution

Question 3

Lewis acid

Answer 3

electron acceptor

Question 4

Lewis base

Answer 4

electron donor

For example, the ligands of the coordinate ions are an example of a Lewis base

Question 5

bronsted Lowry Acid

Answer 5

donates a proton (H+) then forms an acid conjugate base

Question 6

Bronsted Lowry Base

Answer 6

accepts a proton (H+), then forms a bases conjugate acid

Question 7

buffer

Answer 7

resits change in ph

made by a weak acid/base and its conjugate (usually in the form of a salt)

can calculate the pH from the H-H equation

A 1:1 ratio is best, in a titration, the buffer region is anywhere before the equilibrium point because it is resisting change and neutralization

Question 8

coordinate covalent bonds

Answer 8

one of the two provides both electrons in the bonding pair

Question 9

complex ions

Answer 9

made of coordinate bond, bonded to one or more Lewis bases (called ligands)

In general, we assume that the bond btwn the ligands and the metal cation/anion is so strong its stable enough not to dissociate

Question 10

Strong acids

Answer 10

HCl
HI
HBr
H2SO4
HNO3
HClO4

**Increase in Ka=stronger acid

Question 11

strong bases

Answer 11

group 1 A
group 2 A (starting after Ca)

**incease in Kb=stronger base

Question 12

percent ionization

Answer 12

how much acid/base will be ionized, increase with the strength of the acid

H+/HA * 100

Question 13

autoionization of water

Answer 13

water molecules spontaneously break into ions

Ka*Kb=Kw
This can especially be used to figure out the Ka/Kb of the conjugates that you are using in a buffer

Question 14

titrations

Answer 14

a process of neutralization to figure out the concentration of the unknown acid/base

this is a weak acid/base + a stronger acid/base

equivalence point is the same number of moles according to stoichiometric ratio

Question 15

solubility rules

Answer 15

NAG SAG
(nitrates, acetates, group 1, sulfates, ammonium, group 17)

EXCEPTIONS
not soluble with sulfates or group 17, PMS (Pb, mercury, silver)
also not soluble with sulfates CASTRO BEAR (Ca, Sr, Ba)

Question 16

weak acid/base

Answer 16

to figure out the pH, need a RICE table (and sometimes a BCA table) because not all the ions dissociate the same amount

Question 17

Ksp

Answer 17

the solubility constant helps to find the molar solubility of a substance being dissolved

assume that the Ksp is a precipitate, not being dissolved completely

Ksp= [products] **no reactants needed because the reactants are SOLIDS and so the concentration isn’t going to change

an addition of an ion is going to decrease the solubility (think more to dissolve)
lower the pH=more soluble

Question 18

Kf

Answer 18

formation constant, the formation of a complex ion

assuming it forms completely