unit 8 vocab

Question 1

carboxylic acid

Answer 1

often found in substances derived from living organisms

Question 2

alkaloids

Answer 2

organic bases found in plants; often poisonous

Question 3

arrhenius acid

Answer 3

produces H+ in an aqueous solution

Question 4

arrhenius base

Answer 4

produces OH- in an aqueous solution

Question 5

bronstead-lowry acid

Answer 5

proton (H+ ion) donor; becomes a conjugate base

Question 6

bronstead-lowry base

Answer 6

proton (H+ ion) receiver; becomes a conjugate acid

Question 7

monoprotic acid

Answer 7

an acid that only contains one ionizable proton

Question 8

diprotic acid

Answer 8

an acid containing two ionizable protons

Question 9

acid ionization constant (Ka)

Answer 9

the equilibrium constant for the ionization of a weak acid; used to compare the relative strengths of weak acids

Question 10

autoionization

Answer 10

when water acts as an acid and a base with itself

Question 11

Kw

Answer 11

ion product constant for water; at 25 C, Kw = 1.0 * 10^-14

Question 12

sig fig rule for log to pH

Answer 12

if the log has two sig figs, the pH has two decimal places

Question 13

percent ionization

Answer 13

the ratio of the concentration of ionized acid to the initial concentration of that acid, times 100%

Question 14

polyprotic acid

Answer 14

ionizes in steps, each step has its own Ka

Question 15

binary acid

Answer 15

an acid with H and only one other element

Question 16

oxyacid/oxoacid

Answer 16

an acid with H bonded to O and O is bonded with another element

Question 17

adduct

Answer 17

the product of a lewis acid-base reaction

Question 18

4 ways to make a buffer

Answer 18

1. partial neutralization of weak acid and strong base
2. partial neutralization of weak base and strong acid
3. weak acid and salt of its conjugate base
4. weak base and salt of its conjugate acid

Question 19

when an acid is strong, its conjugate base is..

Answer 19

weak

Question 20

adding a strong acid or base to a buffer (steps)

Answer 20

1. initial mol
2. mol of added
3. add base to base n subtract base from acid or other way around
4. find new concentration
5. use henderson-hasselbalch equation to find pH

Question 21

henderson-hasselbalch equation

Answer 21

pH = -log Ka + log [b]/[a]

Question 22

when combining strong acid and strong base, at the equivalence point…

Answer 22

pH is 7

Question 23

when combining strong acid and weak base, at the equivalence point…

Answer 23

pH is acidic

Question 24

when combining strong base and weak acid, at the equivalence point…

Answer 24

pH is basic

Question 25

titration with weak acid or base steps:

Answer 25

1. which is strong, acid or base?
2. find missing K
3. find moles
4. find L of missing substance
5. y = mol/total L
6. missing K = x^2/y-x
7. find pH from there (-log it)

Question 26

Ka =

Answer 26

x^2 over initial concentration

Question 27

[OH-][H+] =

Answer 27

1 * 10^-14

Question 28

LeChatlier’s principle

Answer 28

when an equilibrium is stressed, it’ll adjust to relieve the stress