Kaplan General Chemistry: Chapter 10 Acids and Bases

Question 1

pka is the PH where:

Answer 1

HA = A-

Question 2

low pka means

Answer 2

more acidic

Question 3

low ka means

Answer 3

less acidic

Question 4

high ka means

Answer 4

more acidic

Question 5

formula for pka

Answer 5

pka = -log(Ka)
pka= -log (n x10^m)
pka = m-0.n

Question 6

ka x kb = kw =

Answer 6

10^-14

Question 7

equation for the equivalence point

Answer 7

NaVa = NbVb

Question 8

Henderson-Hasselbach equation

Answer 8

pH = pka + log[A-]/[HA]

Question 9

phosphorous acid compound. What is the conjugate base?

Answer 9

phosphorus acid : H3PO3

conjugate base: phosphite

Question 10

phosphoric acid compound. what is the conjugate base

Answer 10

phosphoric acid H3PO4

conjugate base: phosphate

Question 11

hypophosphorous acid

Answer 11

H3PO2

Question 12

perphosphoric acid

Answer 12

H3PO5

Question 13

How can PI be obtained for acidic amino acids? basic amino acids?

Answer 13

PI can be obtained by averaging 2 acidic pka values for acidic AAs, or 2 basic pka values for basic AAs.

Question 14

what is the equivalence point for a strong acid and strong base titration?

Answer 14

7

Question 15

equivalence point for strong acid and weak base equivalence point

Answer 15

less than 7

Question 16

equivalence point for weak acid and strong base equivalence point

Answer 16

over 7

Question 17

an indicator must be ___ than the acid or base being titrated

Answer 17

must be weaker

Question 18

an indicator chosen for a titration should have a pka:

Answer 18

close to the pH of the expected equivalence point

Question 19

when a solution is optimally buffered, what does ph equal to?

Answer 19

ph = pka
pOH = pkb.

Question 20

what is the equality at the equivalence point? at half the equivalence point?

Answer 20

at equivalence point: [HA]=[A-]

at HALF the equivalence point: pka = pH