Buffers and Titration (5/11)

Question 1

Buffer

Answer 1

A solution that resists change in pH when an acid or base is added. It is created from a mixture of a weak acid and its conjugate base or vise versa

Question 2

Henderson-Hasselbalch

Answer 2

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

Question 3

Bicarbonate buffering system

Answer 3

weak acid of bicarbonate and weak base of HCO3-

Question 4

When adding an acid or the solution…

Answer 4

[A-] become [A- - 1] and [HA] becomes [HA + 1]

Question 5

If more acid than conjugate base in initial solution…

Answer 5

then, buffering capacity decreases

Question 6

Neutralization point

Answer 6

Moles of equivalents of acid = mole of equivalents of base

Question 7

Normality Equation

Answer 7

N=[moles OH]/liters of solution

Question 8

For mono or diprotic reaction

Answer 8

nC1V1=nC2V2
where n=1 for mono
n is the number of H+ ions or OH- ions

Question 9

Indicators

Answer 9

weak acids or bases that take on colors when protonated or deprotonated (changes in pH)

Question 10

Equivalence point

Answer 10

moles acid=moles base and is fully neutralized

Question 11

Half equivalence point

Answer 11

half titrate needed to add to reach equivalence point is added

Question 12

Weak acid/strong base

Answer 12

neutralization is always above a pH of 7