pH and buffers

Question 1

it is considered a weak electrolyte. It is amphoteric and amphiphrotic in nature

Answer 1

water

Question 2

what is amphoteric

Answer 2

can react to both acid and base

Question 3

what is amphiphrotic?

Answer 3

can both accept and donate a proton/ H

Question 4

What is buffer?

Answer 4

a mixture of a weak electrolyte with its salt

Function: resist drastic/ great/ marked change in pH of a system even upon the addition of either acid or base

Question 5

2 types of buffers

Answer 5

Acid buffer and base buffer

Question 6

acid buffer?

Answer 6

mixture of weak acid+ salt of weak acid

E.g Hac + NaAc (KAc, MgAc)

Question 7

base buffer

Answer 7

mixture of WB + salt of WB

E.g. NH4OH+ NH4Cl
NH4OH + NH4NO3

Question 8

Neutralization

Answer 8

base + acid = salt+ water

NaOH+ HCl = NaCl + H2O

Question 9

Acids and Bases Theory

Answer 9

Arrhenius/ ionic
Lewis
Bronsted-lowry theory/ conjugate acid- base pair theory

Question 10

Arrhenius/ ionic theory

Answer 10

Acid: yield H+ in water solution
Base: yield OH- in water solution

Question 11

Lewis theory

Answer 11

Acid: electron pair acceptor
Base: electron pair donor

Question 12

Bronsted- lowry theory/ conjugate acid- base pair theory

Answer 12

Acid: proton donor
Base: proton acceptor

Question 13

conjugate base

Answer 13

anion produced from the dissociation of acid: removal of hydrogen ( LOSS OF PROTON)

Question 14

conjugate acid

Answer 14

proton hydrogen donor: formed when it combines with hydrogen (GAINED PROTON)

Question 15

Henderson- Hasselbach Equation

Answer 15

the pH solution of a WA or WB and its salt given

pH= pKa + log (conjugate base/ acid)

Question 16

What is the first line of defense against changes in internal pH is provided by

Answer 16

Buffer systems

in cells and tissues we have– phosphate and bicarbonate buffer systems

[IMPORTANT NOTE]

The cytoplasm consist of proteins; amino acids with functional groups that are weak acids or weak bases