BUFFER SOLUTIONS
Buffer solutions
Classification
HOW TO PREPARE BUFFER
2. Partial neutralization
Buffer capacity
Buffer capacity depends on :
Buffer capacity
Buffer systems of a body
1. A buffer consists of 0,5 moles of equivalent NH3 and 0,5 moles of equivalent NH4Cl. Which buffer component must be added to
4. What volume of 0,01M NaOH should be added to 100 ml of 0,5M CH3COOH solution to produce a buffer with pH 4,75?
386.50K
Категория: ХимияХимия

Buffer solutions

1. BUFFER SOLUTIONS

2. Buffer solutions

solution which can resist the addition of a strong
acid or a strong base or water. Its’ pH changes
very slightly.
+
• + 1 drop of base
[H ] in 1000 000 times
+
• + 1 drop of acid
[H ] in 5000 times
-4
-7
(from 10 tо 5 х10 )
-7
In buffer solution from 1.00х10
-7
to 1.01х10

3. Classification

Acidic
Amfoteric
Weak acid and its’ salt
Aminoacids, proteins
Acetate
СН3СООН
СН3СОО–
(H3 N+)m – Prot – (COOˉ)n
НСО3–
Н2РО4–
НРO42–
Weak base and its’
salt
Ammonia
Hydrocarbonate Н2СО3
Phosphate
Basic
НА
Acid
Н+ + Аbase
Donor
Аcceptor
NH4+
NH3

4.

Mechanism of buffer action
Acetate buffer
СН3СОО- + Na+
СН3СООNa
СН3СООН
СН3СОО- + Н+
+ 1 mole NaOH
СН3СООН + ОН+1 mole HCL
СН3СОО- + Н+
Н+
ОН1 mole
СН3СОО- + Н2О
(weak electrolite )
СН3СООН
1 mole (weak electrolite)

5.

рН formulas are derived from Kdis.
CH 3COOH CH 3COO Н
CH 3COOK CH 3COO K
К д кисл
[CH3COO ][H ]
[CH3COOH]
[CH 3COO ] Cc , [CH 3COOH ] Cк
К д кисл ·С кисл
[H ]
Сс
lg [H ] lg К д кисл
Ск
lg
Сс
Сc
pH pК a lg
Ск
pH pK д кисл
N c ·Vc
lg
N к ·Vк
pH pK кисл
nc
lg

6. HOW TO PREPARE BUFFER

1. Mixing
the components:
-for acidic buffer
pH = pKa + lg Ns·Vs/Na·Va
-for basic buffer
pH = 14 – pKв – lg Ns·Vs/Nb·Vb

7. 2. Partial neutralization

- For acidic buffer
nacid = nbase = nsalt
СН3СООН + NaOH = CH3COONa + H2O
(exsess)
pH = pKa + lg Nb·Vb / (Na·Va –Nb·Vb)
- For basic buffer
NH4OH + HCL = NH4Cl + H2O
(exsess)
pH = 14 – pKв – lg Na·Va / (Nb·Vb - Na· Va)

8. Buffer capacity

.
Н|
Ba = nacid / |∆р
Vbuf.sol
Вb = nbase/ |∆р Н|. Vbuf.sol
n
– mole equivalents
of a strong acid or a strong base
Vbuf.sol - volume of a buffer solution
∆рН – pH change as a result of acid or base addition

9. Buffer capacity depends on :

1.Components amount
2.nsalt/nacid or
nsalt/nbase
Вmax
- for acidic buffer
at
nsalt = nacid
рН = рКа
- for basic buffer
at
nsalt = nbase
рН = 14-рКb
pH = pKa + lg nsalt/nacid
pH = 14 - pKb - lg nsalt/nbase

10.

Mechanism of buffer action
Acetate buffer
СН3СООNa
СН3СООН
СН3СОО- + Na+
СН3СОО- + Н+
Н+
ОН-

11. Buffer capacity

nsalt > nacid
nsalt < nacid
nsalt = nacid
Вa > Вb
Вa < Вb
Вa = Вb =Вmax
pH = pKa + lg nsalt/nacid

12.

• Choose the buffer with maximum
capacity and рН = 7.36 :
1) acetic
рК = 4.75;
2) phosphate рК = 7.21;
3) hydrocarbonate рК = 6.37.

13. Buffer systems of a body

1.Mineral
Hydrocarbonate Н2СО3
Phosphate
НСО3–
Н2РО4–
НРO42–
2. Protein and aminoacidic.

14.

Hydrocarbonate buffer
(K) NaHCO3/H2CO3
H2 O
atmosphere
СO2 (gas)
СO2 (solution)
lungs
H2СO3
H+ + HСO3-
Blood plasma
рН = pKa (H СO ) + lg C(NaHCO )/C(H2CO3) =
2
3
3
= 6,1 + lgC(HCO3-) – lg p(CO2)
p - CO2 pressure in lungs
Buffer capacity Вa = 40 ммole/L
Вb = 1-2 ммоle/L

15.

рН of blood plasma
7.4 = 6.1 + lg

[НСО3 ]/ [СО2]
[НСО3–]:[СО2] = 20:1
Вa > В b
Н2СО3 – 13 моle/ day
Other acids – from 0.03 to 0.08 моle/ day

16. 1. A buffer consists of 0,5 moles of equivalent NH3 and 0,5 moles of equivalent NH4Cl. Which buffer component must be added to

change pH
to 9? Kb(NH3)=1,8*10-5
2. What is the pH of buffer made of
60 ml of 0,10M NH3 with 40 ml of 0,10M NH4Cl.
Kb=1,8*10-5.
3. What volume of 0,6M CH3COONa must be
added to 600 ml of 0,2M CH3COOH to produce
a buffer with pH=4,75?
Ka(CH3COOH)=1,75*10-5.

17. 4. What volume of 0,01M NaOH should be added to 100 ml of 0,5M CH3COOH solution to produce a buffer with pH 4,75?

pKa(CH3COOH)=4,75
5. A buffer was prepared of 500 ml NaН2РО4 and
500 ml Na2НРO4 . After addition of 1 ml 0.1N HCl
the change of buffer pH = 0.03. Calculate buffer
capacity Ba.
6. Choose a buffer with Вa > Вb:
a). 100 ml 0.2M NaHCO3 + 100ml 0.4M H2CO3
b). 100 ml 0.4M NaHCO3 + 100ml 0.2M H2CO3
c). 100 ml 0.2M NaHCO3 + 100ml 0.2M H2CO3
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