Inorganic and Applied Chemistry

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Inorganic and Applied Chemistry

[OH-]* x M

[CH 3 COO -] = x M

Hereby the following equation is:

x M

x

x x

Kb^10 M 5. 3106

0. 050

5. 610

 (

Thus, the concentrations of OH- ions is 5.3 · 10-6 M, which is why the concentration of H 3 O+ ions are

found using knowledge of the autoprotolysis of water:

  M

M

HO OH K HO M

w

9

6

14 2

(^335). 310 1.^910

1. (^010)
    
   (
   pH is calculated:
   pH log 1. 910
   9  8. 72
   It is seen that the point of equivalence is somewhat in the basic areas. This is always the case for titrations
   of a weak acid with a strong base.
   Case 5: 60.0 mL 0.10 M NaOH solution has been added – solution of a strong base
   When further OH- ions are added after the point of equivalence these ions will dominate in respect to the
   weak base (CH 3 COO- ions). Thus, pH may be determined from the excess concentrations of OH- ions. The
   concentration of excess OH- ions may be determined as:
    M
   L L
   mol
   totalvolumen
   molOH ionerioverskud
   OH^3
   3


2. 110
   ( 0. 0500 0. 0600 )
   1.^010
   
   Thus, the concentrations of OH- ions is 9.1 · 10-3 M which is why the concentration of H 3 O+ ions again
   may be found as:
     M
   M
   HO OH K HO M
   w
   12
   3
   14 2
   (^339). 110 1.^110


3. (^010)
    ^
   (
   Which is why pH becomes:
   pH log 1. 110
   12  11. 96
   On the basis of such calculations as in the five cases it is possible to make a titration curve. This curve
   may be seen from figure 5-2.
   Acids and bases