E agricultural analysis
2.	A   solution   of  hydrochloric  acid   was standardl^^0^   by
precipitating the chlorine from 40 cc as silver chloride.
weight of silver chloride found was 0.6327 gm.    Required
normality of the solution.
• i    i j-	0.6327        .,        _ul   . ,
1 cc acid solution =c= — ttt™ gm silver chloride*
1 cc normal acid solution =c= 0.1433 gm silver chloride-
Therefore normality- ^fUo.I433 =40^^33 -O.HO7N.
To make the solution decinormal 1000 cc would be diluted to
1107 ec.
3.	A similar solution was standardized by titration   of   pure
sodium carbonate in presence of methyl orange, the following
reaction being completed:
NajCOa + 2HC1 ->2NaCl + H_2CO_S.
It was found that 32.2 cc acid =c= 0.1638 gm of the primary
standard, sodium carbonate.   Required the normality.
.,      0.1638	,.	,       ,        ,   •
1 cc acid =£= -n-n' g^m sodium carbonate and
1 cc normal acid =c= 0.053 gin sodium carbonate.
Therefore normality = 32y^fo53^= °-^9598 ^N-
4. Another acid solution was standardized by titration against
a measured volume of standard potassium hydroxide solution
in presence of methyl orange according to the equation :
One cubic centimeter of the primary standard contained O.OO468
gm of potassium hydroxide. It was found from the ti tra/tion
that 50 cc of potassium hydroxide solution o: 43.5 cc of
hydrochloric acid solution.
The weight of potassium hydroxide in 50 cc of solution =
50 X 0.00468 gm. Since this weight was equivalent to -43.5
cc of acid, the potassium hydroxide equivalent to 1 cc sicici =
50 X 0.00468
-jg~ -------- gm.    Ihe normality of the hydrochloric acid, solu-
50 X 0.00468
43.5 x