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Accuracy precission practical sample

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5
th
Nov , 2018 Muhammad Ismail
Roll no 55
Object : Accuracy and precession
Theory
KCl and CaCl2 are both very soluble salts. Adding KCl to a solution that already has CaCl2 in it would simply
add another cation K+ to the mixture, and increase the concentration of Cl- ions that are already present.
Now, if you’re starting with a saturated solution of CaCl2 (you didn’t specify, so I have to guess maybe), then
KCl won’t dissolve in it. That’s because the solubility is a function of both the Ca(2+) and Cl- ion
concentrations. And if it’s already saturated, then neither Ca(2+) nor Cl- can be added. What would probably
happen is some KCl would dissolve and force some dissolved CaCl2 to crystallize out.
Procedure
Take 0.3154 g of oxalic acid and make up in 100.0 ml .
Make a saturated solution of KCl by adding Ca(OH)
2
in a beaker and then filter this solution .
Similarly make saturated solution of CaCl
2
by adding Ca(OH)
2
in a beaker and then filter this
solution .
Take 0.2663 g of Na
2
CO
3
make up in 100.0 ml having concentration 0.1005 M.
Take 2.5 ml of 0.01005 M Na
2
CO
3
solution and titrate it against HCl .
Take 10.0 ml of saturated KCl solution & 20.0 ml of saturated CaCl
2
solution in two different beakers
and titrate with hcl by noting their ph on ph meter after 1.0 ml of hcl consumed .
Observations
Standardization of HCl with Na
2
CO
3
Sr #
initial volume of
hcl (ml)
final volumeof hcl
(ml)
difference
concordant
1
0.0
7.0
7.0
7.0
2
7.0
14.0
7.0
3
14.0
21.1
7.1
For saturated filtrate of KCL solution
Volume of KCL solution = 10.0 ml
sr #
PH
sr #
Volume of HCl
PH
1
13
7
6
10.2
2
12.97
8
7
4.5
3
12.82
9
8
2.15
4
12.64
10
9
1.41
5
12.38
11
10
1.12
6
11.95
12
11
1

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5th Nov , 2018 Muhammad Ismail Roll no 55 Object : Accuracy and precession Theory KCl and CaCl2 are both very soluble salts. Adding KCl to a solution that already has CaCl2 in it would simply add another cation K+ to the mixture, and increase the concentration of Cl- ions that are already present. Now, if you’re starting with a saturated solution of CaCl2 (you didn’t specify, so I have to guess maybe), then KCl won’t dissolve in it. That’s because the solubility is a function of both the Ca(2+) and Cl- ion concentrations. And if it’s already saturated, then neither Ca(2+) nor Cl- ...
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