Question

.) A sample containing both NaCl and NaBr, weighs 0.6400 g and gives a precipitate of AgCl and AgBr that weighs 0.5269 g. Another 0.6400 g sample was titrated with 0.1084 M AgNO3requiring 27.52 mL. Calculate the % w/w of NaCl and NaBr in the sample.

Answer 1

@ax

Answer 2

W(NaCl+NaBr+ inert substance ) = 1g
Let Wt. of NaCl is xg
& Wt. of NaBr is yg
(NaCl+NaBr)+AgNO
3
​
→(AgCl+AgBr)↓
xg yg excess 0.526g

58.5
x
​

103
y
​
Cl
2
​
↓△
AgCl(0.426g)

58.5
x
​
moles of NaCl will produce
58.5
x
​
moles of AgCl

∴ ...........................................................
58.5
x
​
×143.5g

103
y
​
mole s of NaBr will produce
103
y
​
mole of AgBr

∴ ...........................................................
103
y
​
×183g
A/q,

58.5
x
​
×143.5+
103
y
​
×183=0.526g

Answer 3

got it from toppr.com