Q.

When 100ml of 0.06M Fe(NO)3, 50ml of 0.2M FeCl3 and 100ml of 0.26M Mg(NO3)2, are mixed; the concentration of NO3- ions in the final solution is

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a

0.12M

b

0.028M

c

0.32M

d

0.28M

answer is D.

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Detailed Solution

Mixture of solutions contain

A) 100ml of 0.06M Fe(NO3)3

B) 50ml of 0.2M FeCl3

C) 100ml of 0.26M Mg(NO3)2

 

NO3- ions are present only in solution (A) and solution (C)

Solution(A) [Fe(NO3)3]

 

0.06\;=\;\large n_{Fe(NO_3)_3} \times \frac{1000}{100}
\large n_{Fe(NO_3)_3} = 6 \times 10^{-3}

nNO3-(from ferricnitrate) =6×10-3×3

Solution(C) [Mg(NO3)2]

 

\large 0.26\;=\;n_{Mg(NO_3)_2} \times \frac{1000}{100}
\large n_{NO_3^-}

nNO3- [from Mg(NO3)2] =0.026×2= 0.052

Total moles of NO3-ions in the mixture =(18×10-3) + 0.052= 0.07

Total volume of solution = (100 + 50 + 100)ml = 250ml

MNO3-in the mixture =0.07×1000250=0.28 M

 

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When 100ml of 0.06M Fe(NO)3, 50ml of 0.2M FeCl3 and 100ml of 0.26M Mg(NO3)2, are mixed; the concentration of NO3- ions in the final solution is