Question

$500ml$, $1M$ $NaCl\left(aq\right)$ solution is mixed with $1000ml$, $1M$ $Ag{NO}_3\left(aq\right)$ solution. Which of the following option is/are correct for resultant solution?

• A. $\left[{Na}^{+}\right]=\frac{1}{3}$
• B. $\left[{Ag}^{+}\right]=\frac{2}{3}$
• C. $\left[{NO}_3^{-}\right]=\frac{2}{3}$
• D. None of these

Answer 1

The correct option is C $\left[{NO}_3^{-}\right]=\frac{2}{3}$

Moles of $N{a}^{+}=500\times {10}^{-3}\times 1=0.5$

Total volume= $(1000+500)\times {10}^{-3}=1.5L$

$\therefore \left[N{a}^{+}\right]=\frac{0.5}{1.5}=\frac{1}{3}M$

Here $\left[A{g}^{+}\right]\ne \frac{2}{3}$ as it will precipitate in the form of $AgCl$.

For ${N{O}_3}^{-}$ also, number of moles= $1000\times {10}^{-3}\times 1=1$

$\therefore \left[{N{O}_3}^{-}\right]=\frac{1}{1.5}=\frac{2}{3}$