MCQ
When $400\, \mathrm{~mL}$ of $0.2\, \mathrm{M} \,\mathrm{H}_{2} \mathrm{SO}_{4}$ solution is mixed with $600\, \mathrm{~mL}$ of $0.1\, \mathrm{M} \,\mathrm{NaOH}$ solution, the increase in temperature of the final solution is $....\,\times 10^{-2} \,\mathrm{~K}$. (Round off to the Nearest Integer).
$\left[\right.$ Use $: \mathrm{H}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightarrow \mathrm{H}_{2} \mathrm{O}: \Delta_{\mathrm{\gamma}} \mathrm{H}=-57.1\, \mathrm{k} \mathrm{J} \,\mathrm{mol}^{-1}$
Specific heat of $\mathrm{H}_{2} \mathrm{O}=4.18 \mathrm{Jk}^{-} \mathrm{g}^{-}$
density of $\mathrm{H}_{2} \mathrm{O}=1.0\, \mathrm{~g} \mathrm{~cm}^{-3}$
Assume no change in volume of solution on mixing.]
- A$4$
- ✓$2$
- C$86$
- D$90$
