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When 100 mL 0.2 M KOH is mixed with 100 mL 0.2 M HCl in a rigid adiabatic container, temperature of solution increase by $t_{1}^{\circ} C$ while when 300 mL 0.1 M KOH is mixed with 300 mL 0.1 M HCl then increase in temperature is $t_{2}^{\circ} C$ then which one is correct? (Assume density as well as specific heat capacity of final solutions are same.)

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$t_{1} < t_{2}$

$t_{1} = t_{2}$

None of the

$t_{1} > t_{2}$

answer is B.

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Detailed Solution

$\begin{aligned} 200 \times d \times s \times t_{1} = \frac{100 \times 0.2}{1000} \times 13.7 \\ 600 \times d \times s \times t_{2} = \frac{300 \times 0.1}{1000} \times 13.7 \end{aligned}$

$\begin{array}{l} \Rightarrow \frac{t_{1}}{3 t_{2}} = \frac{2}{3} \\ \Rightarrow t_{1} = 2 t_{2} \end{array}$

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