Question

Under the same condition how much milliliter of $1{{ M KOH}}$ and \[0.5{{ M }}{{{H}}_2}S{O_4}\] solutions, respectively. When mixed for a total volume of$100{{ml}} $, produces the highest rise in temperature.
A. $67:33$
B. $33:67$
C. $40:60$
D. $50:50$

Answer 1

Hint: when we neutralize an acid and base reaction the heat is given out because they are exothermic in nature and more and more ions are used up in the progress of the reaction that’s why the temperature of the reaction decreases as the reaction moves in the forward direction. Whereas when a base is added the temperature increases, energy or heat is produced.

Complete step by step answer:
First we have to write the equation of neutralization.
$2KOH + {H_2} S {O_4} \to {K_2} S {O_4} + 2{H_2} O$
${n_1} = 2$ ${n_2} = 1$
‘n’= n factor
$\Rightarrow \dfrac{{{M_1}{V_1}}}{{{n_1}}}(KOH) = \dfrac{{{M_2}{V_2}}}{{{n_2}}}({H_2}S{O_4})$
Since we have not been given the volume in our question, so we will consider $'x'$$ml$$ml$ of potassium hydroxide and $(100 - x) $$ml$ of ${H_2} S {O_4} $for neutralisation.
Now replace the values in the above equation,
$\dfrac {{1 \times x}} {2} = \dfrac{{0.5 \times (100 - x)}} {1} $
We get, $x = 50ml$
$\Rightarrow $ Equal volume of $KOH$ and \[{H_2}S{O_4}\] will be neutralised together to get the highest rise in temperature.

So, the correct answer is Option D.

Note: We know that this reaction is a neutralisation reaction. Where an acid and base or alkali react according to their quantities with each other. These types of reaction are used in chemical titration methods for determining acid and bases. It is also used in wastewater management. Where this method is used to reduce that is caused by chemicals from the industries. It is also used for ph control, which includes calcium carbonate, calcium oxide, and magnesium hydroxide. This reaction is also used in antacids. And to neutralize gastric acids as well.