Question

when 100ml of 0.2M of HCl is mixed with 100ml of 0.2M NaOH solution , the amount of heat produced?
Give ans with Solution​

Answer 1

Explanation:

As NaOH and HCl are monoacidic base and monobasic acid respectively, Molarity and Normality values will be same.

So number of g equivalent of HCl = 0.2 N × 0.1 Litre = 0.02

Number of g equivalent of NaOH = 0.2 N × 0.1 litre = 0.02

so 0.02 g equivalent of NaOH will be neutralized by 0.02 g equivalent of HCl.

So heat released = 0.02 g equivalent × 57.3 KJ/ g equivalent =1.146 KJ

Answer 2

Explanation:

Let's see what happens. The heat of neutralization between a strong acid and a strong base is -57.62kJ/mol (In case you didn't know, that's a calculated value.) Any strong acid reacting with a strong base will yield -57.62kJ/mol).

Also, NaOH and HCl are monoacidic base and monobasic acid respectively, Molarity and Normality values will be the same.

Let us prove it,

1000ml = 1 dm^3

Hence 100ml = 0.1 dm^3

Recall M => mol/dm^3

So the number of moles in 0.1 dm^3>of 0.2M of HCL is 0.1 × 0.2 = 0.02 moles

This also applies to NaOH => 0.1 × 0.2 = 0.02 moles.

So virtually, in this reaction, 0.02 moles of HCl and 0.02 moles of NaOH are mixed, basically giving you 0.02 moles of NaCl. So, when 1 mole of NaCl is formed, 57.62 kJ of energy is released. So you can calculate the amount of heat released during the formation of 0.02 moles of NaCl:

0.02 x (-57.62)=

-1.1524kJ