Question

What volume of M/10 and M/30 solutions of H2

SO4

should be mixed to prepare 1 L of certain H2

SO4

solution whose 50 ml is completely neutralized by 10 ml of 0.5 M NaOH solution.​

Answer 1

Answer:

We know that H2SO4 is a dibasic acid and can release two H+ ions on hydrolysis. NaOH on the other hand is a strong base. So the reaction between a strong acid and a strong base will produce the respective salt and water. So the reaction is:

H2SO4 + 2NaOH -> Na2SO4 + 2 H2O

So, 2 mols of NaOH reacts with 1.mol of H2SO4 to give there respective salt. Therefore 25 mL of 0.1 M H2SO4 reacts with 50mL of NaOH to neutralise each other. Thus the total volume of the solution after neutralisation will be,

25+ 50= 75mL.

Now to obtain 0.05M of H2SO4 we must use some extra volume of it.

Let V1 = volume of extra H2SO4 needed = x mL

S1 = strength of the H2SO4 supplied = 0.1M

V2 = total volume of the resultant solution after adding H2SO4 = (75 + x) mL

S2 = strength of the resultant solution in H2SO4

= 0.05M

Therefore, from the principle of molarity,

V1*S1 = V2*S2

=> x * 0.1 = (75+x) * 0.05

Upon equating the value of x = 75mL.

There fore the total volume of 0.1M H2SO4 needed = 25 (for neutralisation) + 75 (for attaining concentration) = 100mL.

THANK YOU.

marke as brainlist...