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A 25-mL solution of H2SO4 is completely neutralized by 18 mL of 1.0M NaOH. What is the concentration of the H2SO4?

H2SO4(aq) +2NaOH(aq) _ Na2SO4(aq) + 2H2O(l)


A.0.72M

B.0.009M

C.0.50M

D.0.36M

Verified Answer :

taskmasters

There are several information's already given in the question. Based on the information's provided, the answer can be easily deduced.
V1 = 25 ml
     = 25/1000 liter
     = 0.025 liter
V2 = 18 ml
      = 18/1000 liter
      = 0.018 liter
M2 = 1.0 M
M1 = ?
Then
M1V1 = M2V2
M1 = M2V2/V1
      = (1 * 0.018)/0.025
      = 0.72 M
From the above deduction, it can be easily concluded that the correct option among all the options that are given in the question is the first option or option "A". I hope that this is the answer that has actually come to your help.

Answer : The correct option is, (D) 0.36 M

Explanation :

Using neutralization law,

\(n_1M_1V_1=n_2M_2V_2\)

where,

\(n_1\) = basicity of an acid = 2

\(n_2\) = acidity of a base = 1

\(M_1\) = concentration of \(H_2SO_4\) = ?

\(M_2\) = concentration of NaOH = 1.0 M

\(V_1\) = volume of \(H_2SO_4\) = 25 ml

\(V_2\) = volume of NaOH = 18 ml

Now put all the given values in the above law, we get the concentration of the \(H_2SO_4\).

\(2\times M_1\times 25ml=1\times 1.0M\times 18ml\)

\(M_1=0.36M\)

Therefore, the concentration of the \(H_2SO_4\) is, 0.36 M

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