Question

Exactly 17.0 mL of a H2SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH. What was the concentration of the H2SO4 solution

Answer 1

The concentration of H2SO4 will be 0.31 M.

We have the balanced chemical equation:

                      H2SO4 (aq)+ 2NaOH(aq) → K2SO4 (aq) +2H2O (l)

We first find out the moles of the base used, which is sodium hydroxide in this case. We would use the formula:

                                                      c=n x v

n is the number of moles

v is the volume of solution

And so,

n =c x v

  =0.235 M 0.045

L=0.235 molL⋅0.045

L=0.010575mol

So, we got

0.010575

moles of base. From the equation, one mole of acid neutralizes two moles of base, so here, we would need:

0.010575 mol

=0.005287 mol

Now, we find the concentration of the solution of acid. And so,

       c =n v

          =0.0052875 mol

0.017L ≈0.31 mol/L

           =0.31 M

Learn more about Concentration here-

brainly.com/question/4184101

#SPJ4