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a 20.00 ml volume of h2so4 solution is titrated with 0.125 m naoh. the initial volume of naoh in the buret is 0.75 ml and the final volume is 42.35 ml. determine the concentration of the h2so4 solution. a. 0.115 m h2so4 b. 0.150 m h2so4 c. 0.300 m h2so4 d. 0.130 m h2so4 e. 0.260 m h2so4

Answer :

The molarity of H2SO4 when a 20.00 ml volume of h2so4 solution is titrated with 0.125 m NaOH. the initial volume of NaOH in the buret is 0.75 ml and the final volume is 42.35 ml is 0.260 M.

The balanced equation is  2NaOH+H2SO4→Na2SO4+2H2O.

The formula to calculate molarity is

c=n/v

n= c×v

Where, n = moles v= volume and c= molarity

So, the moles in NaOH

nNaOH = 0.125 × 0.75/ 1000

             = 9.3 × 10^-3

From the equation we can see that number of moles of H2SO4 must be half that amount so:

nH2SO4 = 9.3 × 10^-3 /2

               =4.65 × 10^-3

c = n/v

[H2SO4] = 4.65 × 10^-3 /20× 10^-3

              = 0.235 mol/L which equivalent to 0.26 M  H2SO4

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