1. A 10.0-mL solution ofH2SO4(aq) solution is titrated with 0.254 M NaOH(aq). Th

Question

1.       A 10.0-mL solution ofH2SO4(aq) solution is titrated with 0.254 M NaOH(aq). Theequivalence point of the titration is 47.35mL.

a.       What is the molarconcentration of the H2SO4(aq) solution?

b.      What is the mass percent ofH2SO4(aq) in solution? Assuming the density is 1.0 g/mL.

Explanation / Answer

H2SO4 + 2NaOH ->Na2SO4 + 2H2O n(NaOH) = cv = 0.254 x 0.04735 = 0.01203mol n(H2SO4) = 1/2 x n(NaOH) = 0.006013mol c(H2SO4) = n/v = 0.006013/0.01 =0.60M n(H2SO4) = m/M m(H2SO4) = nM = 0.006013 x 98.076 =0.5897g Density of solution = mass/volume 1.0 = mass/1 Mass of solution = 1g Mass percent of H2SO4 = 0.5897/1 x 100 =58.97% Hope this helps! Please rate high

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