Exactly 15.78 mL of 0.1394 M KOH is used to titrate a 12.50 mL sample of H 2 SO

Question

Exactly 15.78 mL of 0.1394 M KOH is used to titrate a 12.50 mL sample of H2SO4. What is the concentration of the sulfuric acid? The molecular chemical equation for this neutralization is:   

H2SO4(aq) + 2 KOH(aq) -> K2SO4(aq) + 2 H2O(l)

The concentration of the sulfuric acid is, H2SO4(aq), is_____x10^_____M.  Please explain

Exactly 15.78 mL of 0.1394 M KOH is used to titrate a 12.50 mL sample of H2SO4. What is the concentration of the sulfuric acid? The molecular chemical equation for this neutralization is: H2SO4(aq) + 2 KOH(aq) -> K2SO4(aq) + 2 H2O(l) The concentration of the sulfuric acid is, H2SO4(aq), is x10^ M. Please explain

Explanation / Answer

Normality of 0.1394 M KOH is (0.1394*1) N= 0.1394N

let the Molarity of H2SO4 solution be M

then, the Normlity of H2SO4 solution will be 2*M

by stichiometry N1V1=N2V2

=>15.78*0.1394=12.50*2*M

=>M=0.0879 M

The concentration of the sulfuric acid is, H2SO4(aq), is__8.79___x10^_-2____M.

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