[pin0y]

 

i'm a bit confused on this
Sulfuric Acid is being standardized against pure HgO(s) by titrating the OH^-(aq) produced from the following equation:
HgO(s)  +  4I^- (aq)   -->   HgI₄^2- (aq)  +  2OH^-(aq)
what would be the mole ratio of H2SO4 to HgO when trying to figure out the molarity of H2SO4 used?
is it 1 mole H2SO4 = 1 mole HgO at end point?
because?   HgO +  H2SO4 -->  H2O  +  HgSO4

thanks

[AWK]

OK

[Borek]

OK

Sorry, but what do you mean by OK? The titration equation given doesn't make sense and pin0y is missing the most important things in the experiment!

[Borek]

HgO +  H2SO4 -->  H2O  +  HgSO4

That's not the reaction that takes place during titration. It is acid/base titration, neutralization reaction done against pH indicator. HgO(s) defines amount of OH^- produced. HgI₄^2- complex is stable enough for the HgSO₄ to not precipitate.

[AWK]

Borek is absolutely right
The second reaction should be
2OH- + H2SO4 =
But surprisingly moles H2SO4 to HgO are OK