0.600g of monoprotic acid is dissolved in 50.00ml water. Titration of this acid sample requires 24.9 ml of 0.100M sodium hydroxide. Calculate the molecular weight of the monoprotic acid.
2007-05-05 22:01:49 · 2 answers · asked by hazardous_century 1 in Science & Mathematics ➔ Chemistry
if you have 0.6 g in 50ml of water = 0.05l , you have 0.6/0.05 = 12g of that acid in 1L
To neutralize 1 Liter of that monoprotic acid solution you must use 24.9 *50 = 1245ml of 0.1M =124.5 millimole
So 12 g correspond to 124.5millimole= 0.1245mole
And the molecular weight is 12/0.1245= 96g
2007-05-05 23:14:17 · answer #1 · answered by maussy 7 · 0⤊ 0⤋
if 1 mole of monoprotic produces 1 mole of proton(H+) then the solution is:
titration; number of moles of monoprotic = number of moles of sodium hydroxid
=0.024 L *0.1M=0.0024 Mole
molar mass = (mass )/(number of moles)=0.6/0.0024=250 g/mole
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mhammad hamshari
2007-05-05 22:25:35 · answer #2 · answered by mohamed h 2 · 0⤊ 0⤋