Question

the following titration data were collected: a 10 mL portion of a unknown monoprotic acid solution was titrated with 1.12340 M NaOH and required 23.95 mL of the base solution for neutralization.


calculate the molarity of the acid solution
calculate the molarity of the acid soluton were it the cas that the acid was diprotic
monoprotic:
HA + OH^- ==> H2O + A^-
moles NaOH = M x L = ?
moles HA = same since 1 mole HA = 1 mol OH^-.
M HA = moles/L = ?moles/0.01L = ?

diprotic:
H2A + 2OH^- ==> 2H2O + A^2-
moles NaOH = M x L = ?
moles H2A = 1/2 moles NaOH (since 1 mole H2A = 2 moles NaOH

M H2A = moles/L = (1/2 ?)/0.01 L = xx
M = 2.691

if diprotic, =134.6

Is this correct?

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