(KOH) in the 250 mL volumetric flask is 1.5 M x 9.6/250 = approx 0.06 but that's an estimate.
mols KOH used = M x L = approx 0.06 x 0.0315 = approx 0.0018
Using the coefficients in the balanced equation, convert mols KOH to mols H3PO4. That's
0.0018 x (1 mol H3PO4/3 mol KOH = 0.0018 x 1/3 = ?
Then M H3PO4 = mols H3PO4/L H3PO4 = ?M
Suppose that 9.6 mL of 1.5 M KOH(aq)
is transferred to a 250 mL volumetric flask
and diluted to the mark. It was found that
31.5 mL of this diluted solution solution was
needed to reach the stoichiometric point in a
titration of 9.6 mL of a phosphoric acid solution
according to the reaction
3 KOH(aq) + H3PO4(aq) →
K3PO4(aq) + 3 H2O(ℓ)
Calculate the molarity of the solution.
Answer in units of M.
1 answer