A solution of 0.314M KOH is used to neutralize 10.0mL H3PO4 solution.
H3PO4(aq) + 3KOH(aq) → K3PO4(aq) + 3H2O(lIf 29.3mL KOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution?)
mols KOH = M x L = ?
Using the coefficients in the balanced equation, convert mols KOH to mols H3PO4.
Then M H3PO4 = mols H3PO4/L H3PO4.
To determine the molarity of the H3PO4 solution, we can use the stoichiometry of the reaction and the volume of KOH solution required to reach the endpoint.
First, let's calculate the amount (in moles) of KOH used to neutralize the H3PO4 solution. Since the molarity of the KOH solution is given as 0.314M and the volume used is 29.3mL, we can multiply these values to get the moles of KOH:
moles of KOH = (0.314M) * (29.3mL / 1000mL/L)
moles of KOH = 0.00919 moles
Next, according to the balanced equation, the ratio of moles of H3PO4 to moles of KOH is 1:3. Therefore, the moles of H3PO4 in the neutralized solution is three times the moles of KOH:
moles of H3PO4 = 3 * 0.00919 moles
moles of H3PO4 = 0.0276 moles
Now, we can calculate the molarity of the H3PO4 solution using the volume of the H3PO4 solution, which is 10.0mL:
Molarity of H3PO4 = moles of H3PO4 / Volume of H3PO4 (in L)
Molarity of H3PO4 = 0.0276 moles / (10.0mL / 1000mL/L)
Molarity of H3PO4 = 2.76M
Therefore, the molarity of the H3PO4 solution is 2.76M.