number of moles of NaOH required to titrate 38.05mL of a 1.500 M H3PO4 solution
To find the number of moles of NaOH required to titrate a given volume of a H3PO4 solution, we can use the equation:
Molarity (M) = Moles (n) / Volume (V)
First, we need to identify the balanced chemical equation for the reaction between NaOH and H3PO4. It is:
3 NaOH + H3PO4 -> Na3PO4 + 3 H2O
From the equation, we can see that one mole of H3PO4 reacts with three moles of NaOH.
Since the molarity of the H3PO4 solution is given as 1.500 M, we can use this information, along with the volume of the H3PO4 solution (38.05 mL), to calculate the number of moles of H3PO4:
Molarity (H3PO4) = Moles (H3PO4) / Volume (H3PO4)
1.500 M = Moles (H3PO4) / 38.05 mL
Rearranging the equation, we can solve for the moles of H3PO4:
Moles (H3PO4) = Molarity (H3PO4) × Volume (H3PO4)
Moles (H3PO4) = 1.500 M × 0.03805 L (since 1 mL = 0.001 L)
Now that we know the number of moles of H3PO4, we can use the mole ratio from the balanced equation to determine the number of moles of NaOH required.
Moles (NaOH) = Moles (H3PO4) × (3 moles NaOH / 1 mole H3PO4)
Substituting the value we calculated for Moles (H3PO4) into the equation:
Moles (NaOH) = (1.500 M × 0.03805 L) × (3 moles NaOH / 1 mole H3PO4)
Calculating this expression will give you the number of moles of NaOH required to titrate 38.05 mL of the 1.500 M H3PO4 solution.