If you have 10.00 mL of 0.5875 M H3PO4, how many mL of 0.2625 M NaOH are needed to reach the point of complete neutralization?
To determine the volume of 0.2625 M NaOH needed to completely neutralize 10.00 mL of 0.5875 M H3PO4, you can use the concept of molar ratio.
First, you need to recognize the balanced chemical equation for the reaction between H3PO4 and NaOH:
H3PO4 + 3NaOH → Na3PO4 + 3H2O
From the equation, you can see that the molar ratio between H3PO4 and NaOH is 1:3. This means that one mole of H3PO4 reacts with three moles of NaOH.
To solve the problem, follow these steps:
1. Calculate the number of moles of H3PO4:
Moles H3PO4 = volume (in L) × concentration (in M) = 10.00 mL × (1 L / 1000 mL) × 0.5875 M
2. Determine the number of moles of NaOH needed based on the molar ratio:
Moles NaOH = Moles H3PO4 × (3 moles NaOH / 1 mole H3PO4)
3. Calculate the volume of 0.2625 M NaOH needed:
Volume NaOH = Moles NaOH / concentration (in M) = Moles NaOH / 0.2625 M
By following these steps, you should be able to calculate the volume of 0.2625 M NaOH needed to completely neutralize 10.00 mL of 0.5875 M H3PO4.