Calculate the volume of a 0.150 M NaOH solution that will be required to neutralize all of the H+ ions in 0.400 grams of phosphoric acid?
H3PO4 + 3NaOH ==> 3H2O + Na3PO4
mols H3PO4 = 0.4/molar mass H3PO4 = ?
Convert mols H3PO4 to mols NaOH using the coefficients in the balanced equation.
M NaOH = mols NaOH/L NaOH.
You know M and mols NaOH, solve for L NaOH
To calculate the volume of a NaOH solution required to neutralize phosphoric acid, you need to use stoichiometry and the balanced chemical equation for the reaction.
The balanced equation for the reaction between NaOH and phosphoric acid (H3PO4) is as follows:
3 NaOH + H3PO4 -> Na3PO4 + 3 H2O
From the balanced equation, we can see that for every 1 mole of H3PO4, we need 3 moles of NaOH to neutralize it completely.
Step 1: Calculate the moles of phosphoric acid.
To find the moles, divide the given mass of phosphoric acid (0.400 grams) by its molar mass (97.99 g/mol):
moles of H3PO4 = 0.400 g / 97.99 g/mol
Step 2: Calculate the moles of NaOH required.
Since the ratio between H3PO4 and NaOH is 1:3, multiply the moles of H3PO4 by 3 to find the moles of NaOH:
moles of NaOH = (moles of H3PO4) * 3
Step 3: Calculate the volume of the NaOH solution.
To find the volume, divide the moles of NaOH by its molarity (0.150 M):
volume of NaOH solution (in liters) = (moles of NaOH) / (molarity of NaOH)
Make sure to convert the volume to the desired unit (milliliters, liters, etc.) if necessary.
Now you have the step-by-step process to calculate the volume of a NaOH solution required to neutralize a given amount of phosphoric acid. Plug in the values for the moles of H3PO4 and the molarity of NaOH to get the final result.