How many moles of potassium hydroxide are required to neutralize 1.25 mol of phosphoric acid?

H3PO4 + 3KOH -> K3PO4 +3H2O

I got 0.42 mol KOH , is this correct?

thanks!

Look at the equation.

1 mol H3PO4 = 3 mols KOH
So, 1.25 mol H3PO4 must need ?? mols KOH and it isn't 0.42.

Okay, so I got 3.75 mol KOH now?

Why do you think that is not right?

If 1 H3PO4 = 3 KOH, then
2 H3PO4 = 6 KOH and 1.25 must be somewhere between.

To determine the number of moles of potassium hydroxide (KOH) required to neutralize 1.25 mol of phosphoric acid (H3PO4), you need to apply the stoichiometry of the balanced chemical equation.

From the balanced equation:
1 mole of H3PO4 reacts with 3 moles of KOH to form 1 mole of K3PO4 and 3 moles of H2O.

Since the stoichiometric ratio between H3PO4 and KOH is 1:3, you can use this ratio to calculate the amount of KOH required.

Given:
Number of moles of H3PO4 = 1.25 mol

To find the number of moles of KOH required, you can use this ratio:

1.25 mol H3PO4 × (3 mol KOH/1 mol H3PO4) = 3.75 mol KOH

So, you would need 3.75 moles of KOH to neutralize 1.25 moles of phosphoric acid.

Therefore, your answer of 0.42 mol KOH is not correct. The correct answer is 3.75 mol KOH.