For the reaction 3KOH+H3PO4⟶K3PO4+3H2O how many grams of potassium phosphate, K3PO4, are produced from 63.3 g of potassium hydroxide, KOH?

Question

Answer looks like mass of potassium phosphate: g

Answer 1

We must first make sure that the chemical equation is balanced.

3KOH_(aq) + H₃PO_4(aq) ==> K₃PO_4(aq) + 3H₂O_(l)

It is.

Next, let's interpret that equation. It tells us that one mole of K₃PO₄ will be produced from three moles of KOH. Therefore, we need to first figure out how many moles of KOH we actually have in our current chemical reaction.

moles KOH = 63.3 g KOH x 1 mol KOH / 56.1 g KOH = 1.128 moles KOH present

Third, we figure out how many moles of K₃PO₄ we will produce in this reaction.

1.128 mol KOH x 1 mol K₃PO₄ / 3 moles KOH = 0.376 moles K₃PO₄ produced

Let's round that to three significant figures: 0.38 mol K₃PO₄

And we're done!