A 2.0 mole sample of H3PO4(aq) reacts with KOH(aq) and produces K3PO4(aq) and H2O(l).how many moles of KOH react with H3PO4 and how many moles of K3PO4 and H2O are produced?

Answer 1

To solve this question, we need to find a balanced equation for the reaction, and then use the molar ratios from the equation to find the answers

1) Balancing Equation: The equation for the reaction is H₃PO_{4 (aq)}+ KOH_(aq) ————> K₃PO_{4 (aq)} + H₂O_(aq)

Balancing the equation, we get the following balanced equation:

H₃PO_{4 (aq)}+ 3KOH_(aq) ————> K₃PO_{4 (aq)} + 3H₂O_(aq)

2) Finding the answers: To find the number of moles of each compound, we use the molar ratio of H₃PO₄ to all the other compounds, and then do the calculation to find the answers.

i) KOH: 2 mol H₃PO₄ * (3 mol KOH/1 mol H₃PO₄) = 6 mol KOH

ii) K₃PO₄ : 2 mol H₃PO₄ * (1 mol K₃PO₄/1 mol H₃PO₄) = 2 mol K₃PO₄

iii) H₂O : 2 mol H₃PO₄ * (3 mol H₂O/1 mol H₃PO₄) = 6 mol H₂O