Question

How many moles of sodium phosphate would be required to react with $1.0mol$ of silver nitrate?

Answer 1

We have the balanced equation as:

$N{a}_{3}P{O}_{4_{\left(aq\right)}}+3AgN{O}_{3_{\left(aq\right)}}\to 3NaN{O}_{3_{\left(aq\right)}}+A{g}_{3}P{O}_{4_{\left(s\right)}}$

The molar ratio between sodium phosphate $\left(N{a}_{3}P{O}_4\right)$ and $AgN{O}_3$ is $1:3$. That means, one mole of sodium phosphate would react fully with three moles of silver nitrate.

So, if $1$ mole of silver nitrate is available, then only $\frac{1}{3}\approx 0.3$ moles of sodium phosphate will react, due to the mole ratios.

Therefore, $0.3$ moles of sodium phosphate would be required.