# What will occur when a 100*mL volume of AgNO_3(aq) at 0.400*mol*L^-1 concentration is added to an excess of potassium chromate, K_2^(+)[CrO_4]^(2-)?

Jun 5, 2017

Approx. $7 \cdot g$ of silver chromate will precipitate.

#### Explanation:

We need a stoichiometric equation........

$2 A g N {O}_{3} \left(a q\right) + {K}_{2} C r {O}_{4} \left(a q\right) \rightarrow A {g}_{2} C r {O}_{4} \left(s\right) \downarrow + 2 K N {O}_{3} \left(a q\right)$

We assume (reasonably) that you have added the silver nitrate to a stoichiometric excess of potassium chromate........

And very insoluble, brick-red silver chromate precipitates with alacrity.

We have a molar quantity of $0.100 \cdot L \times 0.400 \cdot m o l \cdot {L}^{-} 1 = 0.0400 \cdot m o l$ with respect to silver ion. And thus an half equiv of silver chromate will precipitate, i.e. consistent with the given stoichiometry:

0.0200*molxx331.73 *g*mol^-1=??*g