Question

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-)`?

Answer 1

Approx. `7*g` of silver chromate will precipitate.

Explanation:

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

`2AgNO_3(aq) + K_2CrO_4(aq) rarr Ag_2CrO_4(s)darr + 2KNO_3(aq)`

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*Lxx0.400*mol*L^-1=0.0400*mol` 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`