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-)#?

1 Answer
Jun 5, 2017

Answer:

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........

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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#