What will occur when a $100 \cdot m L$ $100mL$ volume of $A g N O_{3} (a q)$ $AgNO_3(aq)$ at $0.400 \cdot m o l \cdot L^{- 1}$ $0.400mol*L^-1$ concentration is added to an excess of potassium chromate, $K_{2}^{+} {[C r O_{4}]}_{4}^{2 -}$ $K_2^(+)[CrO_4]^(2-)$ ?

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What will occur when a $100 \cdot m L$ $100mL$ volume of $A g N O_{3} (a q)$ $AgNO_3(aq)$ at $0.400 \cdot m o l \cdot L^{- 1}$ $0.400mol*L^-1$ concentration is added to an excess of potassium chromate, $K_{2}^{+} {[C r O_{4}]}_{4}^{2 -}$ $K_2^(+)[CrO_4]^(2-)$ ?

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Answer 1 · 2017-06-05T15:52:18

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

Explanation:

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

$2 A g N O_{3} (a q) + K_{2} C r O_{4} (a q) \to A g_{2} C r O_{4} (s) ⏐ ↓ + 2 K N O_{3} (a q)$ $2AgNO_3(aq) + K_2CrO_4(aq) rarr Ag_2CrO_4(s)darr + 2KNO_3(aq)$

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

![chem103csu.wikispaces.com]( useruploads.socratic.org )

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

We have a molar quantity of $0.100 \cdot L \times 0.400 \cdot m o l \cdot L^{- 1} = 0.0400 \cdot m o l$ $0.100*Lxx0.400*mol*L^-1=0.0400*mol$ with respect to silver ion. And thus an half equiv of silver chromate will precipitate, i.e. consistent with the given stoichiometry:

$0.0200 \cdot m o l \times 331.73 \cdot g \cdot m o l^{- 1} = ? ? \cdot g$ $0.0200*molxx331.73 *g*mol^-1=??*g$

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What will occur when a $100 \cdot m L$ $100mL$ volume of $A g N O_{3} (a q)$ $AgNO_3(aq)$ at $0.400 \cdot m o l \cdot L^{- 1}$ $0.400mol*L^-1$ concentration is added to an excess of potassium chromate, $K_{2}^{+} {[C r O_{4}]}_{4}^{2 -}$ $K_2^(+)[CrO_4]^(2-)$ ?

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Explanation:

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What will occur when a 100⋅mL100*mL volume of AgNO3(aq)AgNO_3(aq) at 0.400⋅mol⋅L−10.400*mol*L^-1 concentration is added to an excess of potassium chromate, K+2[CrO4]2−K_2^(+)[CrO_4]^(2-)?

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Explanation:

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What will occur when a $100 \cdot m L$ $100mL$ volume of $A g N O_{3} (a q)$ $AgNO_3(aq)$ at $0.400 \cdot m o l \cdot L^{- 1}$ $0.400mol*L^-1$ concentration is added to an excess of potassium chromate, $K_{2}^{+} {[C r O_{4}]}_{4}^{2 -}$ $K_2^(+)[CrO_4]^(2-)$ ?