Chemistry, 08.04.2020 00:03 landanwithers
Calculate the maximum solubility of silver carbonate, Ag2CO3 in g/L when in the presence of 0.057 M AgNO3. The solubility product of Ag2CO3 is 8.1x10-12 and Ag2CO3 has a molar mass of 167.91 g/mol. Express your answer to the correct number of significant figures, in scientific notation and include units with your answer.
Answers: 1
. 
at equilibrium. The solubility equilibrium for 
.
is 
. For 
concentration be 
. The increase in 
. Note, that because of the 
of 
, the concentration of 
.The concentration of 
.![\begin{aligned}&\rm \left[Ag^{+}\right]^2 \cdot \left[{CO_3}^{2-}\right] = K_{\text{sp}} \\ & \implies (0.057 + x)^2\cdot x = 8.1 \times 10^{-12} \end{aligned}](/tpl/images/0588/0899/128cb.png)
.
is considerably small. Therefore, at equilibrium, the concentration of 
:
.
.
, meaning that there are approximately 
of 
.
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Calculate the maximum solubility of silver carbonate, Ag2CO3 in g/L when in the presence of 0.057 M...
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