Solubility product $(K_{sp})$ of the salts $MX$,$MX_2$,and $M_3X$ at temperature $T$ are $4 \times 10^{-8}$,$3.2 \times 10^{-14}$,and $2.7 \times 10^{-15}$ respectively. The solubilities of these salts at temperature $T$ are in the order:
- A$MX > MX_2 > M_3X$
- B$M_3X > MX_2 > MX$
- C$MX_2 > M_3X > MX$
- D$MX > M_3X > MX_2$
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View SolutionThe solubility product $(K_{sp})$ of the following compounds are given at $25\,\text{°C}$:
Compound $K_{sp}$ $AgCl$ $1.1 \times 10^{-10}$ $AgI$ $1.0 \times 10^{-16}$ $PbCrO_4$ $4.0 \times 10^{-14}$ $Ag_2CO_3$ $8.0 \times 10^{-12}$
The most soluble and least soluble compounds are respectively:
| Compound | $K_{sp}$ |
| $AgCl$ | $1.1 \times 10^{-10}$ |
| $AgI$ | $1.0 \times 10^{-16}$ |
| $PbCrO_4$ | $4.0 \times 10^{-14}$ |
| $Ag_2CO_3$ | $8.0 \times 10^{-12}$ |
The most soluble and least soluble compounds are respectively:
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View SolutionThe relationship between solubility $(S)$ and solubility product $(K_{sp})$ for a salt of type $A_x B_y$ is given by:
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