Which of the following represents the correct solubility product expression for calcium phosphate?

An aqueous solution contains $SCN^{-}$,$Br^{-}$,$I^{-}$,and $Cl^{-}$ ions. When $AgNO_3$ is added to the solution,which of these will precipitate first? Given: $K_{sp}(AgCl) = 1.2 \times 10^{-10}$,$K_{sp}(AgI) = 1.7 \times 10^{-16}$,$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,$K_{sp}(AgBr) = 3.5 \times 10^{-13}$.

Assign $A, B, C, D$ from the given type of reaction.
$CaCl_2 + Na_2C_2O_4 \longrightarrow CaC_2O_4\downarrow + 2NaCl$

Assign $A, B, C, D$ from the given type of reaction.
$ZnS(s) + 2HCl(aq) \longrightarrow ZnCl_2(aq) + H_2S(g)$

If the solubility products of $AgCl$ and $AgBr$ are $1.0 \times 10^{-10}$ and $3.5 \times 10^{-13}$ respectively,then the relation between the solubilities (denoted by the symbol $S$) of these salts can correctly be represented as:

Find the solubility in terms of $mol \ L^{-1}$ if the solubility product of silver bromide is $6.4 \times 10^{-13}$.