Question

The solubility of a A2B in pure water is ​

Answer 1

Answer -

• Let us consider solubility of any general salt AxBy. Let Case 1:Solubility of a salt of strong acid with strong base in pure water ... Solubility product of A2B is 4 × 10-9 (mol/lit)3

→ Hope it will help you ❣️❣️

→ Please mark as Breinliest ❤️❤️

Answer 2

To deduce the solubility of a $A_2B$ compound in pure water we need to deduce it as follows,

• We know that the maximum amount of a substance that can be dissolved in a solvent at a particular temperature is called solubility. To calculate the solubility in g/100g, we need to divide the mass of the substance by the mass of the solvent and multiply by 100 g.
• But in that case, we can say that, $A_2B\leftrightharpoons 2A^+ +B^-$. If we assume that "S" be the solubility of $A_2B$, then we can have the solubility product constant - $K_{sp}$. From this one can find the solubility of a $A_2B$. Here the  $K_{sp}$ be, $[2S]^2$×[S]=$4[S]^3$.

#SPJ3