The solubility of silver(I)phosphate at a given temperature is 1.02 g/L. Calculate the Ksp at this temperature. After you get your answer, take the negative log and enter that (so it's like you're taking the pKsp)

The solubility product of silver (I) phosphate is

Explanation:

We are given:

Solubility of silver (I) phosphate = 1.02 g/L

To convert it into molar solubility, we divide the given solubility by the molar mass of silver (I) phosphate:

Molar mass of silver (I) phosphate = 418.6 g/mol

Solubility product is defined as the product of concentration of ions present in a solution each raised to the power its stoichiometric ratio.

The chemical equation for the ionization of silver (I) phosphate follows:

                            3s                  s

The expression of for above equation follows:

We are given:  

Putting values in above expression, we get:

Hence, the solubility product of silver (I) phosphate is

can you list the answers so i can answer

the answer is na (sodium)