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Question
If ‘S’ is solubility in mol dm–3 and Ksp is the solubility product, then write the relation between them for CaF2 and BaSO4. Calculate the concentration of H3O+ ion in soft drink whose pH is 3.5.
Solution
\[\ce{CaF_{2(s)} <=> Ca^{2+}_{ (aq)} + 2F^-_{ (aq)}}\]
x = 1, y = 2
∴ Ksp = xx yy Sx+y = (1)1 (2)2 S1+2 = 4S3
\[\ce{BaSO_{4(s)} <=> Ba^{2+}_{ (aq)} + SO^2-_{ 4(aq)}}\]
x = 1, y = 1
∴ Ksp = xx yy Sx+y = (1)1 (1)2 S1+1 = S2
Given: pH of soft drink = 3.5
To find: Concentration of H3O+ ion
Formula: pH = − log10[H3O+]
Calculation: From the formula,
pH = −log10[H3O+]
∴ log10[H3O+] = - 3.5
= - 3 - 0.5 + 1 - 1
= (- 3 - 1) + 1 - 0.5
= - 4 + 0.5
= - 3.5
∴ [H3O+] = Antilog10 -3.5
= 3.162 × 10-4 M
The concentration of H3O+ ion in soft drink is 3.162 × 10−4 M.
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