At 18ºC, the solubility product of AgCl is 1.8 × 10–10. In the solution, the value of [Ag+] is 4 × 1 — Ionic Equilibrium Chemistry Question
Question
At 18ºC, the solubility product of AgCl is 1.8 × 10–10. In the solution, the value of [Ag+] is 4 × 10–3mol/litre. The value of [Cl–] to precipitate AgCl from this solution should be greater than
Answer: A
💡 Solution & Explanation
We know that, solubility product of AgCl can be calculated as- The solubility can be found as- Let concentration of A and B ions will be- x sp 10 3 10 3 7 8 AgCl Ag Cl K [Ag ][Cl ] 1.8 10 [4 10 ][ ] [ ] 1.8 10 / 4 10 0.45 10 4.5 10 x x x x x x x x M M If the ionic product exceeds this value, then precipitation takes place. Acid base Titration
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes