A solution is formed by combining 0.025 mol CaCl2 and 0.015 mol Pb(NO3)2 producing one litre of solution. Will PbCl2 precipitate in this solution?
Asked by Topperlearning User | 4th Jun, 2014, 01:23: PM
0.015 mol of Pb(NO3)2 gives 0.015 mol of Pb2+ ions or ,0.015 M)
0.025 mol of CaCl2 yields 0.05 mol Cl- ions or. 0.05 M
Hence , [Pb2+][Cl]2 = (0.015)(0.050)2 = 3.75 x 10-5
Ksp of PbCl2 = 1.6 x 10-5
Since the ion product is larger than the Ksp, the solution precipitates.
Answered by | 4th Jun, 2014, 03:23: PM
- Sir, Can you please explain the method for solving buffer based and PH based questions in equillibrium
- What is the common ion effect?
- What is a buffer solution?
- How do buffer solutions work?
- The Ksp for AgCl is 1.8 x 10-10. If Ag+ and Cl- are both in solution and in equilibrium with AgCl. What is [Ag+] if [Cl-] = .020 M?
- The Ksp for AgCl is 1.8 x 10-10. If Ag+ and Cl- were both present at 0.0001 M, would a precipitate occur?
- Iron (III) nitrate has a solubility of 0.15 M. Find concentration of the ions in solution.
- The Ksp for Ag2CrO4 is 9x10-12 M3. What is the molar solubility of Ag2CrO4 in pure water?
- Calculate [Ag+], when 0.03 mole of KBr is added to one liter saturated solution of AgBr. Given Ksp of AgBr =5.0x10-13
Kindly Sign up for a personalised experience
- Ask Study Doubts
- Sample Papers
- Past Year Papers
- Textbook Solutions
Verify mobile number
Enter the OTP sent to your number