1. The problem statement, all variables and given/known data My molarity is wrong which keeps me from ding the rest of this problem...any help would be greatly appreciated. A researcher has a 450.0 mL solution that is 0.421 M in Hg2(NO3)2 and 0.0191 M in Pb(NO3)2. She plans to add solid potassium iodide to separate the mixture by selective precipitation. Ksp PbI2 = 1.4e-8 Ksp Hg2I2 = 1.2e-28 What is the maximum concentration of iodide ions that may be in solution to achieve the best separation possible? M [I-]= ? How many grams of potassium iodide should she add to achieve this? g of KI What will the percentage of mercury(I) ions remaining in solution be? % Hg2+2 2. Relevant equations ksp= ... 3. The attempt at a solution hg2i2 = hg2 + 2i 1.2e-28 = [.421]^2 = 1.68e^-14, which is wrong and I have no idea what I am doing wrong
Ksp=??? Can you write down the expression for a general compound A_{m}B_{n}? This calculation is not correct. First write down the correct expression for Ksp, then plug in numbers.
thanks, but I already figured that out I failed to realize it said MAXIMUM so would be ksp for pbi = 8.6e-2 but now I am having problems with b and c