posted by KELLY on .
THE FOLLOWING SOLUTIONS AREMIXED TOGETHER: 121mL OF 1.54 M AgNO3 AND 45mL OF 1.07 M K2SO4
CALCULATE THE MOLAR CONCENTRATION OF Ag+ IONS IN THE FINAL SOLUTION
Write the equation and balance it.
mols AgNO3 = M x L
mols K2SO4 = M x L
Determine the limiting reagent. I think K2SO4 is limiting but check me out on that. If so then AgNO3 is a common ion to the ppt of Ag2SO4.
Ag^+ in the final solution, then, is Ag^+ from unused AgNO3 (subtract moles AgNO3 initially - 2(moles K2SO4) = unused AgNO3). That will be the moles of Ag^+ from the unused AgNO3 and you can change that to molarity by M = moles/L. Ag2SO4 is not extremely soluble but it is somewhat soluble. Look up the Ksp of Ag2SO4 and calculate Ag^+ from that, then add to the unused AgNO3. I think the amount from Ag2SO4 is so small that you can ignore that but you may want to check me out on that, too.