Type 7 Predicting Solubility ksp3 note3 (1)

PART 1- Determination of solubility product (Kep) of different salts Table 1- Solubility of Ag2SO4 (add more rows if necessary) Mass of Ag,SO4 added (g) Concentration of Ag* (M) Concentration of SO,? (M) 0.100 0.00641293 0.00320646 0.100 0.0128259 0.00641293 0.100 0.0192388 0.00961939 0.100 0.0256517 0.0128259 0.100 0.0304380 0.0152190 0.100 0.0304380 0.0152190 Write the balanced chemical equation to represent the solubility of Ag2SO4: Calculate the solubility product constant (Kp) for Ag:SO4. Use the constant values obtained for the concentrations of the cation and anion. Show your work below:

The solubility of CUCO3 in NH3 solution will...? O increase. O decrease. O not change. can't tell because more information is needed.

In a conducted experiment solubility increased with temperature. Under which conditions is a reverse solubility relation (decrease in solubility with temperature) observed, and which important industrial process is based on this phenomenon?conditions:process:

Consider dissolving the barium nitrate in nitric acid HNO3 , a strong acid (it reacts completely with water to form hydronium and nitrate ions), instead of water. Does the nitric acid influence the barium nitrate’s solubility equilibrium? If so, how, and will this cause more or less barium nitrate to dissolve in the solution?

Please solve it correctly... posting third time and getting wrong answers

(b) What do you understand by solubility limit?