The correct definition of the Ksp is ..... a. The product of the number of particles of the solution raised to the coefficient Cb. The product of the mole of ions in solution raised to the coefficient c. Product of the concentration of the ions in the unsaturated solution d. The product of the number of ions in the solution raised to the coefficient Ce. The product of the concentration of the saturated solution ions is raised to the co

The addition of 0.3800 L of 1.150 M KCl to a solution containing Ag+ and Pb2+ ions is just enough to precipitate all of the ions as AgCl and PbCl,. The total mass of the resulting precipitate is 61.40 g. Find the masses of PbCl, and AgCl in the precipitate. mass of PbCl, : g mass of AgCl:

Solid aluminum nitrate is slowly added to 150 mL of a 0.0699 M potassium hydroxide solution. The concentration of aluminum ion required to just initiate precipitation is  M.the expert working on my last question, doesnt have to anymore, its been answered thanks.

4. A 25.00 mL sample of a weak acid HX is titrated with 0.1250 M NaOH. The equivalence point in the titration occurs when 19.91 mL of the NaOH solution has been added. Neutralization reaction: HX + NaOH → NaX + H₂O Please answer the following questions. A. B. Based on the volume of 0.1250 M NaOH required to reach the equivalence point, calculate the concentration of the weak acid HX in the original 25.00 mL sample. M D. Please provider your answer below. 0² 0, (0) Check answer Determine the concentration of HX in the solution after the 10.00 mL of 0.1250 M NaOH has been added to the original 25.00 mL of weak acid sample in the titration. Please provider your answer below. 号 (0) Check answer Check answer C. Determine the concentration of NaX in the solution after the 10.00 mL of 0.1250 M NaOH has been added to the original 25.00 mL of weak acid sample in the titration. Please provider your answer below. 0₂ ← A ← Check answer $ ← → ← $ Given that Ka = 4.72x10-8 for the weak acid HX,…