Lead can generally be precipitated as a hydroxide at a pH of 8.0-8.5 and when the pH is raised to above 8.5, lead hydroxides become soluble. The pH levels of Lead Nitrate range from 8.5-9.0%. The pH level is a measure of how acidic or basic a substance is. Lead Nitrate being close to neutral but more basic than acidic. The lead nitrate [Pb(NO3)2] reacts with potassium iodide (Kl) causing exchange of ions between the reactants leading to the formation of potassium nitrate (KNO3) and a yellow precipitate of lead iodide (PbI2). The reaction involved is given as: Pb(NO3)2(aq)+2KI (aq)→PbI2(s)(↓)+2KNO3(aq). Lead (II) chloride can be made as a white precipitate by adding a solution containing chloride ions to lead(II) nitrate solution. You could use things like sodium chloride solution to provide the chloride ions, but it is usually easier just to add some dilute hydrochloric acid. PH is directly related to precipitation. The solubility will decrease by increasing the pH value, and the precipitate formation will increase, respectively. Similarly, the solubility will increase on the decreasing pH value, and precipitation will fall, respectively. We can use the reaction quotient to predict whether a precipitate will form when two solutions containing dissolved ionic compounds are mixed. If Q < Kₛₚ, the newly mixed solution is under saturated and no precipitate will form. If Q > Kₛₚ, the solution is oversaturated and a precipitate will form until Q = Kₛₚ.

PbCO3 is quite insoluble and likely to occur in the described case.

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Rk Naresh Thank you so much for the detailed answer. This means for my adsorption studies I shouldn't increase the pH of solution. I should keep it around 5 or less?

Depends on a reagent that you use for adjusting pH.

Phreeqc modeling shows that pH of 1 m Pb(NO3)2 solution is close to 5.4.

Adjusting pH to higher values requires addition of base and can cause precipitation of Pb(OH)2.