4. When aqueous solutions of lead(II) ion are treated with potassium chromate solution, a bright yellow precipitate of lead(II) chromate, PbCrO4, forms. How many grams o lead chromate form when a 1.00-g sample of Pb(NO3)2 is added to 25.0mL of 1.00M K2CrO4 solution

Lead chromate form = 0.97 g

Explanation:

The Balanced chemical equation of the given reaction is as follows

              K₂CrO₄ + Pb(NO₃)₂ → PbCrO₄ + 2 KNO₃

Given that

        Mass of Pb(NO₃)₂ = 1 g

Mole of 25 ml of 1.00 (M)  K₂CrO₄

                   Mole =   25 x 1 milimol = 25 x 10⁻³

Using mole ratio method to find limiting reagent

Hence K₂CrO₄(potassium chromate) is a limiting reagent.

So lead chromate formed = mole X molar mass

                                           = 0.003 X 323.19 g

                                           = 0.97 g

∴ 0.97 g lead chromate form when a 1.00-g sample of Pb(NO₃)₂ is added to 25.0 ml of 1.00 M K₂CrO₄ solution.

it means there are 3 atoms of oxygen

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