A 50.0-mL portion of a solution containing 0.200 of BaCl2 · 2H,0 is mixed with 50.0 mL of a solution containing 0.300 g of NalO3. Assumc that the solubility of Ba(IO3), in water is negligibly small and calculate (a) the mass of the precipitated Ba(IO3)2. (b) the mass of the unreacted compound that remains in solution.

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Q: How do I solve this 3 part question?

A: Mass of KHP = 1.372 g Volume of NaOH = 21.84 ml Density = 1.01 gml

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Q: Question attached

A: The balanced equation for the reaction between KHP and NaOH is: C8H5KO4 + NaOH → C8H4KO4-Na+ + H2O

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