Answer these prelab questions show work! A 1.146-g mixture of the solid salts Na

Question

Answer these prelab questions show work!

A 1.146-g mixture of the solid salts Na2SO4 and Pb(NO3)2 forms an aqueous solution with the precipitation of PbSO4. The precipitate was filtered and dried, and its mass was determined to be 0.672 g. The limiting reactant was determined to be Na2SO4. Write the molecular form of the equation for the reaction. Write the net ionic equation for the reaction. HOW many moles and grams of Na2SO4 are in the reaction mixture What is the percent by mass of each salt in the mixture?

Explanation / Answer

a> Na2SO4 + Pb(NO3)2 ----> PbSO4 + 2NaNO3

c> moles of Na2SO4 = moles of PbSO4

= 0.672/303

= 0.002218

d> mass of Na2SO4 = 0.002218 * 142 = 0.315 g

mass of Pb(NO3)2 = 1.146 - 0.315 = 0.831 g

% of Na2SO4 = 27.5 %

% of Pb(NO3)2 = 72.5 %

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