The concentration of pb²⁺ in a sample of wastewater is to be determined by using gravimetric analysis. to a 100.0-ml sample of the wastewater is added an excess of sodium carbonate, forming the insoluble lead (ii) carbonate (267 g/mol) according to the balanced equation given below. the solid lead (ii) carbonate is dried, and its mass is measured to be 0.1443 g. what was the concentration of pb²⁺ in the original wastewater sample? pb²⁺(aq) + na₂co₃(aq) -> pbco₃(s) + 2na⁺(aq)

0.005404 M

Explanation:

Since you added an excess of sodium carbonate you warrantied that all the in the sample reacted with it. So we can say that the insoluble lead (II) carbonate contains all the ions in the original sample.  

The moles of are:

One mol of is required to form one mol of . So, the stoichiometric relationship between them is 1:1.

Knowing this, 0.00054 is also the number of moles of in the original sample.  

So, the concentration of in the original sample is:

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