Posted by Asuna on .
Hg2+ + 2Cl → HgCl
Mercuric nitrate was standardized by titrating a solution containing 147.6 mg of NaCl(FM 58.44), which required 28.06 ml of Hg(No3)2 solution.
Part a: Find the molarity of Hg(No3)2.
I already calculated the molarity to be 0.04500 M
Part b: When the same Hg(No3)2 solution was used to titrate 2.00 mL of urine, 22.83 mL was required. What is theconcentration of Cl (mg/mL) in urine.
I know the answer for part b is 36.42 mg/ml, but I'm not sure exactly how to get there...
Thanks.

Analytical Quantitative Chemistry 
Leydi,
1)Calculate the molarity for the mercuric nitrate solution. =0.04500M
2)Use M1V1=M2V2, to find urine concentration. (0.045mol/L)(0.02283L)=(M2)(0.002L), M2=0.513675mol/L
3)Find concentration of Cl using titration equation molecular ratios and molecular mass of Cl.
(0.513675molUrine/L)*(1molHgCl2/1molUrine)*(2molCl/1molHgCl2)*(35.453gCl/1molCl)*(1L/1000mL)*(1000mg/1g)=36.42mg/mL 
Chemistry 
Anonymous,
0.18

Chemistry 
cynthia,
Asuna, How did you calculate the Molarity of in part A?