Asked by Ali
A solution is prepared by placing 27.8 g of KCl in a 0.700 L volumetric flask and adding water to dissolve the solid, then filling the flask to the mark. What is the molarity of an AgNO3 solution if 22.1 mL of the KCl solution react exactly with 43.0 mL of the AgNO3 solution?
Answers
Answered by
DrBob222
27.8g KCl/molar mass KCl = approx 0.37
0.37/0.7 = approx 0.53M
AgNO3 + KCl ==> AgCl + KNO3
mols KCl used = M x L = 0.0221 x 0.53 = ?
mols AgNO3 = the same (since the ratio in the balanced equation is 1:1).
Then M AgNO3 = mols AgNO3/L AgNO3.
0.37/0.7 = approx 0.53M
AgNO3 + KCl ==> AgCl + KNO3
mols KCl used = M x L = 0.0221 x 0.53 = ?
mols AgNO3 = the same (since the ratio in the balanced equation is 1:1).
Then M AgNO3 = mols AgNO3/L AgNO3.
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