[larson]

Hey everyone! I have attempted this problem, but would like to know if I did it correctly.  Thanks!

An aqueous solution of silver nitrate (100.0 mL, 0.112 M silver nitrate) is mixed with an aqueous solution of potassium chloride (75.3 mL, 0.167 M potassium chloride), forming an insoluble precipitate,  After vacuum filtration, washing, and drying, 1.43 grams of the solid precipitate is recovered.

1. Write the chemical equation describing the reaction that occurs.  [Show all species as compounds (e.g. NaCl_(aq)) rather than as ions (e.g. Na⁺_(aq) + Cl^-_(aq)).

AgNO_3(aq) + KCl_(aq) = KNO_3(aq) + AgCl_(s)


2. Write the net ionic equation describing the reaction that occurs.

Ag⁺_(aq) + Cl^-_(aq) = AgCl_(s)


3. What is the theoretical yield (in grams) of the solid precipitate?

From the molarity equation... Moles = Molarity * Liters of Solution
Moles of silver nitrate = 0.112 M * 0.1 L
                             = 0.0112 moles AgNO₃

Moles of potassium chloride = 0.167 M * 0.0753 L
                                     = 0.0126 moles KCl

Grams of AgCl = (0.0126 mol KCl)(1 mol AgCl / 1 mol KCl)(143 g AgCl / 1 mol AgCl)
                   = 1.80 g AgCl


4. What is the percent yield for this reaction?

Percent yield = (actual yield / theoretical yield) * 100
                  = (1.43 g AgCl / 1.80 g AgCl) * 100
                  = 74.4%

Is all of this correct, or no? If not, could somebody help me out?

Thanks,
Larson

[Borek]

Which substance (KCl or AgNO₃) is a limiting reagent?

[larson]

Which substance (KCl or AgNO₃) is a limiting reagent?

I believe AgNO₃ is the limiting reagent.

[Borek]

I believe AgNO₃ is the limiting reagent.

Grams of AgCl = (0.0126 mol KCl)(1 mol AgCl / 1 mol KCl)(143 g AgCl / 1 mol AgCl)

So why you have calculated amount of product from moles of KCl?