Calculate the concentration of the silver ion in a solution that initially is 0.10 M with respect to Ag(NH3)2+.

What is the concentration of Ag+ (aq) ion in 0.010 M AgNO3 that is also1.00 M NH3? Kf for Ag(NH3)2+ is 1.7 x 107.

Calculate the silver ion concentration, [Ag+], of a solution prepared by dissolving 1.00 g of AgNO3 and 10.0 g of KCN in sufficient water to make 1.00 L of solution. (Hint: Because Kf is very large, assume the reaction goes to completion then calculate the [Ag+] produced by dissociation of the complex.)

You have a solution of silver nitrate with an unknown concentration. To determine the concentration, you devise a method of adding an excess of calcium metal to 100.0 cm3 of solution and collecting the silver by filtration.2AgNO3(aq)+Ca(s)→Ca(NO3)2(aq)+2Ag(s)2AgNO3(aq)+Ca(s)→Ca(NO3)2(aq)+2Ag(s)If 0.201 g of silver was collected, calculate the concentration of the silver nitrate solution in mol dm−3.Answer with the numerical value of the concentration to three significant figures, but do not include the units.

What mass of silver iodide can be made by the reaction of 10.0 g of silver nitrate (AgNO3) with 10.0 g of sodium iodide (NaI)?Ag+(aq)  +  I-(aq)  ®  AgI(s)

Determine the mass (in grams) of silver chloride, AgCl, that would be precipitated if an excess of AgNO3 solution is added to 55.0 cm3 of 0.200 mol dm−3 KCl solution. The balanced equation for the reaction is:KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)Mr AgCl = 143.32