Write balanced complete ionic and net ionic equations for

Solution: Step1: a) The reaction between Silver nitrate(AgNO ) and Hydroc3oric acid(HCl) takes place in the following manner: AgNO (a3 + HCl(aq) -----> AgCl(aq) + HNO (aq) 3 In the above reaction, we have seen that 1 mole of AgNO requires 1 mole of HCl to 3 precipitate out all the silver ions. Now, let us calculate the number of moles of 15.0 mL of 0.200 M AgNO solution. 3 Number of moles of AgNO solution 3Volume of solution in litres X Molarity = (15/1000 L) X 0.200 M = 0.015 L X 0.200 M = 0.003 mol Thus, 0.003 mol of AgNO solution3ill require 0.003 mol of HCl to precipitate out all the silver ions. Let us calculate the volume of HCl corresponding to 0.003 mol of 0.150 M HCl solution. Volume of HCl solution in litres = Number of moles of HCl / Molarity = 0.003 mol / 0.150 M = 0.02 L Thus, 0.02 L of a 0.150 M HCl(aq) solution is needed to precipitate the silver ions from 15.0 ml of a 0.200 M AgN0 solutio3 Step2: b) The reaction between Silver nitrate(AgNO ) and potassium chloride(KCl) takes place in 3 the following manner: AgNO (a3 + KCl(aq) -----> AgCl(aq) + KNO (aq) 3 In the above reaction, we have seen that 1 mole of AgNO requires 1 mol3of KCl to precipitate...