Silver nitrate, AgNO₃, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl.What volume of 1.5 M AgNO₃will be required to react with 30.0 mL of a 0.45 M HCl solution AgNO₃(aq) + HCl(aq) $\rightarrow$ AgCl(s) + HNO₃(aq) A)45 mL B)9.0 mL C)9.0 L D)1.0 L E)1.1 *10² mL

Question

Quizplus · Accepted Answer

First, we need to balance the equation to determine the mole ratios of the reactants and products:

AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)

The mole ratio between AgNO3 and HCl is 1:1. Therefore, we can use the following equation to calculate the moles of AgNO3 needed to react with the amount of HCl given:

moles of AgNO3 = (volume of HCl × molarity of HCl) / 1

moles of AgNO3 = (30.0 mL × 0.45 mol/L) / 1000 mL/L = 0.0135 mol

Next, we can use the mole ratio between AgNO3 and AgCl to calculate the volume of AgNO3 needed:

moles of AgNO3 : moles of AgCl = 1 : 1

moles of AgNO3 = molarity of AgNO3 × volume of AgNO3

volume of AgNO3 = moles of AgNO3 / molarity of AgNO3

volume of AgNO3 = 0.0135 mol / 1.5 mol/L = 0.009 L or 9.0 mL

Therefore, the answer is B) 9.0 mL.

Silver Nitrate, AgNO3, Can Be Used to Test for the Presence

Silver Nitrate, AgNO₃, Can Be Used to Test for the Presence