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 AgNO₃ will be required to react with 30.0 mL of a 0.45 M HCl solution AgNO₃(aq)+ HCl(aq)→ 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 calculate the moles of HCl in the 30.0 mL solution: 0.45 mol/L x 0.030 L = 0.0135 mol HCl Since the stoichiometry of the reaction is 1:1 between AgNO₃ and HCl, we know that we need 0.0135 mol of AgNO₃ to react with the HCl. Now, we can use the formula: moles = concentration x volume to find the volume of 1.5 M AgNO₃ needed: 0.0135 mol = 1.5 mol/L x volume volume = 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