Question

What volume (in L) of 0.150 M KCl solution is required to completely react with 0.150 L of a 0.175 M Pb(NO3)2 solution, according to the following balanced equation:

Answer 1

To determine the volume of the KCl solution required to react with the Pb(NO3)2 solution, use the stoichiometry of the balanced equation and calculate the moles of each reactant. Then, use the concentration to calculate the volume of the KCl solution needed.

Step-by-step explanation:

To determine the volume of the KCl solution required to react with the Pb(NO3)2 solution, we can use the stoichiometry of the balanced equation. From the balanced equation: Pb(NO3)2(aq) + 2KCl(aq) → PbCl2(s) + 2NaNO3(aq), we can see that 1 mole of Pb(NO3)2 reacts with 2 moles of KCl.

First, calculate the number of moles of Pb(NO3)2 using the volume and concentration given: Moles of Pb(NO3)2 = Volume of Pb(NO3)2 solution (L) × Concentration of Pb(NO3)2 solution (M) = 0.150 L × 0.175 M = 0.02625 mol.

Since the stoichiometric ratio is 1:2, we need double the moles of KCl: Moles of KCl = 2 × Moles of Pb(NO3)2 = 2 × 0.02625 mol = 0.0525 mol.

Next, calculate the volume of the KCl solution needed using the concentration: Volume of KCl solution = Moles of KCl / Concentration of KCl solution = 0.0525 mol / 0.150 M = 0.35 L.