An acid solution is 0.100 mol L^-1 in HCl and 0.200 mol L^-1 H₂SO₄. What volume of a 0.150 mol L^-1 KOH solution would completely neutralize 500.0 mL of this solution?

Question

Quizplus · Accepted Answer

Step 1: Write the balanced chemical equation for the neutralization reaction: HCl + KOH → KCl + H2O Step 2: Determine the number of moles of HCl present in the solution: 0.100 mol/L x 0.500 L = 0.050 mol HCl Step 3: Determine the number of moles of H₂SO₄ present in the solution: 0.200 mol/L x 0.500 L = 0.100 mol H₂SO₄ Step 4: Determine the total number of moles of acid present in the solution: 0.050 mol + 0.100 mol = 0.150 mol Step 5: Use the mole ratio from the balanced equation to determine the number of moles of KOH needed to neutralize the acid: 1 mol HCl : 1 mol KOH 0.150 mol HCl : x mol KOH x = 0.150 mol KOH Step 6: Use the concentration and volume of the KOH solution to determine the volume needed to supply the required number of moles: 0.150 mol/L x V = 0.150 mol V = 1.00 L However, this is the volume needed to completely neutralize 1.00 L of the acid solution. Since we are starting with only 500 mL (0.500 L) of the acid solution, we need half the volume of the KOH solution: V = 0.500 L x 1.00 L/0.150 mol = 3.33 L V = 3.33 L / 2 = 1.67 L Therefore, the best choice is C.

An Acid Solution Is 0