Question

In a titration, 54.5 mL of 0.6 M hydrochloric acid solution is needed to neutralize 78 mL of potassium hydroxide. What is the molarity of the base?

Answer 1

Is it 0.42?

Answer 2

Yes. I obtained 0.419 M

Answer 3

[AI-generated answer — Explain Bot]

To find the molarity of the potassium hydroxide (base), you need to use the concept of mole-to-mole ratio from the balanced chemical equation. The balanced equation for the neutralization reaction between hydrochloric acid (HCl) and potassium hydroxide (KOH) is as follows:

HCl + KOH -> KCl + H2O

According to the equation, the mole ratio between HCl and KOH is 1:1. This means that 1 mole of HCl reacts with 1 mole of KOH to produce 1 mole of water.

First, we need to determine the number of moles of HCl. To do that, we can use the equation:

moles of HCl = molarity × volume (in liters)

Given that the volume of HCl used is 54.5 mL (which is 0.0545 L) and the molarity of HCl is 0.6 M, we can calculate the moles of HCl as follows:

moles of HCl = 0.6 M × 0.0545 L = 0.0327 moles

Since the mole ratio between HCl and KOH is 1:1, the number of moles of KOH will also be 0.0327 moles.

Next, we can determine the molarity (M) of the KOH solution by using the given volume of KOH and the number of moles of KOH:

Molarity of KOH = moles of KOH / volume of KOH (in liters)

Given that the volume of KOH used is 78 mL (which is 0.078 L), we can calculate the molarity of KOH as follows:

Molarity of KOH = 0.0327 moles / 0.078 L = 0.419 M

Therefore, the molarity of the potassium hydroxide (base) is 0.419 M.