Question

1. For the titration of 3.00 M hydrochloric acid with 2.00 M sodium hydroxide, what volume of sodium hydroxide would be required to react with 1.00 L of hydrochloric acid to reach the endpoint

Answer 1

The reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) is a neutralization reaction and can be written as follows:

HCl + NaOH → NaCl + H2O

From the balanced chemical equation, we see that the ratio of HCl to NaOH is 1:1. This means that one mole of HCl reacts with one mole of NaOH.

First, we need to calculate the number of moles of HCl in the 1.00 L solution:

Moles of HCl = Molarity * Volume

Moles of HCl = 3.00 moles/L * 1.00 L = 3.00 moles

Since the ratio of HCl to NaOH is 1:1, 3.00 moles of HCl will react with 3.00 moles of NaOH.

We can now find the volume of the 2.00 M NaOH solution needed to react with 3.00 moles of HCl using the formula:

Volume = Moles / Molarity

Volume = 3.00 moles / 2.00 moles/L = 1.50 L

So, 1.50 liters of the 2.00 M NaOH solution would be required to react with 1.00 L of the 3.00 M HCl solution to reach the endpoint.