Question

Concentration HCl -- 0.35 M

Volume HCl -- 24.35 mL
Volume NaOH -- 36.44 mL
The data above refers to a titration of NaOH with a known concentration of HCl. Calculate the moles of HCl at the end point.

Answer 1

To determine the moles of HCl at the end point of the titration, multiply the volume of HCl (converted to liters) by its molarity. In this case, 0.02435 L of 0.35 M HCl results in 0.0085225 moles of HCl that reacted at the end point.

Step-by-step explanation:

To calculate the moles of HCl at the end point of a titration with NaOH, you use the provided concentration and volume of HCl. If we have a concentration of 0.35 M HCl and a volume of 24.35 mL (which is 0.02435 L), the number of moles of HCl can be calculated as follows:

# moles HCl = (Volume of HCl in L) × (Concentration of HCl in M)

= (0.02435 L) × (0.35 M)

= 0.0085225 mol HCl

This calculation indicates that at the end point of the titration, 0.0085225 moles of HCl have reacted with the NaOH.

Since the balanced chemical reaction between HCl and NaOH is HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l), which shows a one-to-one mole ratio, at the end point, an equal number of moles of NaOH have also reacted.