Urgent: How many mols of HCl remained after neutralization by the antacid?

Question

25.00 mL of 1.034 M HCl was reacted with an antacid tablet and the remaining HCl was titrated with 1.068 M NaOH.

If the volume of NaOH at the end point of the titration was 18.50 mL, how many mols of HCl remained after neutralization by the antacid?

a.

b.

c.



d.

Answer 1

Hello, Abigail,

The balanced equation for the HCl and NaOH reaction tells us the it takes one mole of NaOH per one mole HCl. Referencing the table below, first calculate how many moles of each are involved in the two solutions by multiplyng the volumes (in LITERS!) times their molarity (moles/Liter). We used 0.020 moles of NaOH to the titration endpoint. Since it is a 1 mole to 1 mole ration, this means that 0.020 moles of HCl was reacted. This leaves 0.026 - 0.020 moles of NaOH, or 0.00609 moles remaining.

Bob