Question

All calculations must be shown. all data must be reported with correct number of sig. fig., and proper units, otherwise points will be deducted.

experimental data trial 1 trial 2
1) molarity of hcl solution, m 0.200 m 0.200 m
2) initial hcl burette reading, ml 0.00 ml 0.00 ml
3) final hcl burette reading, ml
4) volume of hcl solution used, ml 5.00 ml 5.12 ml
5) initial naoh burette reading, ml 0.00 ml 10.22 ml
6) final naoh burette reading, ml 9.94 ml 20.56 ml
7) volume of naoh solutionrequired, ml

calculations
molarity of HCl solution, m
volume of HCl solution used, l
number of moles of HCl, mol
number of moles of NaOH, mol
volume of naoh solution, l
molarity of NaOH solution, m

Answer 1

To find the volume of NaOH needed, use the mole ratio between HCl and NaOH from the balanced chemical equation, and then apply the formula: Volume = Moles of NaOH / Molarity of NaOH, ensuring to report in milliliters with the correct significant figures and units.

Step-by-step explanation:

The question deals with determining the volume of an NaOH solution required to neutralize a given number of moles of HCl, given the molarity of the NaOH solution. To solve this, we use the stoichiometry of the chemical reaction between HCl and NaOH, which is:

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

From the balanced equation above, it's clear that the reaction ratio is 1:1 — for every mole of HCl, one mole of NaOH is required. If we have the number of moles of HCl and the molarity (M) of the NaOH solution, we can calculate the volume (V) of the NaOH solution needed using the formula:

Moles of NaOH = Molarity of NaOH × Volume of NaOH in liters

Rearranging for volume, we get:

Volume of NaOH in liters = Moles of NaOH / Molarity of NaOH

Make sure when you perform this calculation that the final volume is reported in milliliters (mL), and keep in mind to report with the correct number of significant figures and proper units.