You are titrating an unknown weak acid you hope to identify. Your titrant is a 0.0935 mol/L NaOH solution, and the titration requires 39.9 mL to reach the equivalence point. How many moles of acid were in your sample?
To determine the number of moles of acid in the sample, we need to use the equation:
moles of acid = moles of base
Given:
Concentration of NaOH solution (Titrant) = 0.0935 mol/L
Volume of NaOH solution used (Titrant) = 39.9 mL = 0.0399 L
Using the equation:
moles of acid = concentration of NaOH solution × volume of NaOH solution
moles of acid = 0.0935 mol/L × 0.0399 L
We can now calculate the moles of acid in the sample:
moles of acid = 0.00372665 mol
Therefore, there were approximately 0.00373 moles of acid in the sample.
To determine the number of moles of acid in the sample, you need to use the balanced chemical equation for the neutralization reaction between the acid and NaOH.
1. Write the balanced chemical equation:
Acid + NaOH → Salt + Water
2. From the balanced chemical equation, we can see that the stoichiometry between the acid and NaOH is 1:1. This means that for every mole of acid, you need one mole of NaOH to reach the equivalence point.
3. Determine the volume of NaOH used in liters:
39.9 mL = 39.9 / 1000 L = 0.0399 L
4. Calculate the number of moles of NaOH used:
Moles = concentration (mol/L) × volume (L)
Moles of NaOH = 0.0935 mol/L × 0.0399 L = 0.00373 mol
5. Since the stoichiometry between the acid and NaOH is 1:1, the number of moles of acid in the sample is also 0.00373 mol.
Therefore, there were 0.00373 moles of acid in your sample.