Question

At set times during the reaction, you will remove an aliquot of the reaction mixture and titrate it with a known concentration of base. show how to calculate each of the following values for an aliquot removed at time "t": a. if the aliquot is titrated with 0.052 mol/l of naoh solution and the equivalence point is reached after 3.8 ml of naoh is added, how many moles of naoh were added to reach the equivalence point?

Answer 1

To find the number of moles of NaOH added to the aliquot to reach the equivalence point, multiply the concentration of the NaOH solution (0.052 mol/L) by the volume of NaOH dispensed (3.8 mL or 0.0038 L), which yields 0.0001976 mol of NaOH.

Step-by-step explanation:

To calculate the number of moles of NaOH that were added at time "t" to reach the equivalence point in a titration, you need to use the concentration of the NaOH solution and the volume of NaOH that has been dispensed from the burette. The provided concentration of the NaOH solution is 0.052 mol/L, and the volume added to reach the equivalence point is 3.8 mL, which is equivalent to 0.0038 L (since 1 mL = 0.001 L).

Using these values, calculate the number of moles of NaOH using the formula:

Number of moles of NaOH = Concentration (mol/L) × Volume (L)

Number of moles of NaOH = 0.052 mol/L × 0.0038 L = 0.0001976 mol

Therefore, 0.0001976 mol of NaOH were added to the aliquot to reach the equivalence point.