Question

Titration Objective Determine the concentration of a solution of sodium hydroxide (NaOH) using a 0.500 M potassium hydrogen phthalate (KHP) standard solution. This will be done using a simulated experiment on ChemCollective. Background You are working as a chemical laboratory assistant and you observe a bottle of NaOH on a shelf with an approximate concentration. You need to know the exact concentration of the NaOH to conduct an experiment for your supervisor. With only a standardized KHP solution on hand, you come up with a great idea to determine the concentration of the NaOH solution by doing a titration. You decide to use the acid-base indicator phenolphthalein to determine the end-point of the titration between NaOH and KHP. You will add the indicator (colorless) to KHP and proceed to do the titration with NaOH. Once all the KHP reacts with NaOH, the first excess drop of NaOH will cause the indicator to convert to its basic form and the solution becomes light pink. Procedure: Conduct the titration three times and determine an average concentration of NaOH Data Trial 1 Trial 2 Trial 3 Volume of KHP, mL 25.00 mL 25.00 mL 25.00 mL Molarity of KHP, M Final Burette reading, mL Initial Burette reading, mL Volume of NaOH used No. of moles of KHP, mol No. of moles of NaOH, mol Molarity of NaOH solution Average molarity Data Processing Show full calculations for only one determination of the molarity in your lab report. Be sure to include a balanced equation for the reaction. NaOH(aq) + KHC8H4O4 → Post-lab Question The molar concentration of HCl in a solution can be determined by titration with NaOH according to the equation below: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) Consider the following titration experiment: 10.00 mL sample of the HCl solution was added to a 125 mL flask and 50 mL of distilled water was added and 3 drops of phenolphthalein indicator solution. The resulting solution requires 44.00 mL of 0.1250M NaOH solution to reach the endpoint. Calculate the number of moles of NaOH required for the titration Calculate the number of moles of HCl in the HCl sample titrated Calculate the molarity of HCl

Titration

Objective

Determine the concentration of a solution of sodium hydroxide (NaOH) using a 0.500 M potassium hydrogen phthalate (KHP) standard solution. This will be done using a simulated experiment on ChemCollective.

Background

You are working as a chemical laboratory assistant and you observe a bottle of NaOH on a shelf with an approximate concentration. You need to know the exact concentration of the NaOH to conduct an experiment for your supervisor. With only a standardized KHP solution on hand, you come up with a great idea to determine the concentration of the NaOH solution by doing a titration. You decide to use the acid-base indicator phenolphthalein to determine the end-point of the titration between NaOH and KHP. You will add the indicator (colorless) to KHP and proceed to do the titration with NaOH. Once all the KHP reacts with NaOH, the first excess drop of NaOH will cause the indicator to convert to its basic form and the solution becomes light pink.

Procedure:

Conduct the titration three times and determine an average concentration of NaOH

Data

Trial 1
Trial 2
Trial 3
Volume of KHP, mL
25.00 mL
25.00 mL
25.00 mL
Molarity of KHP, M
Final Burette reading, mL
Initial Burette reading, mL
Volume of NaOH used
No. of moles of KHP, mol
No. of moles of NaOH, mol
Molarity of NaOH solution
Average molarity

Data Processing

Show full calculations for only one determination of the molarity in your lab report.

Be sure to include a balanced equation for the reaction.

NaOH(aq) + KHC8H4O4 →

Post-lab Question

The molar concentration of HCl in a solution can be determined by titration with NaOH according to the equation below:

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

Consider the following titration experiment:

10.00 mL sample of the HCl solution was added to a 125 mL flask and 50 mL of distilled water was added and 3 drops of phenolphthalein indicator solution. The resulting solution requires 44.00 mL of 0.1250M NaOH solution to reach the endpoint.

Calculate the number of moles of NaOH required for the titration

Calculate the number of moles of HCl in the HCl sample titrated

Calculate the molarity of HCl

Added by Danielle W.