Assessment Of Hcl 0.1 N With The Standard Na2co3a
1. Prepare 100 mL of a 0.08 N Na2CO3 solution from a 1M Na2CO3 solution.
2. Using a volumetric pipette, transfer a 20 mL aliquot of the Na2CO3 solution to each Erlenmeyer flask (there are three replicates).
3. Add 100 mL of distilled water to each Erlenmeyer flask.
4. To the first Erlenmeyer flask add 0.3 mL of the phenolphthalein indicator, to the other two flasks add 0.5 mL of methyl orange.
5. The HCl solution was added to a 50 mL burette.
6. The aliquot of the first flask, to which the phenolphthalein has been added, was titrated with the HCl solution. After adding the first 4 mL of HCl, the solution is heated to boiling.
7. Continue the titration slowly in this Erlenmeyer flask until the solution turns from pink to colorless. You must add small volumes of 0.5 mL

Based on what you read, answer the following questions:

A. Why does the solution in the Erlenmeyer flask heat up during the titration of the HCl solution?

B. What is the theoretical pH value when half the carbonate equivalence has been neutralized and the neutralization reaction with HCl is complete?

Answer rating: 100% (QA)

A The solution in the Erlenmeyer flask heats up during the titration of ... View the full answer