# Unknown Acid Titration

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Unknown Acid Titration
Titration Lab

A Titration is a process of the concentration of one solution being determined by its reaction with either a standard solution or a known quantity of solid dissolved in solution. It may also be used to calculate the molar mass of an unknown acid or base.
Purpose:
I. Prepare a standard solution of sodium hydroxide II. Standardize a sodium hydroxide solution by using potassium hydrogen phthalate (KHP) III. When given whether the acid is monoprotic, diprotic, or triprotic , determine the molar mass of the unknown organic acid. IV. Calculate the Molarity of the Soft drink.

Materials: * 50 mL Buret * Beaker * Erlenmeyer Flask * Sodium Hydroxide * Water * Balance * Unknown Acids
Repeat the same steps 1-4 from Section B to prepare for the titration of the unknown acid solution.
2. Repeat the same steps 5-7 substituting the unknown acid for KHP. The unknown acids are in labeled jars A, B, and C. It will be indicated whether the acids are monoprotic, diprotic, or triprotic. 10 titrations should be completed for each unknown acid.
3. From the equation on the first page, calculate the molar mass of the acid using your average molarity.
Find the molar mass based on the number of protons in each acid.
4. Accept the values that are within 1.0 of each other. Calculate the average of all the acceptable values and then repeat for the remaining acids.
5. When back in the classroom, you will receive the correct molar mass of the acids so you can calculate the percent error.

D- Calculation of Molarity of a soft drink solution
1. Repeat steps 1-4 from Section B to prepare for the titration of the soft drink solution.
2. Take the soft drink solution from a buret on the back lab table recording the initial and final volume from the soft drink buret. Add approximately 40 mL of the soft drink to your flask. Make sure you record the exact volume to the 100ths place. Do not add water to your
The concentration of one solution was determined by its reaction with a standard solution. The molar mass of unknown acids were also calculated. While learning to titrate, I learned several other skills in the process. I learned how to prepare a standard solution of sodium hydroxide, how to standardize a sodium hydroxide solution by using potassium hydrogen phthalate (KHP), how to find the molar masses of unknown organic acids when given whether the acid is monoprotic, diprotic, or triprotic, and how to calculate the molarity of a soft drink. At the same time, other skills were practiced. Skills such as calculating molarity, molar mass and percent error were exercised.
The molarity was calculated for part B, the standardization of sodium hydroxide. After all of the molarities were calculated, five of them were accepted and the average came out to be 0.0935, which was the number that would be used throughout the lab to help calculate the molar masses of the unknown acids and the molarity of a soft

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