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.
* 50 mL Buret
* Erlenmeyer Flask
* Sodium Hydroxide
* Unknown Acids (A, B, C)
* Soft Drink (Ginger Ale)
A – Preparation of NaOH (standard solution)
1. With portions of water, rinse a 2L bottle.
2. To make 2L of a 0.1M solution, determine the amount of grams of sodium hydroxide that are needed and then weigh out the correct number of grams when showing the calculation.
3. To a container that is ½ to 1/3 full of water, add the pellets of sodium hydroxide. Shake to mix or speed up the dissolving of the pellets and fill to the top with water. Label your container with your name and date.
B - Standardization of NaOH (Determine the actual concentration of the standard solution) 1. Drain the 50 mL buret and remember to fill the buret with water at the end of each lab.
2. To rinse the inside of the buret, pour a small amount of NaOH into it. Drain the buret through the stop cock. Rinse the buret more than once. (Remember to do this before you start th lab experiment to clean the buret.)
3. Fill the buret with the NaOH solution and to remove any air, allow a small quantity to pass through the stopcock.
4. Rinse a 250 mL Erlenmeyer flask and then make sure the bottom of the flask is dry. To get the mass of only the solute, rezero the flask on the...
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