Materials: Solid potassium hydrogen phthalate (KHP) Sodium hydroxide (NaOH) solu
ID: 1074423 • Letter: M
Question
Materials: Solid potassium hydrogen phthalate (KHP) Sodium hydroxide (NaOH) solution Acetic acid (CH,COOH) solution Phenolphthalein indicator Distilled water 250 mL Erlenmeyer flask 25.0 mL volumetric pipette Pipette bulb Burette with stopcock Burette clamp Funnel Retort stand - Balance White paper - pH Meter - - - Part A-Standardization of NaOH Purpose: To calculate the exact concentration of the prepared solution of sodium hydroxide. In order to have accurate titration results we need to know the exact concentration of the sodium hydroxide we are titrating with. Procedure 1. Set up an observation table to record the initial and final volumes, of NaOH in your burette at the beginning and end of titration, volume used, as well as the mass of KHP for each trial. 2. Weigh approximately 1.00 g of potassium hydrogen phthalate (KHP - molecular formula KHC,H,O), and record the mass. Place the KHP into a clean Erlenmeyer flask. Add -50.0 mL of distilled water (enough to dissolve it) and two to three drops of phenolphthalein indicator. Swirl to mix the solution. 3. Carefully fill your burette with NaOH solution. Stop at the 5.0 mL line in order to not overfill the burette. Record the initial volume of NaOH in the burette. Remember to always record your volume at the bottom of the meniscus. 4. Place the Erlenmeyer flask over a sheet of white paper and slowly begin titrating with the NaOH solution. Be sure to add NaOH in slow increments to improve accuracy. Mix your solution during titration by swirling the flask. At the first sign of color change close the stopcock on your burette. From this point forward only 5. add one drop of NaOH at a time. Swirl to mix after each drop and watch for color change. 6. When the solution changes color permanently record the final volume of NaOH in the burette 7. Repeat steps 1-5 (complete at least three trials).Explanation / Answer
Standardization is important for every analytical measurement involving calculation. This is must especially with sodium hydroxide because of it's hygroscopic nature due to which it absorbs moisture from the air. So moisture that it has absorbed is also being weighed alongwith NaOH. Therefore, the concentration of the NaOH solution will be lesser than the calculated or prepared value.