Sodium Hydroxide Reaction Lab

4. To utilize the titration results to calculate the molarity of the hydrochloric acid and the

3.0g of salicylic acid was weighed then 3.0mL of acetic anhydride and 6 drops of 85% H3PO4 were added to it. The mixture was warmed over a water bath for 5 minutes while stirring. After warming, 20 drops of distilled water was slowly added. 15mL of water was added then the solution was heated until it became clear. It was allowed to cool and was placed in an ice bath until the solution becomes cloudy. Using pre-weighed filter paper, the mixture was filtered and was allowed to dry in the filter paper.

Since Alka Seltzer is swallowed and reacts with stomach acid, the vinegar is in this experiment is substituting as the stomach acid. The principle of limiting reagents relates to this lab because

* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube

In 2 and 7 I added 50 mL of .1 M NaCl. I added sodium acetate to the rest of the beakers: 1 gram to 3 and 8, 5 grams to 4 and 9, and 10 grams to 5 and 10. I then filled the beakers that contained the solid sodium acetate with 50 ml of .10 M acetic acid. Specifics can be found on page 84 of the lab manual. Though the lab manual instructed to use a pipet, we did not have an accurate 1 mL pipet or a graduated pipet, so we instead prepared two graduated burets with 1 M Sodium Hydroxide and 1 M hydrochloric acid. Using a standardized pH probe with a Lab Pro to measure changes in pH, we added 1 mL of HCl at a time and recorded the changes. The same was done for the NaOH.

lab bench. Place a beaker from the drawer on the stir plate. Drag the bottle of NH3 to the 5 mL graduated cylinder (the smallest one) by the sink and fill the cylinder by dropping the bottle on the cylinder. Now drag the 5 mL graduated cylinder to the beaker on the stir plate and add the 5 mL of

was to determine the percentage by mass of acetic acid in vinegar using acid/base titration. The

Volumetric burette: This instrument was filled with the sodium hydroxide solution that would be gradually added to the vinegar solution. The burette was used instead of a measuring cylinder as it gives a finer volume

1) Pour 25 mL of the 1 M hydrochloric acid into the beaker and rinse the solid by swirling the acid around in the bottom of the beaker.

The burette was then used to dispense 12.2 mL of solution into a 50 mL beaker. Then, the washed funnel and burette were used to measure and dispense 12.2 mL of 1 M NaOH into another 50 mL

Tools used in this experiment include an electronic scale, a Mohr pipette, a micropipette, test tubes, a bowl of ice, a mortar and pestle, and a ruler. Materials needed include liver extract from bovine liver, water (distilled and regular), hydrogen peroxide, apple cider vinegar, baking soda, and pH paper. In order to achieve and determine our results, we prepared 6 test tubes, each with 2.0 mL of hydrogen peroxide (3% H2O2). We then added 2.0 mL of distilled water into 2 test tubes making that our controlled substance, 0.22g of baking soda into another test tube, 0.24g baking soda into a 4th test tube, and 8.0 mL of apple cider vinegar into the last test tube. The 2 test tubes with the baking soda were used as our basic solution and the 2 test tubes with the apple cider vinegar were used as our acidic solution.

Next prepare your burette for use by rinsing through with distilled water catching the runoff water in the waste beaker. Once clean, use the funnel to carefully pour the 100ml 1.0M NaOH solution into the top of the burette (making sure the stopcock is closed and there are no air bubbles) filling as accurately to 0.00 as possible. If not starting on 0.00 then record actual level as your starting point.

Once neutralized, the unknown base would be expected to precipitate out of the solution and would then be able to be vacuum-filtered producing the unknown base component as a solid. The remaining acid and neutral components in the separatory funnel can then undergo a second extraction with 20mL of NaOH. Much like the unknown base, the unknown acid would become soluble with NaOH and would be easily extracted from the separatory funnel leaving an organic layer of the neutral component in the funnel. The unknown acid component could then be neutralized with HCl in an ice bath to precipitate out and vacuum-filtered just like the unknown base giving an isolated unknown acid solid. The remaining layer contained the neutral was then dried using Na2SO4 and gravity filtered using a glass funnel and cotton swab in the funnel to filter Na2SO4 from the liquid.

Submerge the graduated cylinder in the plastic tub so that it is completely filled with water. Hold the open end of the graduated cylinder and move it vertically upside-down where the open end of the graduated cylinder is still submerged in the plastic tub. Clamp the graduated cylinder the ring stand of the lab table to keep it in place. perforate a hole in the top of the rubber cork for the solution container. Cut a straw the length of about four inches. place the straw inside of the rubber cork hole. Set up your timer for two minutes.

3. A few drops of 6 M acetic acid were added until it became basic.