Titration is a process in which an unknown concentration of an acid is determined in a solution. By this approach, a base solution is added to an acidic solution until an equilibrium is reached between the two substances. When the titration has reached an endpoint, or neutralization, the color of the solution will change. With the volume calculated at the end of this reaction, it is possible to determine the concentrations of the acid and the base of the solution.
The experiment to be conducted involves the standardization of NaOH ( sodium hydroxide) using KHP ( potassium hydrogen phthalate ) and the titration of an unknown acid. By use of a colorless indicator, Phenolphthalein, the end point of neutralization is established. Soon after this process is completed, the concentration of the NaOH will be calculated . In Part two
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In a beaker containing 500mL of distilled water, dissolve 2.0-2.3 g of NaOH.
In a Erlenmeyer flask, determine the mass of 0.4- 0.6 g of KHP ( Potassium hydrogen Phthalate ).
Adding 25-30 mL of water to the flask, dissolve the KHP.
Once dissolved add 3-4 drops of phenolphthalein to the solution.
Rinse the buret with two, 5 mL portions of the NaOH solution.
Fill the buret with the NaOH solution and expel any air bubbles. Empty excess liquid into a 50 mL beaker.
Record the initial buret reading to +/- 0.01 mL at the meniscus.
At a gradual pace, begin opening the stopcock to release NaOH into the KHP solution, shaking the flask in a circular motion.
Slow the amount released by the buret when a faint pink color appears, but disappears shortly after. Continue this process until a vibrant pink color remains.
Record the final volume of the solution and calculate molarity.
Repeat this procedure two more times and receive an average of all trials.
Part 2: Identification of an Unknown
Rinse your beaker thoroughly to wash any excess powder. 12. Repeat steps 7-11 3 more times for reliability. To make sure the temperature still stays hot by continue heating the water a little bit using the hot plate. 13.
Place a clean, dry 125 mL Erlenmeyer flask on balance, and slowly dispense liquid bleach until there is about .5 g. Record the mass of bleach, and add 25 mL of de-ionized water and about 2 g of KI. Swirl contents until the KI dissolves. Then add 3 drops of 1 M H2SO4, mix, and let stand for 1 or 2 minutes.
Each subsequent trial will use one gram more. 2.Put baking soda into reaction vessel. 3.Measure 40 mL vinegar. 4.Completely fill 1000 mL graduated cylinder with water.
neutralize 35ml of our base. Once we weighed out the KHP we then dissolved it
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
I rinsed the burette by opening the tap and allowing the HCl to flow, which released any air bubbles and cleaned the tip of the burette. After adding 5 drops of phenolphthalein indicator, the solution turned pink.
Remove the extra solvent on a steam bath under a hood while flushing the flask with N2 gas, leaving the crude extract. Weigh extract.
The initial and final volumes of NaOH were compared after the solution was titrated in five different
While the solution is cooling, you need NaOH. Add 50g NaOH into the jar and pour 50ml dH2O. The solution will be very hot so cool it by putting it in the freezer. When the two solutions are cooled, start to pour NaOH solution. Pour in small amounts because all of the mixes in the Erlenmeyer flask will start to heat. Add it slowly and stir after addition. You need to do this while you see 2 layers; the ph will be 10-12. When the NaOH is added, wait while all solution cools because you need to pick the top layer
Tweezers Petri dishes Graduated Cylinders Test tubes Procedure: In 100 mL of water, put 3.5 grams of NaCl In a separate test tube, put 9 mL of the solution and 1 mL of water In another test tube, place 8
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and
The experiment in this laboratory is to study pH and buffers. The pH is defined as the –log[H+] and measures the molar concentration of hydrogen ions. In the study of life, life can only be stabilized through a buffer. A buffer is a solution that is able to resist pH change and maintain the stability of everyday life. A buffer requires a weak acid and its conjugated base. When a solution such as an acid or base presents itself into the buffer solution, the buffer will neutralize the amount of acids or base added to the solution. As a result, pH maintains stabilization and cells are able to function properly. In this study experiment, sodium chloride is the tested solution. Sodium chloride (NaCl) is commonly known to many as salt. NaCl is tested
For this experiment we used titration to standardize the exact concentration of NaOH. Titration is the process of carefully adding one solution from a buret to another substance in a flask until all of the substance in the flask has reacted. Standardizing is the process of determining a solutions concentration. When a solution has been standardized it is referred to as a standard solution. To know when a solution is at its end point an indicator is added to acidic solution. An indicator is an organic dye that is added to an acidic solution. The indicator is one color is in the acidic solution and another color in the basic solutions. An end point occurs when the organic dye changes colors to indicate that the reaction is over (Lab Guide pg. 141).