Determining the Volume of Acid that Will React with a Carefully Measured Volume of Alkalai
Aim
The aim of this experiment is to determine the volume of acid that
will react with a carefully measured volume of alkali (base).
Prediction
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Universal indicator
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Acid Alkali Neutral
Red Purple Green
Methyl orange
Acid Alkali Neutral
Red Yellow Yellow
Methyl red
Acid Alkali Neutral
Orange Blue Red
Phenolphthalein
Acid Alkali Neutral
Clear Purple Clear
My prediction when using 10ml of 0.02m solution of sodium hydroxide
(NaOH) is that 75ml of hydrochloric acid (HCl) will be needed for
neutralisation. I also predict that when using 10ml of 0.15m solution
of sodium hydroxide is that 15ml of sulphuric acid (H2SO4).
I also predict that when I add the acid and bases together they will
react forming other chemicals as such: -
NaOH + HCl = H2O + NaCl
The sodium hydroxide and the hydrochloric acid will react together and
produce water and sodium chloride.
2NaOH + H2SO4 = H2O + Na2SO4
The sodium hydroxide and the sulphuric acid react together and produce
water and sodium sulphate.
Method
The apparatus was set up as shown.
Universal indicator was used to show firstly the acid and alkali and
secondly that the neutralisation had taken place. 10ml of 0.15m NaOH
was placed in a conical flask and after making sure that the tap on
the burette was closed, 0.02m of HCl was placed into the burette. This
was released slowly until the indicator turned green showing
neutralisation had taken place. The test was repeated exactly but
instead of HCl, H2SO4 with a molar of 0.1 was used in its place. The
amount of acid used to neutralise the base was recorded in both cases.
The type and volume of acid that was used in these tests were
variable.
Safety
Normal laboratory safety conditions applied.
Other safety precautions that had been taken were goggles were worn to
Experiment: First prepared a well plate with the appropriate amounts of distilled water, HCl, and Na2S2O3 in each well according to the lab manual. The well where the reaction
Firstly, an amount of 40.90 g of NaCl was weighed using electronic balance (Adventurer™, Ohaus) and later was placed in a 500 ml beaker. Then, 6.05 g of Tris base, followed by 10.00 g of CTAB and 3.70 g of EDTA were added into the beaker. After that, 400 ml of sterilized distilled water, sdH2O was poured into the beaker to dissolve the substances. Then, the solution was stirred using the magnetic stirrer until the solution become crystal clear for about 3 hours on a hotplate stirrer (Lab Tech® LMS-1003). After the solution become clear, it was cool down to room temperature. Later, the solution was poured into 500 ml sterilized bottle. The bottle then was fully wrapped with aluminium foil to avoid from light. Next, 1 mL of 2-mercaptoethanol-β-mercapto was added into fully covered bottle. Lastly, the volume of the solution in the bottle was added with sdH2O until it reaches 500 ml. The bottle was labelled accordingly and was stored on chemical working bench.
Well, this looks like its using some calculations so what I would do is take my 0.045 M and equal it to the 0.25 mL of NH3 and multiply that by 45.0 mL and multiply it by 10 with an exponent of negative 3. Once all of that is multiplied together we should get an answer of 0.01135 moles of our HCI. Now we can find our “Concentration” Which means we would divide our moles (0.01125) to our vol in liters which is 0.025, once we do that, we get an answer of 0.045M of our NH3. Well, since we are on the topic of pH we know that we can use the formula: pH = -log (H3O+). Then what we would do is plug everything into the formula: pH equals -log (2.4 multiplied by 10 (with an exponent of -5). Once we find the answer to this and we add up all of our calculations, we can come to a conclusion that the answer is: 4.6197 as our pH.
Note to environmentalists: The sulfuric acid was completely neutralized and properly discarded. Credits I would like to thank all the people who helped me with this project. I would especially like to thank my mother, for letting my go through an abundance of Baking Soda, Vinegar, and many of our other household items. I would like to thank my Father for helping me understand the science of this project, and my whole family for helping me do well. I'd also like to give credit to the following Brands of substances I used: Arm & Hammer Drano Revco Aspirin Mylanta Seaway And any other products I may have used along the way.
This was allowed to mix for a few minutes; a little excess water was used to ensure that sodium bromide was fully dissolved. This mixture was placed in an ice bath while continuing to stir. 1.3 ml (24.39 mmols) of concentrated sulfuric acid was added dropwise. The flask was removed from the ice bath and heated to reflux for 1 hour while continuing to stir. The resulting top layer was transferred to a conical vial in which 1.5 mL (22.51 mmols) of 80 % sulfuric acid was added. 2.0 mL of water was added to allow a layer to form. The bottom layer was removed and transferred to another conical vial in which 2.0 mL of saturated sodium bicarbonate was added. The bottom, organic layer, was transferred to a conical vial. Calcium chloride, a drying agent, was used to collect the remaining aqueous layer that
Acid-Base Titration I. Abstract The purpose of the laboratory experiment was to determine equivalence. points, pKa, and pKb points for a strong acid, HCl, titrated with a. strong base, NaOH using a drop by drop approach in order to determine. completely accurate data. The data for this laboratory experiment is as follows.
To neutralize 10 mL of Acid ‘A’ we used 3.35 mL of Sodium Hydroxide and to neutralize 10 mL of...
of distilled water. For the 1M solution I added 50 cm3 of HCl and 50
This is very important as changing the volume can have a negative effect on your experiment and report. Make sure that you use 10cm3 of hydrochloric acid throughout all the 5 trials, You can measure the volume with help of a measuring cylinder or you can also use a pipette to measure it accurately
The Purpose of the Chemical Reaction Lab was to examine and measure the chemical reaction of H-C-L, hydrochloric acid and CuCl2, Copper chloride solution to determine different types of reactions, within specific elements and compounds; Aluminum foil, Al aluminum shot, Ammonium hydroxide, Magnesium, Silver nitrate, Sodium carbonate, Sodium bicarbonate, Sodium hydroxide, and Zinc. By completing the trials, the data displayed chemical changes. These changes were observable in changes of substances, such as formation of precipitate, change in color, release of gas, and difference of temperature.
Prepare .05 to .075 g of crude lipid by dissolving it in hexane. Add to the silica gel slurry in the column.
Chemistry: Acid-Base Titration. Purpose: The objective of this experiment were: a) to review the concept of simple acid-base reactions; b) to review the stoichiometric calculations involved in chemical reactions; c) to review the basic lab procedure of titration and introduce the student to the concept of a primary standard and the process of standardization; d) to review the calculations involving chemical solutions; e) to help the student improve his/her lab technique Theory: Titration was used to study acid-base neutralization reaction quantitatively. In acid-base titration experiment, a solution of accurately KHP concentration was added gradually to another solution of NaOH concentration until the chemical reaction between the two solutions was completed. The equivalence point was the point at which the acid was completely reacted with or neutralized by the base.
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
50 mL of deionized water and 6 mL of 6.0 M h2so4 was also added. This was repeated two more times for a total of three flasks. A flask was placed on a hot plate and heated until it was at 80 C. As the solution was heated a burette was filled with a KMno4 solution. After the solution was at the required heat a magnetic stir bar was added to create a whirlpool. The KMno4 was then titrated into the solution until the heated solution turned light pink in color. This process was repeated for the two other flasks. The average molarity was then found for the kMno4
In my experiment, I will use an overall volume of 50 cm³ of 2moles of