Neutralisation of an Alkali
In this investigation, I plan to find a pattern or rule in the
neutralisation of an alkali. I plan to use hydrochloric acid and
sodium hydroxide. I will use the indicator, phenolphthalein, to tell
when the sodium hydroxide has been neutralised, which will turn from
purple to clear.
The Background of the Reaction
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The reaction is neutralisation.Neutralisation is where an acid and
alkali are mixed to neutralise the substance to pH7.
Acids and alkalis are chemical opposites - when they react together,
they "cancel each other out".
The reaction equation:
Hydrochloric acid + Sodium hydroxide = Water + Salt
HCl + NaOH = H20 + NaCl
Ion Reaction
============
The sodium hydroxide gives an OH-ion and the hydrochloric acid gives
an H+ ion.
When mixed together, they cancel each other out and the substance is
neutralized to make H20. After this has happened, the sodium and the
chlorine (that is left over from the sodium hydroxide and hydrochloric
acid) mix with each other to make a salt (sodium chloride).
Apparatus and Equipment
- Sodium Hydroxide
- Hydrochloric Acid
- 1 flask
- 1 burette
- phenolphthalein
- boss & clamp
Method
Set up equipment:
The flask contains one of three different volumes of sodium hydroxide
- 5, 10, or 15cm³, and a few drops of the indicator, phenolphthalein.
The burette is full of hydrochloric acid.
Add the hydrochloric acid in small drops to the sodium hydroxide.
Record how much acid is required for the phenolphthalein to turn
clear.
Predictions
I did the experiment for 3 different variables and then noticed a
pattern. For the last 7 rows of results, I predicted the outcome
(shown in green).
Acid (Hydrochloric)
Alkali (Sodium Hydroxide)
Concentration
(Moles)
Volume
(cm3)
Amount
(Moles)
Concentration
(Moles)
Volume
2-ethyl-1,3-hexanediol. The molecular weight of this compound is 146.2g/mol. It is converted into 2-ethyl-1-hydroxyhexan-3-one. This compounds molecular weight is 144.2g/mol. This gives a theoretical yield of .63 grams. My actual yield was .42 grams. Therefore, my percent yield was 67%. This was one of my highest yields yet. I felt that this was a good yield because part of this experiment is an equilibrium reaction. Hypochlorite must be used in excess to push the reaction to the right. Also, there were better ways to do this experiment where higher yields could have been produced. For example PCC could have been used. However, because of its toxic properties, its use is restricted. The purpose of this experiment was to determine which of the 3 compounds was formed from the starting material. The third compound was the oxidation of both alcohols. This could not have been my product because of the results of my IR. I had a broad large absorption is the range of 3200 to 3500 wavenumbers. This indicates the presence of an alcohol. If my compound had been fully oxidized then there would be no such alcohol present. Also, because of my IR, I know that my compound was one of the other 2 compounds because of the strong sharp absorption at 1705 wavenumbers. This indicates the presence of a carbonyl. Also, my 2,4-DNP test was positive. Therefore I had to prove which of the two compounds my final product was. The first was the oxidation of the primary alcohol, forming an aldehyde and a secondary alcohol. This could not have been my product because the Tollen’s test. My test was negative indicating no such aldehyde. Also, the textbook states that aldehydes show 2 characteristic absorption’s in the range of 2720-2820 wavenumbers. No such absorption’s were present in my sample. Therefore my final product was the oxidation of the secondary alcohol. My final product had a primary alcohol and a secondary ketone
CL-, as the ions of H+ and OH- react to form H2O. These spectator ions
As shown in Fig. 5, the final pH of the NaClO-NH3 solution after simultaneous removal are 5.4, 6.9, 7.2, 7.5, 8.5, 9.6, 10.7, 11.5 and 12.8 with respect to the initial pH of 5, 6, 7, 8, 9, 10, 11, 12 and 13, from which, an interesting law can be concluded as that if the initial pH is an acidic, the final pH is slightly increased; but if the initial pH is an alkaline, the final pH is declined. NaClO-NH3 is macromolecule compounds with a large inter surface area. It contains abundant functional groups such as hydroxyl (OH), carboxyl (COO), quinone, amino (–NH2), etc, which determines that NaClO-NH3 is a salt of strong base and weak acid, as well the ionization equilibrium and hydrolytic equilibrium would be complicated. When the pH of the NaClO-NH3 solution was acidic, the functional groups such as OH, COO and NH2- would react with H+ to generate the NH3 sediment, resulting in a decrease of inter surface area owing to the block and a great loss of NaClO-NH3, then the NOx removal as well as the duration time was decreased. As for the increase of the final pH in the acidic conditions, this was a result of the consumption of H+ by NaClO. The decrease of the
Apparatus: * 1 measuring cylinder * 1 test tube * 1 stop clock * A large gelatine cube containing indicator and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly * Record your results and repeat this same process 3 times for each molar of acid: § 1 molar § 1.5 molar § 2 molar
Purpose/Introduction: In this experiment, four elimination reactions were compared and contrasted under acidic (H2SO4) and basic (KOC(CO3)3) conditions. Acid-catalyzed dehydration was done on 2-butanol and 1-butanol; a 2o and 1o alcohol, respectively. The base-induced dehydrobromination was performed on 2-bromobutane and 1-bromobutane isomeric halides. The stereochemistry and regiochemistry of the four reactions were analyzed by gas chromatography (GC) to determine product distribution (assuming that the amount of each product in the gas mixture is proportional to the area under its complementary GC peak).
Hydrochloric Acid, Sodium Thiosulphate Reaction. Research: What is the difference between Hydrochloric acid is a strong colourless acid formed when hydrogen chloride gas dissociates in water, used in industrial and laboratory. processes. The.
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Investigating Factors that Affect the Amount of Heat Produced in Neutralisation I am going to investigate factors that affect the amount of heat
Theories have often been developed to explain how delinquents violate social norms and still manage to maintain positive self images of themselves. Neutralization theory, developed by Gresham Sykes and David Matza in 1957 set out to do just this. Critics, however, have claims that the theory, on it’s own, is not a sufficient explanation for adolescent’s participation in crime in delinquency. It has also been claimed by critics that neutralization theory is best viewed as a components of larger theory of crime and can be incorporated into other theories such as social bond theory.
For the experiment, the effect of different alkaline solutions on the quality of yellow wet noodles was investigated. Four different formulations were used. For formulation A, sodium carbonate was used; formulation B, soda ash; formulation C, potassium carbonate and formulation D was the control with no alkaline solution added.
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