Neutralising Hydrochloric Acid
Over the past few weeks we have been learning about most chemical
reactions, acids and bases, and endothermic and exothermic reactions
are the main things do to with this investigation.
A base is used usually to neutralise acids, we are in the
investigation looking to see weather Magnesium, Magnesium Oxide, or
Magnesium Carbonate can significantly neutralise Hydrochloric acid.
Aim
We aim to in this experiment to see if one of Magnesium, Magnesium
Oxide, or Magnesium Carbonate can neutralise Hydrochloric Acid in an
exothermic reaction to a PH of seven.
Equipment
The items needed to do this investigation are:
1. A test tube rack.
2. Three test tubes.
3. Measuring cylinder.
4. Thermometers.
5. A small volume of Hydrochloric acid.
6. Magnesium.
7. Magnesium Carbonate.
8. Magnesium Oxide.
9. Universal Indicator.
10. U.I Chart
Key factors
The key factors in this experiment are:
* Volume- The volume of the Hydrochloric Acid could change the
effect of the base, this is because to neutralise the acid you may
need a small amount of acid or there may not be enough base
particles to neutralise all the acid particles. This is also an
easy factor to change.
* Temperature- The temperature can effect the amount of neutralising
goes on, however this is a factor that is not possible to change
as it may depend on how much neutralising goes on, or vice-versa.
* Amount of base- This is also an easy factor to change, and its
principles lie exactly as the key factor "Volume" does.
* Neutralising time-The time it takes to neutralise the acid is hard
to experiment with however, one way of doing it would be to start
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
First, the freezing point depression of magnesium chloride was found. To begin, an ice bath was created in a 600 mL beaker filled with ice provided in the laboratory and rock salt. Next, Four different solutions with concentrations of 0.0 g (control), 0.2 g, 0.4 g, and 0.6g of magnesium chloride and 15 mL of deionized water were created. Each solution was made in a 100 mL beaker. The solutions containing magnesium chloride were stirred with a glass rod until the salt was completely dissolved. All equipment was cleaned with deionized water to minimize cross contamination. To calculate the freezing point, a Vernier temperature probe provided in the laboratory was used. The temperature probe was plugged into the GoLink!
The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction with Magnesium Aim: To investigate the effect of concentration of hydrochloric acid on the rate of reaction with magnesium Prediction: As the concentration of the hydrochloric acid increases, so will the rate of reaction Hypothesis: In a reaction, particles of two different reactants react together to form a product. The reaction only takes place on account of two things, if the particles collide, and if the collision has enough 'activation energy'. The two reactant particles, in this case magnesium particles and hydrochloric acid particles, must collide with each other on the correct 'collision course'. If this does not occur then no chemical reaction will take place. The reaction must also have enough energy, this can be affected by temperature, the more heat the particles have the faster they move and so the more energy therefore more chance of successful collisions.
ΔH2 released only 74.24 kilojoules of energy per mole, which is half when compared to the 144.79 kilojoules per mole that was released when the first and third reaction was summated. Although the algebraic sum of equation of 1 and equation 3 is equation 2, and the summated change in enthalpy per mole are drastically different, appearing to contradict Hess’s Law, this conclusion changes once limiting reagents are considered.
will result in an increase in the speed of the rate of reaction it has
Investigate how the concentration of hydrochloric acid effects the rate at which it reacts with calcium carbonate
Investigating Factors that Affect the Amount of Heat Produced in Neutralisation I am going to investigate factors that affect the amount of heat
The Arrhenius equation ln k = ln A – (Ea / RT) can be shown
Neutralization Experiment AIM:- To investigate how heat is given out in neutralizing sodium hydroxide (NaOH) using different concentrations of Hydrochloric Acid. Background Information:- Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl), Sulphuric acid (H2SO4) etc.
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
the acid was at 14 C the magnesium took 141 seconds to react and 27 C
Overall this experiment was a success yielding 98.8% of the initial 1.34g of known compounds. Looking at Table 1 the problem of separation quickly becomes apparent, both M-Toluic Acid and Acetanilide are insoluble in water. This left two non-salts in one mixture, and what solvent to use to separate these two was the most important question as their respective melting points are also very similar. After looking at both compounds and noticing the M-Toluic Acid (Image 2) had an OH group hanging off of it next to a double bond, the H ion on the end would be susceptible to a base. But further investigation showed the large number of hydrogen atoms hanging off the Acetanilide (Image 3) and it was thought that the NaHCO3 would be strong enough to rip the Acetanilide apart.
1. The labels have fallen off of three bottles thought to contain hydrochloric acid, or sodium chloride solution, or sodium hydroxide solution. Describe a simple experiment which would allow you to determine which bottle contains which solution.
Investigating the Effects of Temperature on the Rate of Reaction between Magnesium and Hydrochloric Acid
Preparation of Ethanol and Ethanoic Acid Introduction to report ---------------------- This report contains 5 practical experiments to produce ethanoic acid from ethanol. The first practical is the preparation of ethanol from glucose using yeast during the process of fermentation; this has been demonstrated in class. In this practical the glucose is converted into ethanol and carbon dioxide by respiratory enzymes from the yeast. The ethanol solution will be between 5-15% and the ethanol will be separated from the yeast by filtering.