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the titration practical
titration chemistry lab
titration chemistry lab
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Recommended: the titration practical
Investigating the Concentrations of Unknown Acids
Aim
To find out each of the concentrations of the hydrochloric acids in
the Winchesters labelled A-E. This is going to be carries out by
titrating the acid with NaOH.
Equipment needed for this investigation
Pipette - 25ml
Burette
Phenolphthalein
Conical flask
Beaker
Funnel
Pipette filler
Clamp
NaOH - the known acid of 0.1M
HCl - the unknown concentration of acids
White tile
My predictions
I predict that the different acid solutions of the HCl will be less
than 0.1M because the Winchesters were topped up with water, which
would have obviously weakened the concentration of the acid making the
number of moles less than 0.1.
Safety precautions when doing the experiment:
v The equipment should be used carefully to prevent breakage of any
glass.
v The acids should be used carefully avoiding spillages and if any
acid came into contact it should be rinsed with water immediately to
prevent any irritation to the skin.
Planning
All the equipment is gathered together first and made sure that it is
clean and safe to use.
25ml of the unknown concentration of the HCl is measured using a
pipette and taken using a pipette filler, the liquid is then drained
into a clean conical flask. 3 drops of phenolphthalein indicator is
added to 25ml of HCl.
The burette is securely placed onto the clamp and the NaOH is poured
into the burette using a funnel and making sure that the tap at the
bottom is closed. The conical flask containing the HCl and
Phenolphthalein is placed on a white tile at the bottom end of the
burette.
The tap of the burette is opened to slowly release the NaOH while
swirling the conical flask to combine the two acids. The NaOH is
steadily added until the solution in the conical flask turns a pale
pink colour. If the solution stays the pale pink for up to 20 seconds
The pH of the analyte, in this case a strong acid like HCl, is plotted against the volume of the strong base, NaOH, that is being added. The titration of a strong acid with a strong base produces a titration curve as above.
Possible improvements: If the this task were to be repeated experiments could be conducted to clarify areas of doubt by simply repeating the experiment many times, using different pH levels. The experiment could be repeated multiple with same procedure to verify the results that were collected, to check if the results are reliable and to have more confidence with the conclusion. Another improvement that could be made is improving random errors. There are lists of random errors that we made; for example the measurement of glucose and yeast
From the experimental data, the [H+] decreases as the concentration of the HCl in each solution decreases. Since acids dissociate in water, the dilution of the acid’s concentration (Macid) will determine the number of free hydrogen ions in the solution, being that they are equal to each other when the -log is used. By changing the concentration of the HCl, the acid strength decreases, as shown in the change in pH, due to the presence of H+ ions as they break away from the original molecules of the acid. These free ions are in the form of hydronium ions, which shows in the decrease of the H+ in the table above.
Investigation to find out if changes in concentration of acid affect the rate of a chemical reaction
There are a few changes that should be made to the procedure so that the experiment could generate better results. More time should be allowed to dissolve the tablets as if they are not dissolved colour changes are harder to identify during the titration and also the results are less accurate. The acid used should also be more concentrated as a 0.5mol or 0.3mol would mean a smaller amount of acid would be required.
The sought to determine the effects of mixing various levels of acids and bases to see which combination would have the most explosive reaction, and measure the resulting pH levels. I did this by testing an assortment of different pH levels of acids and bases, mixing them together and measuring the results. Most of the experiments resulted in a pH neutral solution, except for the Sulfuric Acid and the Sodium Hydroxide. By far, the Sulfuric Acid was the most explosive, followed by the Citric and Acetic acid.
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.
every size of chip. By doing this I will find out if the rate of
As 10 mL of NaOH was added drop wise, the solution began to have a pink tint. The fuchsia color did not permanently stay until 9mL of NaOH was added. The pH indicator demonstrated when exactly the reaction has neutralized. Because an acid and a base reacted to form water and a salt, the reaction is a neutralization
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.
second test tube also add 6 mL of 0.1M HCl. Make a solution of 0.165
Compared to the 0.5 M hydrochloric acid that was less concentrated, the more concentrated 2 M hydrochloric acid c...
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.
Titration is a technological process in which a solution, known as a titrant, is slowly and carefully added from a burrette into a fixed volume of another solution (known as the sample). In an acid-base titration an acid neutralizes a base or vice versa. This process is maintained untill the reaction between the titrant and the sample (acid and the base) is judged to be complete. The reaction is judged to be complete when the endpoint is reached. An endpoint in a titration analysis is referred to as the point at which no more titrant is added due to an observable colour change of an indicator. Indicators can be used to find an endpoint because they change colour when the pH of a solution changes and an endpoint in a titration is an empirical approximation of the equivalence point, which is the point of major pH change in the titration sample due to the fact that equal chemical amounts of reactants have been combined at that point. All indicators have a pH range, which is the range of pH values at which the colour of the indicator changes. Thus
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).