Titration Practical

Length: 1201 words (3.4 double-spaced pages)
Rating: Excellent
Open Document
- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - -

Text Preview

More ↓

Continue reading...

Open Document

Titration Practical

Planning assessment

The apparatus to be used:

· Beaker

· 250cm 3 volumetric flask

· Funnel

· Burette

· Pipette

· White tile

· Conical Flask

· Balance

· Spatula

· Weighing bottle

· Glass rod


Making a standard solution:

A weighing bottle was accurately weighed and approximately 5g of
anhydrous sodium carbonate was added and the weight of the bottle plus
the solid recorded. The anhydrous sodium carbonate was then
transferred into a 100cm3 clean beaker. The bottle was carefully
rinsed out two or three times with water and the washings were
transferred to the beaker each time. About 25cm3 of water was poured
into the beaker and stirred with a glass rod until the solid had
completely dissolved. This solution was then added to a 250cm3
volumetric flask using a funnel. The beaker and funnel were swilled
thoroughly using a small amount of water these washing were then added
to the volumetric flask. Water was then added to the volumetric flask
until it was about 1cm below the graduation mark. The water was then
added slowly from a clean pipette so that at eye level the bottom of
the meniscus was just touching the graduation mark. The volumetric
flask was then stoppered and then inverted.

Carrying out a titration:

A conical flask was swilled out with water and a pipette and pipette
filler were used to withdraw 25.0cm3 of the sodium carbonate solution
from the volumetric flask and transfer it to the conical flask. A
burette was first swilled with sulphuric (VI) acid using a clean, dry
beaker and a funnel and then filled to below the zero mark. A little
of the solution was then run out of the burette into the beaker and
the funnel removed. A white tile was then placed underneath the
conical flask and a few drops of the indicator methyl orange was added
to the sodium carbonate solution.

How to Cite this Page

MLA Citation:
"Titration Practical." 123HelpMe.com. 25 Jun 2017
Title Length Color Rating  
Essay on Assessed Practical Titration Write-Up - Assessed Practical Titration Write-Up Equation: Na2CO3 + H2SO4 à Na2SO4 + CO2 + H2O One mol of Na2CO3 reacts with one mol of H2SO4. Results: The weight of my sodium carbonate crystals was 2.67g and the results of the titrations are as follows: Rough 1st 2nd 3rd 4th 5th 6th Initial Reading 00.00 00.50 00.00 00.00 00.00 00.00 00.20 Final Reading 26.45 26.45 26.05 27.00 25.85 25.90 26.10 Titration 26.45 25.95 26.05 27.00 25.85 25.90 25.90 pH slightly acidic neutral slightly acidic slightly acidic slightly alkali neutral ne...   [tags: Papers] 564 words
(1.6 pages)
Strong Essays [preview]
Volumetric Analysis practical Essay examples - Volumetric Analysis Practical To determine the pH of commercially supplied 32% Hydrochloric acid solution. Investigative question Can the pH of an acid which is Hydrochloric acid be calculated by using titration with a standardized base solution of Sodium Hydroxide. Hypothesis That the pH of the hydrochloric acid solution can be calculated using titration with a standardised sodium hydroxide base solution as long as concentration and temperature of base solution remain constant. Variables Independent variable Volume of base (sodium hydroxide) needed to titrate the acid solution Dependant Variable Volume of acid (hydrochloric acid) placed in beaker to be titrated....   [tags: Hydrochlorica Acid Solution, pH Levels]
:: 3 Works Cited
1596 words
(4.6 pages)
Powerful Essays [preview]
Chemistry Practical Investigation-Volumetric Analysis Essay examples - ... Random errors are errors in measurement that lead to measured values being inconsistent. The word random indicates that they are unpredictable and have unexpected value even when the same instrument is used. If random error is present in this experiment it would be because of the variation of eye level on the meniscus solution to the making on the apparatus suck as volumetric flask, burette, pipette and so on. This ransom error can be reduced by repeating the experiment. Thus the precision is accurate because it is not affected by any random errors....   [tags: concordant titres, measurement, random errors] 738 words
(2.1 pages)
Research Papers [preview]
Practical Uses of Marijuana and Hemp Essays - Marijuana is a hot button topic in America today. The plant is looked down upon, usually as a harmful and useless drug. But this propaganda has been spread by the government and anti-legalization organizations for the past 20-25 years. In reality, marijuana legalization would have a positive impact on today’s society. The American people must look past the prevailing advertisements and publications degrading marijuana use and uncover its practical uses. George Washington once said to one of his servants at Mount Vernon, “Make the most of the hemp seed....   [tags: Marijuana, illegal, drugs, hemp, practical uses,] 1221 words
(3.5 pages)
Strong Essays [preview]
Essay on Chemistry: What is A Complexometric Titration - Introduction: According to (Khan): A complexometric titration as defined by IUPAC as a volumetric titration where a soluble complex can be formed by titrating a metal ion with a ligand in an aqueous solution and a titrant is one of the reacts used in the titration. [4] M(H2O)n + L = M(H2O)(n-1)L + H20 [4] (Khan): further states, here L are the Ligand and which is formed via the complete replacement of water molecules by other ligands can occur till the formation of the MLn complex. “n” is the coordination number of the metal ion and represents the maximum number of monodentate ligands which can be bound to it [8] Figure 1: The h...   [tags: metal ion, donor atom, molecules]
:: 17 Works Cited
1857 words
(5.3 pages)
Term Papers [preview]
Essay about Complexometric Titration - Complexometric titration is defined as a form of volumetric analysis in which the formation of a coloured complex is used to indicate the endpoint of the titration (1). Complexometric titrations rely on the formation of complexes between metal ions and compounds capable of donating electrons to form a stable, soluble complex (2). The complex is formed as a result of metal ions being titrated with a complexing agent or ligand. The principle of complexometric titrations is based on a simple ion being transformed into a complete ion and using a metal indicator to determine the endpoint (3), and the displacement of water from the solvation sphere of the metal ions by ligands (5)....   [tags: Pharmaceutical Chemistry ]
:: 5 Works Cited
3069 words
(8.8 pages)
Research Papers [preview]
Essay about Titration - Titration Titration is a laboratory technique by which we can use to determine the concentration of an unknown solution using a standard concentration of another solution that chemically reacts with the unknown. This standard solution is referred to as the "titrant". We have to have some way to determine when the reaction is complete so you add indicator to the unknown so you can see when the reaction is complete. This is referred to as the "end point" or more technically the equivalence point....   [tags: Papers] 499 words
(1.4 pages)
Strong Essays [preview]
Determination of Cu2+ by Titration Essay - Determination of Cu2+ by Titration Introduction: The purpose of this lab is to determine the concentration of copper ions in an unknown solution. Complexometric titration will be used to determine the concentration. A buret will be used to deliver the complexing agent to the unknown solution. Ethylenediaminetetraacetic acid will be used as the complexing reagent. An indicator, Murexide in our case, will be used to indicate the endpoint of the reaction. Theories and Concepts: The anion of the acid, EDTA4-, will complex to the metal....   [tags: Chemistry] 507 words
(1.4 pages)
Good Essays [preview]
Titration Investigation Essay - Titration Investigation Aim: The aim of my investigation is to determine the solubility of calcium Hydroxide solution with the aid of the titration process. Titration can be defined as the method of determining the concentration of a substance in solution by adding to it a standard reagent of known concentration in carefully measured amounts until a reaction of definite and known proportion is completed, as shown by a color change or by electrical measurement, and then calculating the unknown concentration....   [tags: Papers] 1338 words
(3.8 pages)
Strong Essays [preview]
Essay on Acid-Base Titration - 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. Using a concentration of .1 NaOH we had the largest NaOH volume before the largest pH increase at 6.38ml. For the largest NaOH volume after the largest pH increases we used 6.73ml of base....   [tags: Papers] 411 words
(1.2 pages)
Strong Essays [preview]

Related Searches

The amount of sulphuric (VI) acid in
the burette recorded by seeing at eye level what mark the bottom of
the meniscus touched to the nearest 0.05cm3. The sulphuric (VI) acid
was then added to the sodium carbonate solution in small volumes until
the sodium carbonate solution had turned orange. The amount of
sulphuric (VI) acid left in the burette was measured and the amount
added to the sodium carbonate was then recorded by subtracting the
final reading of the burette from the initial one. This was a rough
titration; more titrations were done until there were three volumes
which agreed to within 0.1cm3.


The funnel was removed from the burette before reading it as drops of
sulphuric (VI) acid could have fallen into the burette after the
reading was taken which would have made the readings inaccurate and
larger then it should have been. A white tile was placed underneath
the conical flask so that any colour changes could be observed more
clearly as the white would contrast with orange. The burette was read
at eye level to avoid any parallax errors, as this is where the best
view of the meniscus is, and from different angles the water can look
different. A rough titration was carried out to see how much of the
sulphuric (VI) acid was roughly needed to react with the hydrous
sodium carbonate. The conical flask was swilled as the solution from
the burette was added so that all of the solutions reacted with each
other. The burette and pipette were washed out with the solutions that
were to go in them before they were used to ensure that any other
substances are rinsed out and they are the only substances in the
glassware. If this was forgotten and the burette was not washed out
the reading would be inaccurate and larger then they should have been
as it would seem more sulphuric acid would be needed to neutralise the
sodium carbonate. The conical flask was swilled with water to get rid
of any impurities in the conical flask, the solution going into the
flask already contained water as a solvent so no new substances were
added. The solution was released from the burette drop by drop when
the end point was near to find the exact drop at which the sulphuric
(VI) acid stops reacting with the sodium carbonate solution. If it
were let out very quickly there would be a larger percentage error, as
the readings would have a large difference in values. The experiment
was repeated until concordant results were obtained so that reliable
and accurate readings were acquired. Approximately 5cm of the
anhydrous sodium carbonate was used as this was a logical amount; not
too much so that it would not completely dissolve, but not too little
so that only a small amount of the sulphuric (VI) acid would be needed
to neutralise it as a smaller reading gives a larger percentage error.
250cm3 standard solution of sodium carbonate was made so that the same
solution could be used when doing repeats because this ensures that
the concentration of the sodium carbonate solution used for each
titration is the same. 25.0cm3 of sodium carbonate was used for the
titration as this was a reasonable amount; enough to be able to stir
it and see a colour change, not too much so that large amounts of
sulphuric (VI) acid would be needed to neutralise it. Only a few drops
of the methyl orange indicator was added to the sodium carbonate
solution as if too little was added then the colour would be too faint
to see; but if too much was added the colour would be too deep for the
colour change to be seen clearly, which would lead to less accurate

Methyl Orange is a weak acid so just a small proportion of their
molecules ionise in aqueous solution. We can show this as an equation:





HIn represents the methyl orange which is a weak acid, and In– the ion
it forms when it ionises. HIn and In– have different colours: HIn is
red and In– is yellow. Because it is a weak acid it will be mostly in
the HIn form and therefore coloured red. But when added to the sodium
carbonate solution, this will react with the H+ ions and then more HIn
will ionise so as to replace them. So more In– will be formed and
eventually the indicator will appear yellow. This will show up when
the In– concentration is about 10 times greater than the HIn

The reaction is reversible, as we add the sulphuric (VI) acid from the
burette the neutralsation will occur but because the sulphuric acid is
a strong acid and sodium carbonate is a weak alkali the point of
neutralisation for such a titration will occur when the pH of the
solution is in the region of pH3.2 and pH4.4 which corresponds to the
pH range over which point the methyl orange changes colour from yellow
to orange, so it is appropiate to use this indicator

Risk assessment

As sodium carbonate is an irritant goggles and a lab coat must be worn
to prevent any irritation to the eyes or skin. Try not to inhale
vapours as sodium carbonate can irritate the respiratory system. If
swallowed drink plenty of water and seek medical attention. If
substance gets into eyes flood the eyes with gently running tap water
for 10 minutes and seek medical attention. If sodium carbonate
solution is spilt onto skin or clothes immediately remove contaminated
clothing and wash skin with plenty of water. Soak contaminated
clothing ands rinse repeatedly. If any of the substance is spilt in
the lab scoop up the solid and if any solution is spilt add mineral
absorbent and scoop into a bucket. Rinse the area of the spill and the
cloth or mop thoroughly. If methyl orange is swallowed immediately
wash out mouth, have a glass or two of water and seek medical
attention. If the indicator gets into the eyes flood eyes with gently
running tap water for 10 minutes and seek medical attention. If methyl
orange is spilt on skin or onto clothes remove contaminated items and
flood area with water and then wash thoroughly with soap and cold
water. If spilt in the lab, wash the area thoroughly. Sulphuric (VI)
acid is a corrosive and can cause burns to the skin so a lab coat must
be worn at all times. If swallowed, wash out mouth and have a glass or
two of water. Do not induce vomiting and seek medical attention as
soon as possible. If splashed into the eye flood eye with gently
running tap water for 10 minutes and seek medical attention. If the
acid is spilt onto skin or clothes remove the contaminated clothing
and quickly wipe as much liquid off the skin as possible with a dry
cloth before drenching the area with a large excess of water. If a
large area is affected or blistering occurs seek medical attention. If
spilt in the laboratory wear eye protection and gloves. Cover with
mineral absorbent and scoop it into a bucket. Add anhydrous sodium
carbonate over the mixture and leave to react, and then add lots of
cold water. Rinse the area of the spill several times with water.

Sources of information

AS Chemistry At Esher College Work Book 1 “The Elements of Life” and
“Developing Fuels”, pg. 4-5

Hazcards, Cards 98, 95 and 32


Return to 123HelpMe.com