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Summary Grade 12 IEB Physical Science - Titrations Overview CA$8.05   Add to cart
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Summary Grade 12 IEB Physical Science - Titrations Overview
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  • Course
  • Physical Sciences
  • Institution
  • 12th Grade

This guide on titrations for Grade 12 IEB Physical Science includes acid-base titration methods, choosing indicators, calculating unknown concentrations, and interpreting titration curves. The document provides a structured approach to understanding equivalence points and performing titration calcu...

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  • November 1, 2024
  • 4
  • 2021/2022
  • Summary

Subjects

  • chem

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  • 12th Grade
  • Physical Sciences
  • 200
All documents for this subject (633)

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TanyaChigs

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Indicators:
Indicators are dyes which are added to a solution to determine e whether the solution is acidic, neutral or
basic. (changes colour according to the hydronium ion concentration in the solution in which they are
added)

Common indicators:
Indicators pH in which Colour when Colour when Recommended titration
colour changes acid is added base is added

Methyl Orange 3,1 - 4,4 Red Yellow Strong acid + weak base

Litmus 5,0 - 8,0 Red Blue Strong acid + strong base

Bromothymol Blue 6,0 - 7,6 Yellow Blue Strong acid + strong base

Phenolphthalein 8,3 - 10,0 Colourless Pink Weak acid + strong base



Acid-base Titrations:

Titration: A titration is a process used to determine the unknown concentration of an acid or a base

Why? The aim of a titration is to react an acid with a base until neither is in excess.

Equivalence Point: The point where amounts of acid and base have reacted so that neither is in excess.
( An indicator can be used to determine the equivalence point of a titration - the point where one stops a
titration [changes colours] is called the end point )

NaOH + HC1 > Nall +
12
example
:




mol of base and I mol of acd react completely so that only the product is left )
11
.




N.B. indicator must be chosen so that end point corresponds with equivalence point
‣ i.e if salt produce is neutral, indicator used must change colour at a pr around 7

Preforming a titration:

1. One burette is filled with a standard solution (known
concentration). Making up a standard solution
2. A second burette is filled with the solution of unknown
concentration. 1. Calculate the mass of solute needed:
3. A fixed volume of the solution of unknown am'3
> 9
-


mv
mol .




concentration is emptied into a clean conical flask. -
C =
- am3

4. A few drops of a suitable indicator are added to the
1
>9
- . mol



solution in the conical flask. 2. Measure out the mass of solute on a watch
5. The conical flask is placed on a white tile to allow glass
colour changes to be seen easily 3. Transfer all the solute to the volumetric flask
6. Run a small quantity of the standard solution out of and dissolve the solute.
the burette. Record the initial burette reading. 4. Fill the volumetric flask to its graduation mark.
7. The standard solution is slowly added to the solution Calculate the exact concentration of the
in the conical flask while the flask is swirled. When you solution, correct to three decimal digits.
get close to the endpoint add the standard solution
drop by drop.

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