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Acid-Base Titration: Determining Unknown Acid or Base Concentration, Streszczenia z Chemia analityczna

Uniwersytet Łódzki (UL)Chemia analityczna

The concept of acid-base titration, a quantitative analysis technique used to determine the concentration of an acid or base by neutralizing it with a solution of known concentration. Key points include the use of indicators, the concept of equivalence point, and the process of setting up a titration. Common indicators and their applications are also discussed.

Typologia: Streszczenia

2018/2019

Załadowany 25.11.2019

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Acid-base titration
Learning Objective
•Compute the concentration of an unknown acid or base given its volume and the
volume and concentration of the standardized titrant.
Key Points
•An acid-base titration is a quantitative analysis of acids and bases; through this
process, an acid or base of known concentration neutralizes an acid or base of
unknown concentration.
•The titration progress can be monitored by visual indicators, pH electrodes, or
both.
•The reaction’s equivalence point is the point at which the titrant has exactly
neutralized the acid or base in the unknown analyte; if you know the volume
and concentration of the titrant at the equivalence point, you can calculate the
concentration of a base or acid in the unknown solution.
Terms
•acid-base titrationdetermines the concentration of an acid or base by exactly
neutralizing it with an acid or base of known concentration
•equivalence pointthe point at which an added titrant’s moles are stoichiometrically
equal to the moles of acid/base in the sample; the smallest amount of titrant needed to
fully neutralize or react with the analyte
•titrantthe standardized (known) solution (either an acid or a base) that is added during
titration
•analytethe unknown solution whose concentration is being determined in the titration
Setting up an Acid-Base Titration
An acid-base titration is an experimental procedure used to determined the unknown
concentration of an acid or base by precisely neutralizing it with an acid or base of known
concentration. This lets us quantitatively analyze the concentration of the unknown solution.
Acid-base titrations can also be used to quantify the purity of chemicals.
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A cid-base titration

Learning Objective

  • Compute the concentration of an unknown acid or base given its volume and the

volume and concentration of the standardized titrant.

Key Points

  • An acid-base titration is a quantitative analysis of acids and bases; through this

process, an acid or base of known concentration neutralizes an acid or base of

unknown concentration.

  • The titration progress can be monitored by visual indicators, pH electrodes, or

both.

  • The reaction’s equivalence point is the point at which the titrant has exactly

neutralized the acid or base in the unknown analyte; if you know the volume

and concentration of the titrant at the equivalence point, you can calculate the

concentration of a base or acid in the unknown solution.

Terms

  • acid-base titrationdetermines the concentration of an acid or base by exactly

neutralizing it with an acid or base of known concentration

  • equivalence pointthe point at which an added titrant’s moles are stoichiometrically

equal to the moles of acid/base in the sample; the smallest amount of titrant needed to

fully neutralize or react with the analyte

  • titrantthe standardized (known) solution (either an acid or a base) that is added during

titration

  • analytethe unknown solution whose concentration is being determined in the titration

Setting up an Acid-Base Titration

An acid-base titration is an experimental procedure used to determined the unknown

concentration of an acid or base by precisely neutralizing it with an acid or base of known

concentration. This lets us quantitatively analyze the concentration of the unknown solution.

Acid-base titrations can also be used to quantify the purity of chemicals.

Acid-base titration The solution in the flask contains an unknown number of equivalents of base (or acid). The burette is calibrated to show volume to the nearest 0.001 cm 3. It is filled with a solution of strong acid (or base) of known concentration. Small increments are added from the burette until, at the end point, one drop changes the indicator color permanently. (An indication of the approaching equivalence point is the appearance, and disappearance after stirring, of the color that the indicator assumes beyond neutralization.) At the equivalence point, the total amount of acid (or base) is recorded from the burette readings. The number of equivalents of acid and base must be equal at the equivalence point.

Alkalimetry, or alkimetry, is the specialized analytic use of acid-base titration to determine the

concentration of a basic (alkaline) substance; acidimetry, or acidometry, is the same concept

applied to an acidic substance.

Materials for a Titration Procedure

  • burette
  • white tile (used to see a color change in the solution)
  • pipette
  • pH indicator (the type depends on the reactants)
  • Erlenmeyer or conical flask
  • titrant (a standard solution of known concentration; a common example is aqueous sodium carbonate)
  • analyte, or titrand (the solution of unknown concentration) Equivalence Point Indicators

Before you begin the titration, you must choose a suitable pH indicator, preferably one that

will experience a color change (known as the “end point”) close to the reaction’s equivalence

Titration of a weak acid by a strong base The pH of a weak acid solution being titrated with a strong base solution can be found at each indicated point.

Titration Procedure

  1. Rinse the burette with the standard solution, the pipette with the unknown solution, and the conical flask with distilled water.
  2. Place an accurately measured volume of the analyte into the Erlenmeyer flask using the pipette, along with a few drops of indicator. Place the standardized solution into the burette, and indicate its initial volume in a lab notebook. At this stage, we want a rough estimate of the amount of known solution necessary to neutralize the unknown solution. Let the solution out of the burette until the indicator changes color, and record the value on the burette. This is the first titration and it is not very precise; it should be excluded from any calculations.
  3. Perform at least three more titrations, this time more accurately, taking into account where the end point will roughly occur. Record the initial and final readings on the burette, prior to starting the titration and at the end point, respectively. (Subtracting the initial volume from the final volume will yield the amount of titrant used to reach the endpoint.)
  4. The end point is reached when the indicator permanently changes color.