Titration is a general class of experiment where a known property of one solution is used to infer an unknown property of another solution. An acid-base titration is a method in titration that allows quantitative analysis of the concentration of an unknown acid or base solution. Acid-base titration involves neutralization reaction that occurs between acids and bases. Acid-base titration can be dividing into:
1. Strong acid versus strong base
2. Weak acid versus strong base
3. Weak base versus strong acid
The equipments that involve in titration are usually Burette, Pipette, Acid/Base Indicator, Erlenmeyer flask, Standard solution, and Solution of unknown concentration, White Tile or white paper used to see a color change in the solution.
The standard solution is the solution that the concentration is known and usually takes place in the burette and called as “titrant”. The solution of unknown concentration called “analyte” and take place in the Erlenmeyer.
Before we start doing acid-base titration, we should choose a suitable acid-base indicator. We use indicator to determine the endpoint of the reaction. An indicator for an acid-base titration is a weak acid or weak base that is highly colored. The indicator changes color when the endpoint is reached.
First, the burette should be rinsed with the standard solution and it should be filled to the top of its scale. You should rinse the pipette with the unknown solution, and the conical flask with distilled water.
Solution of unknown concentration in a known volume should be taken with pipette and placed in Erlenmeyer and add a small amount of acid-base indicator. The standard solution should then be allowed from the burette into the Erlenmeyer. Let the standard solution out of the burette until the indicator changes color than record the value on the burette. Perform three or more titration, record the readings on the burette and then average these at the endpoint.
1. Strong acid versus strong base
2. Weak acid versus strong base
3. Weak base versus strong acid
The equipments that involve in titration are usually Burette, Pipette, Acid/Base Indicator, Erlenmeyer flask, Standard solution, and Solution of unknown concentration, White Tile or white paper used to see a color change in the solution.
The standard solution is the solution that the concentration is known and usually takes place in the burette and called as “titrant”. The solution of unknown concentration called “analyte” and take place in the Erlenmeyer.
Before we start doing acid-base titration, we should choose a suitable acid-base indicator. We use indicator to determine the endpoint of the reaction. An indicator for an acid-base titration is a weak acid or weak base that is highly colored. The indicator changes color when the endpoint is reached.
First, the burette should be rinsed with the standard solution and it should be filled to the top of its scale. You should rinse the pipette with the unknown solution, and the conical flask with distilled water.
Solution of unknown concentration in a known volume should be taken with pipette and placed in Erlenmeyer and add a small amount of acid-base indicator. The standard solution should then be allowed from the burette into the Erlenmeyer. Let the standard solution out of the burette until the indicator changes color than record the value on the burette. Perform three or more titration, record the readings on the burette and then average these at the endpoint.
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