Standardisation Of Sodium Hydroxide Lab Report
Standardisation of a Solution of Sodium Hydroxide:
Introduction:
In a lot of cases it isn’t possible to prepare a solution by accurate weighing of the solute, dissolving in water and diluting to volume. There are many possible reasons for this, but in the case of sodium hydroxide, the solid absorbs moisture from the air, and also reacts with carbon dioxide from the air. In that case, it cannot be accurately weighed in air.
In an experiment like this, a solution of the approximate required concentration was prepared. Afterwards, the exact concentration was determined by titration against a solution whose concentration can be calculated accurately from careful weighing. This experiment included a standard solution, which according to Lewis, R. and Evans, W. 2011, “is a solution of known concentrations”. They also stated that “the procedure in finding the concentration of a solution is called volumetric analysis. It involves reacting a solution …show more content…
Burette and Conical flask measuring the solution. (Aus-e-Tute, 2014)
Discussion: (from email but may have to edit it)
According to Yeow, X., 2011, “the main reaction in the series of acid-base titration is neutralization. As all the reactants are colourless, an appropriate indicator must be added to indicate the colour change at the end point”. In this case, the indicator was phenolphthalein solution. WHAT IS THE COLOR CHANGE AND HOW DID YOU FIND IT
What effect would each of the errors described below have on the concentration of the potassium hydrogen phthalate:
- Some of the solid potassium hydrogen phthalate was spilled in making the transfer
- Not enough water was added to bring the volume up to the mark
These errors would affect the overall results of the experiment.
What effect would each of the errors described below have on the calculated value of the concentration of sodium hydroxide:
- The burette is not rinsed with sodium hydroxide
- The tip of the burette is not filled before titration
Introduction:
In a lot of cases it isn’t possible to prepare a solution by accurate weighing of the solute, dissolving in water and diluting to volume. There are many possible reasons for this, but in the case of sodium hydroxide, the solid absorbs moisture from the air, and also reacts with carbon dioxide from the air. In that case, it cannot be accurately weighed in air.
In an experiment like this, a solution of the approximate required concentration was prepared. Afterwards, the exact concentration was determined by titration against a solution whose concentration can be calculated accurately from careful weighing. This experiment included a standard solution, which according to Lewis, R. and Evans, W. 2011, “is a solution of known concentrations”. They also stated that “the procedure in finding the concentration of a solution is called volumetric analysis. It involves reacting a solution …show more content…
Burette and Conical flask measuring the solution. (Aus-e-Tute, 2014)
Discussion: (from email but may have to edit it)
According to Yeow, X., 2011, “the main reaction in the series of acid-base titration is neutralization. As all the reactants are colourless, an appropriate indicator must be added to indicate the colour change at the end point”. In this case, the indicator was phenolphthalein solution. WHAT IS THE COLOR CHANGE AND HOW DID YOU FIND IT
What effect would each of the errors described below have on the concentration of the potassium hydrogen phthalate:
- Some of the solid potassium hydrogen phthalate was spilled in making the transfer
- Not enough water was added to bring the volume up to the mark
These errors would affect the overall results of the experiment.
What effect would each of the errors described below have on the calculated value of the concentration of sodium hydroxide:
- The burette is not rinsed with sodium hydroxide
- The tip of the burette is not filled before titration