Interpretation and Evaluation:
Rinsing Process: When performing a volumetric analysis all equipment to be used must be washed with deionised water. This is done in order to remove anything that contaminate your solution and have an effect on the results. It is important that deionised water is used and not regular tap water, this is because tap water could itself contains many unwanted impurities such salts, other solids and bacteria. If these were to contaminate the solutions to be used it would create a margin of error in your results. In analytic chemistry there are four main pieces of glassware used which must be cleaned carefully and appropriate
Burette
The burette is to first be cleaned with deionised water, this is to remove and contaminants …show more content…
This is required essential because the volumetric pipette is being used to transfer 20.0 mL of 1.00 molL-1 Sodium Hydroxide into an Erlenmeyer flask to be diluted. By rinsing it with water first it ensures that the sodium hydroxide wont react with anything in the volumetric pipette and be diluted. When creating the 200 mL of 0.100 molL-1 solution it is assumed the sodium hydroxide is 1.00 molL-1, with this information the amount of sodium hydroxide required is calculated. Hence if the sodium hydroxide is diluted before even making the solution it would mean that the solution would have a lower concentration then 0.100 molL-1 this would result in more solution being required to neutralise the ethanoic acid, ultimately meaning that a higher (%w/w) will be calculated then there actually is. The volumetric pipette also has to be cleaned with 1.00 molL-1 sodium hydroxide before the sodium hydroxide is actually pipetted into the Erlenmeyer flask, this is to flush out any deionised water that could be clinging to the walls of the volumetric pipette. This is done because if any water is left in the pipette it could dilute the sodium hydroxide before it is transferred into the Erlenmeyer flask meaning the concentration would no longer be known accurately. This would result in a greater concentration (%w/w) then there really …show more content…
The volumetric flask isn’t rinsed with the solution to be added to, this is because 20.0 mL of 1.00 molL-1 sodium hydroxide is to be added to it and then further topped up with distilled water. If there is sodium hydroxide adhering to the walls of the volumetric flask it would mean, there would be more the 20.0 mL once the solution is made resulting in a higher concentration then the expected 0.100 molL-1. This would affect the practical because a lower then should be titre value would be obtained resulting in the (%w/w) of ethanoic acid being less than it should be. Any left over deionised water is irrelevant because the Erlenmeyer flask has to be topped up with deionised water until the graduation line anyway after the 20.0 mL of standard solution was
Rinsing Process: When performing a volumetric analysis all equipment to be used must be washed with deionised water. This is done in order to remove anything that contaminate your solution and have an effect on the results. It is important that deionised water is used and not regular tap water, this is because tap water could itself contains many unwanted impurities such salts, other solids and bacteria. If these were to contaminate the solutions to be used it would create a margin of error in your results. In analytic chemistry there are four main pieces of glassware used which must be cleaned carefully and appropriate
Burette
The burette is to first be cleaned with deionised water, this is to remove and contaminants …show more content…
This is required essential because the volumetric pipette is being used to transfer 20.0 mL of 1.00 molL-1 Sodium Hydroxide into an Erlenmeyer flask to be diluted. By rinsing it with water first it ensures that the sodium hydroxide wont react with anything in the volumetric pipette and be diluted. When creating the 200 mL of 0.100 molL-1 solution it is assumed the sodium hydroxide is 1.00 molL-1, with this information the amount of sodium hydroxide required is calculated. Hence if the sodium hydroxide is diluted before even making the solution it would mean that the solution would have a lower concentration then 0.100 molL-1 this would result in more solution being required to neutralise the ethanoic acid, ultimately meaning that a higher (%w/w) will be calculated then there actually is. The volumetric pipette also has to be cleaned with 1.00 molL-1 sodium hydroxide before the sodium hydroxide is actually pipetted into the Erlenmeyer flask, this is to flush out any deionised water that could be clinging to the walls of the volumetric pipette. This is done because if any water is left in the pipette it could dilute the sodium hydroxide before it is transferred into the Erlenmeyer flask meaning the concentration would no longer be known accurately. This would result in a greater concentration (%w/w) then there really …show more content…
The volumetric flask isn’t rinsed with the solution to be added to, this is because 20.0 mL of 1.00 molL-1 sodium hydroxide is to be added to it and then further topped up with distilled water. If there is sodium hydroxide adhering to the walls of the volumetric flask it would mean, there would be more the 20.0 mL once the solution is made resulting in a higher concentration then the expected 0.100 molL-1. This would affect the practical because a lower then should be titre value would be obtained resulting in the (%w/w) of ethanoic acid being less than it should be. Any left over deionised water is irrelevant because the Erlenmeyer flask has to be topped up with deionised water until the graduation line anyway after the 20.0 mL of standard solution was