Nahco3 Hydrochloric Acid
Working out mean or average results
26.3+26.1+23.8= 76.2/3=25.4
The average ml of HCL needed in order to react for a colour change was 26.5ml.
NaHCo3+ HCl NaCl+H2O+Co2
Calculation:
25 ml 0.1 mole dm3
26.3+26.1+23.8= 76.2 ml
76.2÷3=25.4÷1000=0.025 volume
0.1x0.25ml=0.025 moles
0.025÷0.254=0.98 (Rounded up to one decimals places) =0.1 M
To begin with concentration I have choose three volumes form my results table which I have added them and then divided by three to get an average results.
Describe the stages you followed in collecting the primary data and any secondary data.
Titration Steps:
• Firstly we weighed the solid sample of sodium hydrogen carbonate with an accurate balance; then dissolved in distilled water up to 250ml to make a …show more content…
Used a pipette to measure accurately the volume of this solution. For example, 25cm3. Safety pipette filler will be used to draw solution into the pipette. then it will be emptied into a conical flask add three to four drops of an indicator of methyl orange solution to the conical flask and note it will show a colour change. After that record the initial reading of the burette and making sure that all your burette readings must be to an appropriate precision.
Titrate the contents of the conical flask by adding to it 0.100 mole dm3 hydrochloric acid from the burette. Add the solution slowly. Swire the flask gently to mix the contents at the end indicator turns as define red colour. This is the end point of the titration. Record the final burette reading in your table of result. Repeat the titration to obtain several sets of results or until you obtain two results which are concordant. You should always carry out at least three titrations. Record all of the results that you obtain. Calculate and record the average (mean) titre volume of hydrochloric acid solution. Remember …show more content…
From my results I can see that the accurate result was 0.98 and our estimated was 0.1M but I rounded up my answer to 1 decimal places to see so there was not that much of a difference. Overall my experiment went well because I have followed instruction and I archived my hypothesis because I calculate that the chemical will have more concentration because it is a hydrochloric acid which will react with a methyl orange indicator solution and cause colour change from yellow to pink in my experiment I could clearly see the change of the colour. Form my results table I can see that my results were close to 0.1M which means that I have used the accurate amount of standard solution in my experiment If I was to improve my experiment I could attempt to read the burette to the bottom or top of the meniscus by doing this it might give me accurate results for my experiment. Another way of improving my experiment could be that I use volumetric pipettes for measuring.
Calculate the maximum percentage error in the average titre value.
Percentage error = maximum error x 100% Value of
26.3+26.1+23.8= 76.2/3=25.4
The average ml of HCL needed in order to react for a colour change was 26.5ml.
NaHCo3+ HCl NaCl+H2O+Co2
Calculation:
25 ml 0.1 mole dm3
26.3+26.1+23.8= 76.2 ml
76.2÷3=25.4÷1000=0.025 volume
0.1x0.25ml=0.025 moles
0.025÷0.254=0.98 (Rounded up to one decimals places) =0.1 M
To begin with concentration I have choose three volumes form my results table which I have added them and then divided by three to get an average results.
Describe the stages you followed in collecting the primary data and any secondary data.
Titration Steps:
• Firstly we weighed the solid sample of sodium hydrogen carbonate with an accurate balance; then dissolved in distilled water up to 250ml to make a …show more content…
Used a pipette to measure accurately the volume of this solution. For example, 25cm3. Safety pipette filler will be used to draw solution into the pipette. then it will be emptied into a conical flask add three to four drops of an indicator of methyl orange solution to the conical flask and note it will show a colour change. After that record the initial reading of the burette and making sure that all your burette readings must be to an appropriate precision.
Titrate the contents of the conical flask by adding to it 0.100 mole dm3 hydrochloric acid from the burette. Add the solution slowly. Swire the flask gently to mix the contents at the end indicator turns as define red colour. This is the end point of the titration. Record the final burette reading in your table of result. Repeat the titration to obtain several sets of results or until you obtain two results which are concordant. You should always carry out at least three titrations. Record all of the results that you obtain. Calculate and record the average (mean) titre volume of hydrochloric acid solution. Remember …show more content…
From my results I can see that the accurate result was 0.98 and our estimated was 0.1M but I rounded up my answer to 1 decimal places to see so there was not that much of a difference. Overall my experiment went well because I have followed instruction and I archived my hypothesis because I calculate that the chemical will have more concentration because it is a hydrochloric acid which will react with a methyl orange indicator solution and cause colour change from yellow to pink in my experiment I could clearly see the change of the colour. Form my results table I can see that my results were close to 0.1M which means that I have used the accurate amount of standard solution in my experiment If I was to improve my experiment I could attempt to read the burette to the bottom or top of the meniscus by doing this it might give me accurate results for my experiment. Another way of improving my experiment could be that I use volumetric pipettes for measuring.
Calculate the maximum percentage error in the average titre value.
Percentage error = maximum error x 100% Value of