6.4: Data Analysis
- Page ID
- 374947
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As always, fill out the cover page of your Google Workbook
Solutions
The material in light brown represents data or values you used in making the solutions (like the concentration of a reagent you diluted, and the volume you diluted it to). The stuff in blue represents calculations you do with the data. Some of these you will use in other sheets of this workbook.
Figure \(\PageIndex{1}\): Solutions worksheet of the acid equilibrium workbook. (Bob Belford CC-0)Remember, you can use formulas in worksheets. For example you wish to find the initial volume of concentrated acetic acid from the dilution formula. So you know that
\[M_iV_i=M_fV_f\] and can solve for the volume you need with the spreadsheet, and then use that volume in the lab. So in the cell B4 you can type
=(Z1*Z2)/Z3
where Z1, Z2 and Z3 are the cells of your sheet that have the data you wish to use in your calculation.
Data Analysis
Once again, you can use functions or work the data up by hand.
Figure \(\PageIndex{1}\): Copy and Paste Caption here. (Copyright; author via source)- Row 2 for solutions 1-4 are the molarities of the solutions created in the solutions worksheet (you can cut and paste values).
- Row 3 has the pH values for each of the solutions you measured and recorded in your data sheet.
- Calculate hydronium ion concentration from pH (weak acid equilibria above).
- For solutions 1-3
- Calculate acetate ion concentration from hydronium ion concentration (Table \(\PageIndex{3}\) above)
- Calculate undissociated acid concentration at equilibrium from the initial concentration and the extent of reaction (Table \(\PageIndex{3}\) above)
- Calculate Ka from equilibrium acid, hydronium and acetate concentrations
- Calculate percent ionization from initial acid concentration and extent of reaction (x) in (Table \(\PageIndex{3}\)
- For solution 4 insert values but calculate Ka from just the pH measurement (see eq. 6.2.13)
- The unknown is acetic acid and you are using the pH meter to determine its concentration. Use the average Ka from the four solutions you prepared.