Question

Determination of an equilibrium constant by usind a spectrophometer
1 procedure written in your own words.
2 write a reaction that might have occurred during the experiment.
3 Draw and label equipment set up used in the experiment

Answer 1

Ans - Procedure -

1.   Take a chart that provides the volumes of reactants needed to prepare the standard solutions. Notice that the concentration of the iron solution is much greater than that of the KSCN solution. This is to ensure that all of the KSCN is used up in the reaction. The concentration of the product will be determined from the volume and concentration of the KSCN used in each trial. (mostly given in lab files )

2. Turn on the spectrophotometer and permit it to warm up. Set the wavelength to 447 nm. Utilize a cuvet loaded with the 0.05 M HNO3 as the clear. Take after your educator's bearings to gauge the absorbance values for each of the arrangements arranged in

Step 1. Record every one of the qualities in your information table (you can take the concentration and wavelength accordingly )

3. Construct a calibration curve for the data collected in Step 2. Plot absorbance on the y-axis and concentration of [Fe(SCN)²⁺] on the x-axis. Draw a best-fit line though the data points. This graph will be used to determine the amount of product formed in the next step

4.Use a buret or pipet to measure the volumes of the reactants In the tble you will use or make . Note that this set of combinations uses the more dilute Fe(NO₃)₃ solution.

5. After the above mixes have been blended, examples ought to be filled clean cuvets. The absorbance of every arrangement ought to be measured and recorded in the information table. Utilizing your alignment chart, decide the grouping of [Fe(SCN)2+] for each of the trials.

6. From the centralization of [Fe(SCN)2+] delivered and the first groupings of the reactants, develop tables to decide the balance convergences of all species. Utilize these qualities to ascertain the balance consistent for every trial.