2. Unbeknownst to you a mistake was made and the stock solution was prepared at

Question

2. Unbeknownst to you a mistake was made and the stock solution was prepared at a concentration of 1 x 104 M (moles/), not 1 x 10 M. That is 10X too concentrated. You make dilutions assuming that the concentration on the stock bottle (1 x 10) is correct. How would this affect your unknown in terms of molar concentration? What would happern when you read these solutions on the spectrophotometer? What is incorrect with each dilution? What is the quickest, simplest way to correct this mistake and prepare the proper dilutions? 0 3. To prepare your standard curve you used the technique of "Least Squares" to calculate the line rather than fitting the line by hand to the data. What is the purpose of using this technique and what is the equation derived for the line? Why don't you use a ruler and move it for a best fit like you did in 7th grade? Note you can use Microsoft Excel for this step and it will plot a "trend line", similar to the Least Squares best fit line. However, you still need to do and show the calculations. Make a table of your data similar the lab manual. If you have Excel force the line through the 0,0 intercept how does the equation change?

Explanation / Answer

All the molar concentration would be10 tines more conctrated than the dilution which are made. i.e, a 10-3 M would actually be 10-2 M.

Since absorption is directly proportional to the concentration, the value of absorption obtained would decreased by a factor of 10.

Easch dilution is 10 times stronger than it is actually marked at.

The quickest and simplest way will be to re-dlitue the stock 10 times. That is dilute 10-5 marked stock 20 times, so it will become so in real.

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