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Chapter 11: Q71P (page 263)

Titrating nicotine with strong acid.Prepare a spreadsheet to reproduce the lower curve in Figure 11-4.

Short Answer

Expert verified

The spreadsheet developed is shown below

Step by step solution

01

Information given

Titration of 10.0 mL of 0.100 M nicotine (pKb1 = 6.15, pKb2 = 10.85) with 0.100 M HCl.

As nicotine is a weak base the reaction here will be in between weak base with strong acid.

02

Equation need to be used to develop spreadsheet

Fromtable 11.5 the equation for the fraction of titration of weak base with strong acid. is as follows

ϕ=CaVaCbVb=αBH++2αBH2++H+-OH-Cb1-H+-OH-Ca

Other formulas need to be used

H+=10-pHOH-=KwH+αBH2+=H+2H+2+H+K1+K1K2αBH+=H+K1H+2+H+K1+K1K2

03

Spreadsheet

Spreadsheet developed

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Most popular questions from this chapter

Select indicators from Table 11-3 that would be useful for the titrations in Figures11-1and11-2and theρK2=8curve in Figure11-3. Select a different indicator for each titration and state what color change you would use as the end point.

Calculate the pH at each of the following points in the titration of pH50.00mLof 0.0100MNaOH with 0.100MHCI . Volume of acid added: 0.00,1.00,2.00,3.00,4.00,4.50,4.90,4.99,5.00,5.01,5.10,5.50,6.00,8.00,and 10.00mL. Make a graph of pH versus volume of HCl added.

Titration on Diprotic Systems

11-30. This problem deals with the amino acid cysteine, which we will abbreviate H2C.

(a) A 0.0300Msolution was prepared by dissolving dipotassium cysteine, in water. Then of this solution were titrated with 0.0600MHCIO4. Calculate the pHat the first equivalence point.

(b) Calculate the quotient [C2-]/[HC-] in a solution of cysteinium bromide (the saltH3C+Br-).

The balance says that you have weighed out 1.023 g of tris to

standardize a solution of HCl. Use the buoyancy correction in Section 2-3 and the density in Table 11-4 to determine how many grams you have really weighed out. The volume of HCl required to react with the tris was 28.37 mL. Does the buoyancy correction introduce a random or a systematic error into the calculated molarity of HCl? What is the magnitude of the error expressed as a percentage? Is the calculated molarity of HCl higher or lower than the true molarity?

Finding the end point from pH measurements. Here are

data points around the second apparent end point in Figure 11-5:

(a) Prepare a spreadsheet or table analogous to Figure 11-6, showing

the first and second derivatives. Plot both derivatives versusvb

and locate the end point in each plot.

(b) Prepare a Gran plot analogous to Figure 11-8. Use the least-squares

procedure to find the best straight line and find the end point. You will

have to use your judgment as to which points lie on the “straight” line.
See all solutions

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