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Chapter 11: Q37P (page 261)

Finding the End Point with Indicators 11 - 37. Why does a properly chosen indicator change color near the equivalence point in a titration?

Short Answer

Expert verified

The change of color should appear near the equivalence point, in other words in the center of the steep part of the titration curve.

Step by step solution

01

Indicators

  • When acidic or alkaline solutions are introduced to indicators, their color changes.
  • In the laboratory, markers like as litmus, phenolphthalein, and methyl orange are widely employed.
02

Determine the equivalence point in a titration

  • The properly chosen indicator changes color in the range of pH from pKHlnH-1 to pKHln+1and if the equivalence point is in in the given range of pH, the color of the indicator should change respectively.
  • Therefore, the change of color should appear near the equivalence point, in other words in the center of the steep part of the titration curve.

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Most popular questions from this chapter

11-22. The figure compares the titration of a monoprotic weak acid with a monoprotic weak base and the titration of a diprotic acid with a strong base.

(a) Write the reaction between the weak acid and the weak base and show that the equilibrium constant is 107.78. This large value means that the reaction goes "to completion" after each addition of the reagent.

(b) Why doespK2intersect the upper curve at 32Ve and the lower curve at 2Ve? On the lower curve, "pK2"is pKathe acid, BH+.


(a) Titration of 100mL of 0.050MH2A(pK1=2.86,pK2=10.64) with 0.050 M NaOH.

(b) Titration of 100mL of the weak acid localid="1663575238403" HA(0.050M,pKa=2.86) with the weak baselocalid="1663575247899" B(0.050M,pKb=3.36).

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?

Derive the following equation for the titration of potassium hydrogen phthalate (K+HP-) with NaOH:

蠒=CbVbCaVa=伪HP-+2伪P2--1-[H+]-[OH-]Ca1+[H+]-[OH-]Cb

Select indicators from Table 11-3 that would be useful for the titrations in Figures11-1and11-2and the蚁K2=8curve in Figure11-3. Select a different indicator for each titration and state what color change you would use as the end point.

Titration on Diprotic Systems

11-28 . A solution containing 0.100M glutamic acid (the molecule with no net charge) was titrated to its first equivalence point with0.0250MRbOH.

(a) Draw the structures of reactants and products.

(b) Calculate the at the first equivalence point.
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