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Chapter 10: QEE (page 230)

(c) Calculate the percentage in the major form at each pH.

Short Answer

Expert verified

When the pH is raised to 11, the dihydroxy benzene takes on two forms: one deprotonated and one protonated.

Step by step solution

01

Step 1: Define the term “predominant form”  

The term "predominant form" refers to the most stable form of matching molecules in a compound with the least amount of energy.

02

Calculate the pH

Given pH:

pH 9.00 pH 11.00

Secondary species:

66.5%

52.9%

The formula was used to compute the main form of the 伪H2Aand伪HA- When pH9.00

When the pH is raised to 11, the dihydroxy benzene is di-protonated, and the dihydroxy benzene is deprotonated and protonated.

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Most popular questions from this chapter

(a) Derive equations for 伪H3A,伪H2A,伪HA2-,伪A3-for a triprotic system.

(b) Calculate the values of these fractions for phosphoric acid at pH 7.00.

Calculate 伪H2A,伪HA-,伪A2- for cis-butenedioic acid at pH 1.00, 1.92, 6.00, 6.27 and 10.00.

Draw the structure of the predominant form of pyridoxal-

5-phosphate at pH 7.00

The diprotic acid H2Ahas pK1=4.00and pK2=8.00.

(a) At what pH is [H2A]= [HA-]?

(b) At what pH is [HA-]= [A2-]?

(c) Which is the principal species at pH 2.00: H2A,HA-or A2-?

(d) Which is the principal species at pH 6.00?

(e) Which is the principal species at pH 10.00?

(a) Which two of the following compounds would you mix to make a buffer of pH7.45: H3PO4(FM 98.00), NaH2PO4(FM 119.98), Na2HPO4(FM 141.96), and Na3PO4(FM 163.94)?

(b) If you wanted to prepare 1.00Lof buffer with a total phosphate concentration of 0.0500M, how many grams of each of the two selected compounds would you mix together?

(c) If you did what you calculated in part (b), you would not get a pH of exactly 7.45. Explain how you would really prepare this buffer in the lab.
See all solutions

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