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Chapter 9: Q13P (page 208)

Barbituric acid dissociates as follows:

(b)Calculate the pH and fraction of dissociation of 10-10.00 M barbituric acid.

Short Answer

Expert verified

The pHof10-10.00Mis7

The fraction of disassociation is 99.9%

Step by step solution

01

Step 1 : Definition of pH.

pH is defined as a quantitative measure of acidity and basicity. Compounds having pH more than 7 is acidic in nature while when shown above than 7 is basic in nature. When pH comes 7 , compound is said to be neutral.

02

Step 2 : Calculate pH and fraction of dissociation.

Since the solution is highly diluted, we can consider thatpH=7H+=10-7.

We will calculate the fraction of dissociation by:

Ka=H+A-HAA-=KaH+脳HA=9.8脳10-510-7脳HAA-=980HA

03

Step 3 : Calculate fraction of dissociation.

Now, using the same reaction, we will find fraction of dissociation:

a=A-HA+A-=980HAHA+980HA=980/981=99.9%

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Most popular questions from this chapter

When is a weak acid weak and when is a weak acid strong? Show that the weak acid 99%dissociatedrole="math" localid="1654854665468" F=(0.0102)Ka will be 92%dissociated when dissolved in water if the formal concentration is one-tenth (F=Ka/10)of Show that the fraction of dissociation is 27%whenF=10Ka. At what formal concentration will the acid be 99%dissociatedCompare your answer with the left -hand curve in Figure 9-2

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