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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 $pH of 10^{- 10.00} M is 7$

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 that $pH = 7 ([H^{+}] = 10^{- 7})$ .

We will calculate the fraction of dissociation by:

$K_{a} = \frac{[H^{+}] [A^{-}]}{[HA]} [A^{-}] = \frac{K_{a}}{[H^{+}]} 脳 [HA] = \frac{9.8 脳 10^{- 5}}{10^{- 7}} 脳 [HA] [A^{-}] = 980 [HA]$

03

Step 3 : Calculate fraction of dissociation.

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

$a = \frac{[A^{-}]}{[HA] + [A^{-}]} = \frac{980 [HA]}{[HA] + 980 [HA]} = 980 / 981 = 99.9 %$

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Most popular questions from this chapter

Which of the following acids would be most suitable for preparing a buffer of pH 3.10? (i) hydrogen peroxide; (ii) propanoic acid; (iii) cyanoacetic acid; (iv) 4-aminobenzenesulfonic acid.

(Without activities), calculate the pH of

(a) $1.0 脳 10^{- 8} MHBr$

(b) role="math" localid="1654840353627" $1.0 脳 10^{- 8} {MH}_{2} {SO}_{4}$ $(H_{2} {SO}_{4}$ dissociates completely to $2 H^{+}$ plus ${SO}_{4}^{2 -}$ at this low concentration).

Find the pH and concentrations of ${({CH}_{3})}_{3}$ Nand ${({CH}_{3})}_{3} {NH}^{+}$ in a 0.060M solution of trimethylamine.

Would you need $N a O H o r H C I$ to bring the pH of $0.0500 M$ HEPES (Table 9-2) to 7.45?

(b) Describe how to prepare $0.250 L o f 0.0500 M$ HEPES, $p H 7.45$ .

Find theand fraction of dissociation ( a ) of a $0.100 M$ solutionof the weak acid $HA$ with $Ka = 1.00 脳 10^{- 5}$

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