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Chapter 9: Q8TY (page 203)

If, instead, mmol of strong base were generated, by how much would the pH of the original buffer rise?

Short Answer

Expert verified

The increment in the of the original buffer by $0.27 pH$ units

Step by step solution

01

Define The formula for Henderson- Hassel Balch equation

The Henderson- Hassel Balch equation for an acidic reaction can be given as,

$pH = {pK}_{3} + \log \frac{|A^{-}|}{[HA]}$

02

Step 2: Calculate the Ph of increment of buffer solution.

Given,

Moles of HA= $50 mmol$

Moles ofrole="math" localid="1654852922651" $A^{-} = 50 mmol$

Moles of strong base $= 15 mmol$

The moles of $HA = 50 + 15 = 65 mol$

The moles of $A^{-} = 50 - 35 = 15 mol$

$p H = p K_{3} + \log \frac{[m o l A^{-}]}{[m o l H A]} p H = p K_{3} + \log \frac{35 m o l}{65 m o l} p K_{3} - 0.27$

The increment in the of the original buffer by $0.27 p^{H}$ units.

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Most popular questions from this chapter

Show that the limiting fraction of association of a base in water, as the concentration of base approaches $0, is a = 10^{7} Kb / (1 + 10^{7} K_{b})$ Find the limiting value of $a$ for $K_{b} = 10^{- 4}$ and for $K_{b} = 10^{- 10}$

What is the pH of a solution prepared by dissolving $1.23 g$ of

2-nitrophenol (FM 139.11) in 0.250 L?

Barbituric acid dissociates as follows:

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

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.

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

See all solutions

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