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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

Calculate the quotient $[{HCO}_{2}^{-}] / [{HCO}_{2} H]$ at $pH 3.744$ if the ionic strength is $0.1 M$ by using the effective equilibrium constant listed for $μ = 0.1$ in Appendix G.

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

Find pH if $pKa = 3.00$ instead of $2.00$ Does the answer make sense?

Find the pH of 0.050 M sodium butanoate (the sodium salt ofbutanoic acid, also called butyric acid).

(a) Calculate the pH of a solution prepared by mixing $0.00100 mol$ of the base $B (K_{b} = 10^{- 2.00})$ with $0.0200 mol$ of ${BH}^{+} {Br}^{-}$ and diluting to $1.00 L$ .First calculate the pH by assuming $[B] = 0.0100$ and $[{BH}^{+}] = 0.0200 M$ . Compare this answer with the pH calculated without making such an assumption.

(b) After working part (a) by hand, use Excel Goal Seck to find the same answers.

See all solutions

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