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Chapter 9: Q9TY (page 206)

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

Short Answer

Expert verified

The $pH if pKa = 3.00$ then $3.07$

Step by step solution

01

Define the acid dissociation constant

The acid dissociation constant $K_{3}$ can be given as,localid="1654854432154" $K_{3} = \frac{[H^{-}] |A^{-}|}{[H A]}$

A weak acid is one that doesn't undergo completion

02

Step 2: Calculate the H+ ion for Ka.

The $H^{+}$ can be calculated from

$HA ◽ H^{+} + A^{-} {nK}_{a} K_{a} = \frac{[H^{+}] {IA}^{-}]}{[HA]} 10^{- 3.00} = \frac{(X) (0.0100 + X)}{(0.0100 - X)} X = 8.44 \times 10^{- 4} Now Ph . pH = - \log (8.44 \times 10^{- 4}) pH = 3.07$

Thus, The $pH if {pK}_{3} = 3.00$ then $3.07$

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Most popular questions from this chapter

How many milliliters of $0.246 {MHNO}_{3}$ should be added to $213 mL$ of $0.00666 M 2,$ -bipyridine to give a pH of $4.19$ ?

(Without activities), calculate the pH of

(a) $1.0 \times 10^{- 8} MHBr$

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

Explain how you would use a spreadsheet such as Figure 8-9 to find the and concentrations of all species if you know the values of the equilibrium constants and the formal concentration $F$

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.

Effect of ionic strength on ${pK}_{a} . K_{a}$ for the localid="1654774253353" $H_{2} {PO}_{4} / {HPO}_{4}^{2 ‐}$ buffer islocalid="1654774257371" $K_{a} = \frac{[{HPO}_{4}^{2 ‐}] [H^{+}] Y_{HP {O_{4}}^{2 ‐}} Y_{H^{+ +}}}{[H_{2} P {O_{4}}^{‐}] Y_{H_{2} P {O_{4}}^{‐}}} = 10^{‐ 7.20}$ If you mix a localid="1654774261368" $1 : 1$ mole ratio of localid="1654774264927" $H_{2} {PO}_{4}$ andlocalid="1654774269015" $H_{2} P {O_{4}}^{‐ 2}$ at 0 ionic strength, the is 7.20. Using activity coefficients from Tablelocalid="1654774273534" $8 ‐ 1$ calculate the pH of a localid="1654774278805" $1 : 1$ mixture of and localid="1654774317458" $HP {O_{4}}^{‐ 2}$ at an ionic strength of 0.10. Remember thatlocalid="1654774320706" $pH = - {logA}_{H^{+}} = - \log [H^{+}] Y_{H^{+}}$

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