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

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

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

Short Answer

Step by step solution

Define the acid dissociation constant

Step 2: Calculate the H+ ion for Ka.

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

Short Answer

Step by step solution

Define the acid dissociation constant

Step 2: Calculate the H+ ion for Ka.

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Chemical Reactions

The Earths Atmosphere

Chemical Analysis

Ionic and Molecular Compounds

Making Measurements

Study anywhere. Anytime. Across all devices.

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