In terms of pKa, which acid will be stronger? How does pKa relate to pKb?

2 Answers
anor277
Jul 5, 2017

pH≡−log10[H3O+], and thus bases, and then weaker acids will have the NUMERICALLY higher pH........

Explanation:

For example 1, the weaker acid will have the higher pH.

For example 2, the weaker acid will have the higher pH; the acid whose Ka=8×10−6.

For example 3, the stronger BASE will have the SMALLER pKb, and thus the base with pKB=4.5 will give rise to the GREATER [HO−] conc..........

We recall (i) that pH=−log10[H3O+],

and that pOH=−log10[HO−].

And (ii) in aqueous solution under standard conditions, pH+pOH=14.......just as under these conditions pKa+pKb=14. The stronger the acid, the weaker the conjugate base, and vice versa.

David Drayer
Jul 5, 2017
  1. .1 M of a weak acid
    2 . Ka = 8×10−6
  2. pKb = 4.5

Explanation:

Acid have a low pH the stronger the acid the lower the pH.
Bases have a high pH the strong the base the higher the pH.

  1. The .1 Molar solution of weak acid will have a higher pH than a strong acid.

  2. The Ka of 10−6 will be a weaker acid than one with a Ka of 2×10−3 so have a higher pH.

  3. The pkb of 4.5 is stronger than than a base with a pkb of 6.5.
    so the pkb of 4.5 will have a higher pH.

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