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Chapter 16, Problem 16.69QP

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CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

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Chapter
Section
FindFindarrow_forward

CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933
Interpretation Introduction

Interpretation:

The pH of a 0.30-M solution of a weak base is 10.66 at 25oC. The Kb of the given base has to be calculated.

Concept Information:

Strong base and weak base:

Strong base dissociates into its constituent ions fully. It produces more of hydroxide ions while dissolved in water.  Weak bases partially dissociates into its constituent ions.

According to Bronsted-Lowry, strong base is a good proton acceptor whereas weak base is a poor proton acceptor

Since, the ionization of a weak base is incomplete; it is treated in the same way as the ionization of a weak acid.

The ionization of a weak base B is given by the below equation.

B(aq)+H2O(l)HB+(aq)+OH-(aq)

The equilibrium expression for the ionization of weak base B will be,

Kb=[HB+][OH-][B]

Where,

Kb is base ionization constant,

[OH] is concentration of hydroxide ion

[HB+] is concentration of conjugate acid

[B] is concentration of the base

pOH definition:

The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion [OH-] concentration. pOH scale is analogous to pH scale.

pOH=-log[OH-]

Relationship between pH and pOH

pOH is similar to pH.  The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH, the concentration of hydronium ion is used.

The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation,

pH+pOH=14,at25oC

As pOH and pH are opposite scale, the total of both has to be equal to 14.

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