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

14th Edition
Burdge
ISBN: 9781259327933

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FindFindarrow_forward

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

14th Edition
Burdge
ISBN: 9781259327933
Interpretation Introduction

Interpretation:

The pH values for 0.10-M solutions of NaOH and NH3 has to be compared and the difference between a strong base and a weak base has to be illustrated

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]

Strong and weak base can be determined based on their equilibrium constant Kb and pH

  • When the Kb is large, it indicates strong base
  • When the Kb is small, it indicates weak base
  • When the pH is higher, it indicates strong base
  • When the pH is lower, it indicates weak 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.

To Discuss: The pH values for 0.10-M solutions of NaOH and NH3 and the difference between a strong base and a weak base.

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