Skip to main content
Ch.16 - Acids and Bases
Chapter 16, Problem 93

Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?

Verified Solution

Video duration:
0m:0s
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Weak Bases

Weak bases are substances that partially ionize in solution, establishing an equilibrium between the un-ionized base and its ions. Unlike strong bases, which completely dissociate, weak bases have a lower tendency to accept protons (H+), resulting in a less significant increase in pH. Understanding the behavior of weak bases is crucial for calculating their dissociation constants.
Recommended video:
Guided course
00:51
ICE Charts of Weak Bases

pH and pOH

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. The pH scale ranges from 0 to 14, with values below 7 being acidic, 7 neutral, and above 7 basic. The relationship between pH and pOH is given by the equation pH + pOH = 14, which is essential for determining the hydroxide ion concentration in basic solutions.
Recommended video:
Guided course
02:09
pH and pOH Calculations

Base Dissociation Constant (Kb)

The base dissociation constant (Kb) quantifies the strength of a weak base in solution, representing the equilibrium constant for its ionization. It is calculated using the concentrations of the products and reactants at equilibrium. For a weak base like morphine, Kb can be derived from the pH of the solution, allowing for the determination of its ionization extent and strength.
Recommended video:
Guided course
03:50
Characteristics of Ka and Kb