Ionization Of Acids And Bases
Chapter Name : Equilibrium |
Sub Topic Code : 102_11_07_12_03 |
Topic Name : Ionization Of Acids And Bases |
|
Sub Topic Name : The Ph Scale |
|
Introduction
The pH of a solution
is defined as the negative logarithm to base 10 of the activity (aH+ )
of hydrogen
•
In dilute solutions (< 0.01 M), activity of
hydrogen ion (H+) is equal in magnitude to molarity represented by
[H+].
•
It should be noted that activity has no units and is
defined as:
aH+ = [H+] / mol L–1
Pre-Requisites:
Reaction, ionization,
water, acid, base
Activity:
Some foods are acidic in nature some are
basic,
Blood
pH is almost neutral
Real Life Question:
Why is water called
neutral?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
|---|---|
| Acid, base | Acid have pH less that 7 and base have pH greater than 7 |
Learning aids / Gadgets
| Gadgets | How it can be used |
|---|---|
| Litmus paper | Dip litmus paper in soapy water, normal water and observe the color |
Real life uses :
pH scale helps to
tell what is acidic and what is basic
Places to visit :
Kitchen, bathroom
Practical examples around us
| Examples | Explainations |
|---|---|
| Some foods are acidic in nature some are basic | Acidic – lime juice, Coffee - acidic |
What you learn in Theory:
The pH of a solution
is defined as the negative logarithm to base 10 of the activity (aH+ )
of hydrogen
•
In dilute solutions (< 0.01 M), activity of
hydrogen ion (H+) is equal in magnitude to molarity represented by
[H+].
•
It should be noted that activity has no units and is
defined as:
aH+ = [H+] / mol L–1
What you learn in Practice:
The pH of a solution
is defined as the negative logarithm to base 10 of the activity (aH+ )
of hydrogen
•
In dilute solutions (< 0.01 M), activity of
hydrogen ion (H+) is equal in magnitude to molarity represented by
[H+].
•
It should be noted that activity has no units and is
defined as:
aH+ = [H+] / mol L–1