It is analytical topic

1. pH
pH is the measure of the concentration of hydrogen ions in a solution.
 pH is measured on a log scale.
pH = - log[H+]
 pH is used to indicate the degree of acidity or alkalinity (basic) of a solution in a polar solvent
like water.
 When there is a high [H+], the solution is more acidic but their value on pH scale is small.
 On the other hand when the [H+] concentration is low, the solution is basic but their value on pH
is high.

2. pH
 Pure water should have a neutral pH, due to have equal amounts of [H+] and [OH-].
 Acid and bases are created by adding polar molecules to water to increase [H+] or increase [OH-
] respectively.
 The pH scale ranges from 0 to 14. 0 being the most acidic and 14 being the most basic
 pH and pOH relate in the following way
pH + pOH = 14
 pOH is the measure of the [OH-], in a solution.
Q. What would be the pOH of an solution with a pH of 5.75?
pOH = 14 - 5.75
pOH = 8.25

3. pH
1. What is the pH of an HCl having 0.001 M conc.
2. Determine pH of a H2SO4 having 0.0001 M conc?
3. What is the pH of NaOH having 0.01 M NaOH.
4. Determine the pH of a 0.001 M HNO3?
5. What is the pH of a base with an [OH-] of 3.44X10-5 M?

4. pH
Ans:
3. 12.0
4. 3.0
5. 9.54

6. Co- Precipitation
It is a process in which more than one soluble compounds are precipitate out
from solution.
In precipitation normally water insoluble compounds precipitate.

8. Fractional Precipitation
 A process in which compounds, elements or ions of similar solubilities are
separate out by using different analytical techniques.

9. Fractional Precipitation
 https://www.youtube.com/watch?v=c80RnSmGRG4

10. Working of Indicators
 Please see your notes of 2nd semester