pH measurement
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Transcript of pH measurement
Need of pH measurement
• To produce products with defined properties
• To protect equipment
• For research and development
Basics about pH
• pH is the abbreviation of pondus hydrogenii
• pH = -log [H+]
• [H+] is in molar concentration
Basics about pH
In any aqueous solution
Kw = [H+] [OH-] = Dissociation constant
It depends on temperature
Acids
[H+] increases and [OH-] decreases
Bases
[OH-] increases and [H+] decreases
Electrochemical method
• Depends on hydrogen
activity in the solution
• It consists of two
electrodes
• 1. Measuring electrode
• 2. Reference electrode
Nernst Equation
• E=E0 + 2.3RT*log aH+
F
E0 = constant
R = the gas constant
T = temperature(k)
At 25˚C,slope=59.18mV/pH
• Comparing with standard formula for straight line
• Y= a+bx
a= offset
b= slope of the line
Reference electrode
• insensitive to the H+ ions in the solution
• most widely used is the silver/silver chloride electrode
• another commonly used reference electrode is the calomel electrode
Sodium Error
• Occurs at high pH
[H+] less than [Na+]
• Electrode respond to [Na+]
• Measured pH is lower than the actual pH
Liquid Junction Potential
• Equitransferent KCL is used as fill solution
• Different mobility of ions result in liquid junction potential
Diagnostics
• Glass pH Electrode Impedance
- normally in the range 0f 10-100 MΩ
- crack in glass electrode will result in short
• Reference Electrode Impedance
- Coating or blockage of the liquid junction will increase the result