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Ghanshyam Padshala
146490305039
UI&CP
pH meter
Introduction
• •A pH meter is an electronic instrument used for
measuring the pH (acidity or alkalinity) of a liquid
(though special probes are sometimes used to
measure the pH of semi-solid substances). A
typical pH meter consists of special measuring
probes (a glass electrode and a reference
electrode) connected to an electronic meter that
measures and displays the pH reading.
History
• •The first commercial pH meter was built around
1936 by Radiometer in Denmark and by Arnold
Orville Beckman in the United States.
• Principle
• pH is defined as the negative logarithm of
hydrogen ion concentration.
• pH= -log [ H+ ]
• p = power
• H = hydrogen
• [H+] = hydrogen ion concentration
The pH of a solution can be measured by the pH
meter. The glass electrode is an half-cell and the
calomel electrode is another half-cell.
The pH scale
Table showing different pH
values
pH strips
• Litmus dye is a natural pH indicator. Litmus paper
is a small strip of paper that has dyes in it. When it
touches a base or a dye then the litmus paper
changes colors depending on, either it is a base or
it is an acid. If a litmus paper is exposed to an acid
it either changes its color to pink or red. If a strip
of litmus paper touches a base then the paper
changes to a shade of blue.
Construction of pH meter
Types of pH meter
Manual pH meter
Digital pH meter
Calibration
• •Calibration should be performed with at least
two standard buffer solutions that span the range
of pH values to be measured.
• •For general purposes buffers at pH 4 and pH 10
are acceptable.
• •The pH meter has one control (calibrate) to set
the meter reading equal to the value of the first
standard buffer and a second control (slope) which
is used to adjust the meter reading to the value of
the second buffer.
• •A third control allows the temperature to be set.
Conclusion
• •A pH meter is an electronic instrument used for
measuring the pH of liquid/semi • solid
substances. We exploited the properties of this
indicator to determine with precision the acidity or
alkalinity of various substances. pH meter is more
useful than the other pH indicators because it
gives accurate reading (e.g. , for detection of blood
pH ) and can measure the ph of a liquid as well as a
semi-solid substance.
Reference
• •Wilson Keith & Walker John, (2008), pH and
oxygen electrodes, Principles and Techniques of
Biochemistry and Molecular Biology, Cambridge
University Press, 6th edition. Pg. 18-23
• •Source
• 1.http://en.wikipedia.org/wiki/PH_meter
• 2.http://www.alliancets.com/site/files/408/29497
/109873/159912/Guide_to_pH_Measurement.pdf

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Ghanshyam padshala

  • 1. Ghanshyam Padshala 146490305039 UI&CP pH meter Introduction • •A pH meter is an electronic instrument used for measuring the pH (acidity or alkalinity) of a liquid (though special probes are sometimes used to measure the pH of semi-solid substances). A typical pH meter consists of special measuring probes (a glass electrode and a reference electrode) connected to an electronic meter that measures and displays the pH reading. History • •The first commercial pH meter was built around 1936 by Radiometer in Denmark and by Arnold Orville Beckman in the United States.
  • 2. • Principle • pH is defined as the negative logarithm of hydrogen ion concentration. • pH= -log [ H+ ] • p = power • H = hydrogen • [H+] = hydrogen ion concentration The pH of a solution can be measured by the pH meter. The glass electrode is an half-cell and the calomel electrode is another half-cell. The pH scale
  • 3.
  • 4. Table showing different pH values pH strips • Litmus dye is a natural pH indicator. Litmus paper is a small strip of paper that has dyes in it. When it touches a base or a dye then the litmus paper changes colors depending on, either it is a base or it is an acid. If a litmus paper is exposed to an acid it either changes its color to pink or red. If a strip
  • 5. of litmus paper touches a base then the paper changes to a shade of blue. Construction of pH meter
  • 6. Types of pH meter Manual pH meter Digital pH meter
  • 7. Calibration • •Calibration should be performed with at least two standard buffer solutions that span the range of pH values to be measured. • •For general purposes buffers at pH 4 and pH 10 are acceptable. • •The pH meter has one control (calibrate) to set the meter reading equal to the value of the first standard buffer and a second control (slope) which is used to adjust the meter reading to the value of the second buffer. • •A third control allows the temperature to be set.
  • 8. Conclusion • •A pH meter is an electronic instrument used for measuring the pH of liquid/semi • solid substances. We exploited the properties of this indicator to determine with precision the acidity or alkalinity of various substances. pH meter is more useful than the other pH indicators because it gives accurate reading (e.g. , for detection of blood pH ) and can measure the ph of a liquid as well as a semi-solid substance.
  • 9. Reference • •Wilson Keith & Walker John, (2008), pH and oxygen electrodes, Principles and Techniques of Biochemistry and Molecular Biology, Cambridge University Press, 6th edition. Pg. 18-23 • •Source • 1.http://en.wikipedia.org/wiki/PH_meter • 2.http://www.alliancets.com/site/files/408/29497 /109873/159912/Guide_to_pH_Measurement.pdf