pH meter is an instrument used to measure acidity or alkalinity of a solution - also know as pH. pH is the unit of measure that describes the degree of acidity or alkalinity. It is measured on a scale of 0 to 14.
The quantitative information provided by the pH value expresses the degree of the activity of an acid or base in terms of hydrogen ion activity. The pH value of a substance is directly related to the ratio of the hydrogen ion [H+] and the hydroxyl ion [OH-] concentrations. If the H+ concentration is greater than OH-, the material is acidic; i.e., the pH value is less than 7. If the OH- concentration is greater than H+, the material is basic, with a pH value greater than 7. If equal amounts of H+ and OH- ions are present, the material is neutral, with a pH of 7. Acids and bases have free hydrogen and hydroxyl ions, respectively. The relationship between hydrogen ions and hydroxyl ions in a given solution is constant for a given set of conditions, either one can be determined by knowing the other.
Learn more about pH meters
A rough indication of pH can be obtained using pH papers or indicators, which change color as the pH level varies. These indicators have limitations on their accuracy, and can be difficult to interpret correctly in colored or murky samples.
More accurate pH measurements are obtained with a pH meter. A pH measurement system consists of three parts: a pH measuring electrode, a reference electrode, and a high input impedance meter. The pH electrode can be thought of as a battery, with a voltage that varies with the pH of the measured solution. The pH measuring electrode is a hydrogen ion sensitive glass bulb, with a millivolt output that varies with the changes in the relative hydrogen ion concentration inside and outside of the bulb. The reference electrode output does not vary with the activity of the hydrogen ion. The pH electrode has very high internal resistance, making the voltage change with pH difficult to measure. The input impedance of the pH meter and leakage resistances are therefore important factors. The pH meter is basically a high impedance amplifier that accurately measures the minute electrode voltages and displays the results directly in pH units on either an analog or digital display. In some cases, voltages can also be read for special applications or for use with ion-selective or Oxidation-Reduction Potential (ORP) electrodes.
pH electrode technology has not changed much in the past 50 to 60 years. With all the technological advancements of the last 30 to 40 years, pH electrode manufacturing remains an art. The special glass body of the electrode is blown to its configuration by glass blowers. Not a terribly advanced nor “high tech” process but a very critical and important step in the electrode manufacturing. In fact, the thickness of the glass determines its resistance and affects its output.
Temperature compensation is contained within the instrument, because pH electrodes and measurements are temperature sensitive. The temperature compensation may be either manual or automatic. With manual compensation, a separate temperature measurement is required, and the pH meter manual compensation control can be set with the approximate temperature value. With automatic temperature compensation (ATC), the signal from a separate temperature probe is fed into the pH meter, so that it can accurately determine pH value of the sample at that temperature.
Buffers are solutions that have constant pH values and the ability to resist changes in that pH level. They are used to calibrate the pH measurement system (electrode and meter). There can be small differences between the output of one electrode and another, as well as changes in the output of electrodes over time. Therefore, the system must be periodically calibrated. Buffers are available with a wide range of pH values, and they come in both premixed liquid form or as convenient dry powder capsules. Most pH meters require calibration at several specific pH values. One calibration is usually performed near the isopotential point (the signal produced by an electrode at pH 7 is 0 mV at 25°C), and a second is typically performed at either pH 4 or pH 10. It is best to select a buffer as close as possible to the actual pH value of the sample to be measured.
Frequently Asked Questions
Effects of Temperature on pH
Temperatures Above 25°C: temperature compensation lowers high pH and raises low pH, resulting in value closer to neutral. Temperatures Below 25°C: temperature compensation raises high pH (more basic) and lowers low pH (more acidic), resulting in values further away from neutral. Whether or not temperature compensation needs be used is a matter of the needed pH accuracy. For example, if the accuracy requirement is ±0.1 pH, at a pH of 6 and a temperature of 45°C (113°F), the error is 0.06, well within the accuracy requirements. On the other hand, with the same ±0.1 pH accuracy requirement, operating at pH 10 and 55°C (131°F) would give an error of 0.27 pH and compensation should be used.
When compensation is required, it can be done in one of two ways. If the temperature fluctuates, then an automatic compensator should be used. If the temperature is constant within several degrees C, then a manual compensator can be used. If no compensator is needed, a fixed resistor can be installed across the temperature compensator terminals. Any of the above devices–automatic compensation, manual compensation or fixed resistor–operate as a function of the pH meter’s electronic circuit. As such, information and parts should be obtained from the meter manufacturer. If automatic compensators are used, they should always be at the same location as the pH electrode. When electrodes are calibrated in buffer, the temperature compensator also should be in the buffer. In a similar way, a manual temperature compensator should be adjusted to reflect the temperature to which the pH electrode is exposed during both calibration and operation.
Challenges of pH Measurement Applications
No pH complications are created equal. The list below illustrates the types of problems that you can expect when measuring pH and how to handle them.
1. Instrumentation is frequently the source of disturbance for pH systems, through repeatability error, measurement noise, or valve hysteresis.
2. In-line pH loops will oscillate, regardless of controller modes and tuning, if setpoints are on the steep parts of the titration curves.
3. pH electrode submersion assemblies with unencapsulated terminations below the liquid surface will eventually have wet terminations.
4. Reagent control valves that are not close-coupled to the injection point on in-line systems will cause reagent delivery delays large enough to describe the tools of your trade n words that may seem foreign.
5. You need either a flow meter or a seer to diagnose reagent delivery problems.
6. Flow feedforward signals should be multiplied by pH controller outputs and employed to operate reagent valves directly or to establish reagent flow control setpoints.
7. Transportation delays to pH electrodes in analyzer houses will exceed mixing deadlines - such that increasing comfort in checking the electrodes is offset by decreasing comfort in checking trend recordings.
8. Injection electrodes should be preferred to sample holder assemblies whenever possible to reduce maintenance problems and improve response times - but not all injection electrodes are created equal.
9. Large tanks are fine if you don't have to control them; use the volume upstream to reduce reagent consumption or downstream to reduce control error. If you can't make-up your mind where to use one, put it downstream.
10. Install one or three but never two electrodes for a pH measurement.
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