by Chris Woodford. Last updated: April 29, 2015.
If it turns pink, it's acid I think—you probably learned that useful phrase once upon a time, along with the second half of the
same rhyme: "and if it turns blue, it's an alkali true." Measuring
acids and alkalis (bases) with litmus paper is something pretty much
everyone learns how to do in school. It's relatively easy to compare
your little strip of wet paper with the colors on a chart and figure
out how acidic or alkaline something is on what's called the
pH scale. But sometimes that's too crude a measurement. If you keep
tropical fish, for example, or you're a gardener with specimens that
like soil of a certain acidity or alkalinity, getting things wrong
with the litmus risks killing off your prized pets or your plants.
That's why many people invest in a meter that can measure pH
directly. What are pH meters and how do they work? Let's take a
Photo: US naval hospital technicians test a water sample for acidity, alkalinity, and chlorine levels. This sophisticated two-probe, digital meter is made by Hach. It can be hooked up to a computer with a USB cable to download data from its internal memory, which can store 500 measurements. Photo by Nick De La Cruz courtesy of Defense Imagery.
What is acidity?
If you're interested in measuring acidity, it helps if you know
what it is before you start! Most of us have only the faintest idea
what an acid or an alkali really is. We know it's a substance that
can "burn" our skin (though it's a chemical burn, not a heat
burn), but that's about it. What's even more confusing is that we can
safely eat some acidic things (lemons, for example, contain citric
acid) but not others (drinking a chemical like sulfuric acid would be
Photo: Some acids, such as lemon juice, are perfectly safe to handle;
others will burn your skin and can do painful, permanent damage.
Acids and alkalis are simply chemicals that dissolve in water to
form ions (atoms with too many or too few electrons). An acid
dissolves in water to form positively charged hydrogen ions (H+),
with a strong acid forming more hydrogen ions than a weak one. An
alkali (or base) dissolves in water to form negatively charged
hydroxide ions (OH−). Again, stronger alkalis (which can burn you as
much as strong acids) form more of those ions than weaker ones.
What does pH actually mean?
The pH (always written little p, big H) of a substance is an
indication of how many hydrogen ions it forms in a certain volume of
water. There's no absolute agreement on what "pH" actually stands
for, but most people define it as something like "power of
hydrogen" or "potential of hydrogen." Now this is where it gets
confusing for those of you who don't like math. The proper definition
of pH is that it's minus the logarithm of the hydrogen ion
activity in a solution (or, if you prefer, the logarithm of the reciprocal of the
hydrogen ion activity in a solution). Gulp. What
does that mean?
It's simpler than it sounds. Let's unpick it a bit at a time.
Suppose you have some liquid sloshing about in your aquarium and you
want to know if it's safe for those angelfish you want to keep. You
get your pH meter and stick it into the "water" (which in reality
is a mixture of water with other things dissolved in it). If the
water is very acidic, there will be lots of active hydrogen ions and
hardly any hydroxide ions. If the water is very alkaline, the
opposite will be true. Now if you have a thimble-full of the water
and it has a pH of 1 (it's unbelievably, instantly, fish-killingly
acidic), there will be one million times (10 to the power of 6, written 106) more hydrogen ions
than there would be if the water were neutral (neither acidic nor
alkaline), with a pH of 7. That's because a pH of 1 means 101 (which is just 10),
and a pH of 7 means 107 (10 million), so dividing the two gives us 106 (one million).
There will be 10 million million (1013)
more hydrogen ions than if the water were extremely alkaline, with a
pH of 14. Maybe you can start to see now where those mysterious pH
numbers come from?
Photo: The pH scale relates directly to the concentration of hydrogen ions in a solution, but not
in a simple linear way. The relationship is what we call a "negative exponential": the higher the pH (lower the acidity), the fewer the hydrogen ions—but there are vastly fewer ions at high pH than at low pH.
Suppose we decide to invent a scale of acidity and start it off at
very acidic and call that 1. Then something neutral will have far fewer
(one millionth or 10−6 times as many hydrogen ions) and
something alkaline will have fewer still (that's one 10 trillionth,
or one 10 million millionth, or 10−13 times as many). Dealing with
all these millions and billions and trillions is confusing and daft
so we just take a logarithm of the number of hydrogen ions and refer
to the power of ten we get in each case. In other words, the pH means
simply looking at the (probably gigantic) number of hydrogen ions,
taking the power of 10, and removing the minus sign. That gives us a
pH of 1 for extremely acidic, pH 7 for neutral, and pH 14 for
extremely alkaline. "Extremely alkaline" is another way of saying
incredibly weakly acidic.
How does a pH meter work?
If you're using litmus paper, none of this matters. The basic idea
is that the paper turns a slightly different color in solutions
between pH 1 and 14 and, by comparing your paper to a color chart,
you can simply read off the acidity or alkalinity without worrying
how many hydrogen ions there are. But a pH meter somehow has to
measure the concentration of hydrogen ions. How does it do it?
An acidic solution has far more positively charged hydrogen ions
in it than an alkaline one, so it has greater potential to
produce an electric current in a certain situation—in other words,
it's a bit like a battery that can produce a greater voltage. A pH
meter takes advantage of this and works like a voltmeter: it measures
the voltage (electrical potential) produced by the solution whose acidity we're
interested in, compares it with the voltage of a known solution, and uses the difference
in voltage (the "potential difference") between them to deduce the difference
What's it made of?
A typical pH meter has two basic components: the meter itself,
which can be a moving-coil meter (one with a pointer that moves against a scale) or
a digital meter (one with a numeric display), and either one or two probes that you insert into
the solution you're testing. To make electricity flow through something, you have to create a complete electrical circuit;
so, to make electricity flow through the test solution, you have to put two electrodes (electrical terminals) into it.
If your pH meter has two probes (like the one in the photo at the top of this
article), each one is a separate electrode; if you have only one probe, both of the two
electrodes are built inside it for simplicity and convenience.
The electrodes aren't like normal electrodes (simple pieces of metal wire); each one
is a mini chemical set in its own right. The electrode that does the
most important job, which is called the glass electrode, has a
silver-based electrical wire suspended in a solution of potassium
chloride, contained inside a thin bulb (or membrane) made from a special
glass containing metal salts (typically compounds of sodium
and calcium). The other electrode is called the reference electrode and has a potassium chloride wire
suspended in a solution of potassium chloride.
Artwork: Key parts of a pH meter: (1) Solution being tested; (2) Glass electrode, consisting of (3) a thin layer of silica glass containing metal salts, inside which there is a potassium chloride solution (4) and an internal electrode (5) made from silver/silver chloride. (6) Hydrogen ions formed in the test solution interact with the outer surface of the glass. (7) Hydrogen ions formed in the potassium chloride solution interact with the inside surface of the glass. (8) The meter measures the difference in voltage between the two sides of the glass and converts this "potential difference" into a pH reading. (9) Reference electrode acts as a baseline or reference for the measurement—or you can think of it as simply completing the circuit.
How does it work?
The potassium chloride inside the glass electrode (shown here colored orange)
is a neutral solution with a pH of 7, so it contains a certain amount of hydrogen ions (H+). Suppose the unknown solution you're testing (blue) is much more acidic, so it contains a lot more hydrogen ions.
What the glass electrode does is to measure the difference in pH between the orange solution
and the blue solution by measuring the difference in the voltages their hydrogen ions produce.
Since we know the pH of the orange solution (7), we can figure out the pH of the blue solution.
How does it all work? When you dip the two electrodes into the blue test solution, some of the hydrogen ions move toward the outer surface of the glass electrode and replace some of the metal ions inside it, while some of the metal ions move from the glass electrode into the blue solution. This ion-swapping process is called ion exchange, and it's the key to how
a glass electrode works. Ion-swapping also takes place on the inside surface of the glass electrode from the orange solution.
The two solutions on either side of the glass have different acidity, so
a different amount of ion-swapping takes place on the two sides of the glass.
This creates a different degree of hydrogen-ion activity on the two surfaces of the glass, which
means a different amount of electrical charge builds up on them.
This charge difference means a tiny voltage (sometimes called a potential difference, typically
a few tens or hundreds of millivolts) appears between the two sides of the glass, which
produces a difference in voltage between the silver electrode (5)
and the reference electrode (8) that shows up as a measurement on the meter.
Animation (above): How ion exchange works.
Although the meter is measuring voltage, what the pointer on the scale
(or digital display) actually shows us is a pH measurement.
The bigger the difference in voltage between the orange (inside) and blue (outside)
solutions, the bigger the difference in hydrogen ion activity between.
If there is more hydrogen ion activity in the blue solution, it's more acidic than the orange
solution and the meter shows this as a lower pH; in the same way, if there's less hydrogen ion
activity in the blue solution, the meter shows this as a higher pH (more alkaline).
Making accurate pH measurements
For pH meters to be accurate, they have to be properly calibrated
(the meter is accurately translating voltage measurements into pH
measurements), so they usually need testing and adjusting before you
start to use them. You calibrate a pH meter by dipping it into buffers
(test solutions of known pH) and adjust the meter accordingly.
Another important consideration is that pH measurements made this way
depend on temperature. Some meters have built-in thermometers and
automatically correct their own pH measurements as the temperature
changes; those are best if fluctuations in temperature are
likely to occur while you're making a number of different measurements. Alternatively, you can correct the pH measurement
yourself, or allow for it by calibrating your instrument and making
pH measurements at broadly the same temperature.
Who invented the pH meter?
Who do we have to thank for this clever stuff? First, Nobel-Prize winning German chemist Fritz Haber (1868–1934) and his student Zygmunt Klemensiewicz (1886–1963) developed the glass electrode idea in 1909.
The modern, electronic pH meter was invented about a quarter century later, around 1934/5, when American chemist Arnold Beckman (1900–2004) figured out how to hook up a glass electrode to an amplifier and voltmeter to make a much more sensitive instrument.
Photo: How do you measure the pH of soils on Mars? Simple! You build a pH meter into a robotic
space probe. The Mars Phoenix Lander space probe (left) used this built-in, mini chemical laboratory (right) to measure different aspects of the Martian soil, including acidity and metal concentrations. Photos by courtesy of NASA Jet Propulsion Laboratory (NASA-JPL).
Find out more
On this website
On other sites
- Acids and Bases: An Introduction by Anthony Carpi. A good simple introduction to what makes things acidic or alkaline and the concept of pH.
- Chemguide: British chemistry teacher and writer Jim Clarke has an excellent website packed with very good, clear explanations of school-level chemistry (ideal for ages 11–18), which will be useful to older readers too. There's a section all about acids and bases that will help you figure out pH and how to measure it.
- Lab Math by Dany Spencer Adams. CSHL Press, 2003. A basic guide to math and statistics, mainly aimed at biological scientists but also of interest to chemists. Covers everyday techniques such as calculating molarity, calibrating a micrometer, using a pH meter, etc.
- At the Bench: a Laboratory Navigator by Kathy Barker. CSHL Press, 2005. Another guide to basic lab techniques, data collection, statistics, and analysis, including how to set up experiments, keeping a lab notebook, and running experiments themselves.
- Chemical Technicians' Ready Reference Handbook by Gershon J. Shugar and Jack T. Ballinger. McGraw-Hill, 1996. A huge, detailed handbook packed with helpful material on everyday chemical procedures, including a short section on pH meters.
For much deeper technical detail, try some of the following:
- US Patent 2,058,761: Apparatus for testing acidity by Arnold O. Beckman and Henry E. Fracker, National Technical Laboratories, granted October 27, 1936. Beckman's patent (originally filed in October 1934) explains his glass-electrode pH meter in detail.
- US Patent 2,311,976: pH measurement and control device by Edwin D. Coleman, granted February 23, 1943. An alternative glass electrode pH meter.
- US Patent 3,219,556: Ion measurement apparatus and method by Edwin P. Arthur and John E. Leonard, Beckman Instruments, granted November 23, 1965. Describes an alternative method of ion measurement without using a glass electrode.
- US Patent 4,288,308: Continuous pH meter by Clifford C. Hach, Hach Chemical Company, granted September 8, 1981. A pH meter that can make continuous measurements over a long period of time.