What does ph stand for?

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What does ph stand for?

The pH perpetually addressed as little p, big H. The pH of a substance is a sign that how many hydrogen ions it can produce in a specific volume of water. 

There’s no unblemished arrangement against what “pH” really stands for, however most people describe this as something like “power of hydrogen” or “potential of hydrogen.” 

The precise meaning 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 easier than it seems. Let’s unwrap it a little at a time. 

Assume you hold some liquid sloshing around in your aquarium and you need to know if it’s secure for those angelfish you require to grip. You prepare your pH meter and attach it to the “water” (It containsin a mixture of water with other substances suspended in it). 

If the water is highly acidic, there will be many fresh hydrogen ions and rarely any hydroxide ions. If the water is highly alkaline, the contrast will be true. Now if you hold a thimble-full of the water and it possesses a pH of 1 (it’s terribly, immediately, fish-killingly acidic), there will be one million times (10 to the power of 6, written 106) more extra hydrogen ions than there would be if the water remained neutral (neither acidic nor alkaline), including 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), therefore dividing the two provides us 106 (one million). There will be 10 million (1013) more hydrogen ions than if the h2O stayed remarkably alkaline, including a pH of 14. Perhaps you can begin to notice instantly were those strange pH numbers come from?

Assume we choose to develop a scale of acidity and begin it off at highly acidic and estimate that 1. When 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 by all these millions and billions and trillions is complex and crazy therefore we simply use a logarithm of the amount of hydrogen ions and connect to the strength of ten we receive in each circumstance. In different terms, the pH indicates directly looking at the (probably gigantic) amount of hydrogen ions, using the strength of 10, and eliminating the minus sign. That delivers us a pH of 1 for remarkably acidic, pH 7 for neutral, and pH 14 for remarkably alkaline. “Extremely alkaline” is a different method of responding amazingly weakly acidic.

pH definition

  • pH is a device used to measure the hydrogen ion concentration, a test of the acidity or alkalinity of a suspension.
  • The pH ranges normally from 0 to 14. 
  • Aqueous suspensions at 25°C with a pH smaller than 7 are acidic, while those by a pH higher than 7 are basic or alkaline. 
  • A pH level of 7.0 at 25°C is designated as “neutral” because the concentration of H3O+ matches the density of OH− in clear water.
  • Extremely active acids might possess a negative pH, while extremely strong bases might possess a pH higher than 14.

pH Calculation/Equation

The formula for determining pH was introduced in 1909 by Danish biochemist Søren Peter Lauritz Sørensen:

pH = -log[H+]


log is the base-10 logarithm and [H+] stands for the hydrogen ion intensity in units of moles per liter solution. 

The word “pH” originates from the German term “potenz,” which proposes “power,” combined with H, the element sign for hydrogen, so pH is an abstraction for “power of hydrogen.”

Examples of pH Values 

pH Values of Common Chemicals

hydrochloric acid 0
lemon juice 2.0
vinegar 2.2
wine 4.0
sodium hydroxide 14.0
pure water (neutral) 7.0
human blood 7.4
lye 13.0

pH values of living systems

Gastric acid 1.5-3.5
Lysosomes 4.5
Human skin 4.7
Granules of chromaffin cells 5.5
Urine 6.0
Cytosol 7.2
Blood (natural pH) 7.34–7.45
Cerebrospinal fluid (CSF) 7.5
Pancreas secretions 8.1
Mitochondrial matrix 7.5

pH in soil

Ultra acidic < 3.5
Extremely acidic 3.5–4.4
Very strongly acidic 4.5–5.0
Strongly acidic 5.1–5.5
Moderately acidic 5.6–6.0
Slightly acidic 6.1–6.5
Neutral 6.6–7.3
Slightly alkaline 7.4–7.8
Moderately alkaline 7.9–8.4
Strongly alkaline 8.5–9.0
Very strongly alkaline > 9.0

PH Meter Definition, Principle, Parts, Types, Application, Procedure.

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