pH Calculator

Material pH Value Acid or Base?
Hydrochloric Acid (HCl) 0.0 Acid
Battery Acid (H2SO4 sulfuric acid) 1.0 Acid
Gastric juice 1.2 Acid
Lemon Juice or Lime 2.2 Acid
Vinegar 2.8 Acid
Apples 3.0 Acid
Soft drinks 3.0 Acid
Wine and Beer 4.0 Acid
Tomatoes 4.5 Acid
Black coffee 5.0 Acid
Human saliva 6.4 Acid
Rain water 6.5 Acid
Milk 6.8 Acid
Pure water (H2O) 7.0 Neutral
Human Blood 7.4 Base
Tears 7.4 Base
Egg 7.8 Base
Baking Soda (Sodium Bicarbonate) 8.3 Base
Milk of Magnesia 10.5 Base
Ammonia (NH3) 11.0 Base
Lime (Calcium Hydroxide) 12.4 Base
Sodium Hydroxide (NaOH) 14.0 Base
Oven Cleaner 13.8 Base

Math plays an extremely important role in the concepts of the natural sciences, especially physics and chemistry. In order to understand the underlying principles behind these disciplines, a science student must have a certain level of mathematical skill. Speaking of chemistry, the branch of physical chemistry describes chemical properties using mathematical computations and theories of physics. Physical chemists also use mathematical statistics and analysis to learn more about chemical compounds and reactions.

One such important concept of physical chemistry is the pH of chemical solutions. Once known only among scientists, this term has now become so widely used that even a layman is likely to have come across it somewhere or the other. The concept of pH plays a very important role not only in the natural sciences like chemistry and biology, but in our everyday lives as well. The chemical calculations required to find out the pH of an aqueous solution can be complicated and time-consuming. Therefore, we now have an excellent online pH calculator to help us with this.

Let us now take a look at the features of the pH calculator, along with a brief understanding of the concept of pH and pOH.

What is the pH Of a Solution?

In chemistry, pH (denoting the “power of hydrogen” or “potential of hydrogen”) is a scale used to measure the acidity or alkalinity of a given aqueous solution. Pure water (H 2 O) is a non-electrolyte, but at room temperature it contains a very small and equal amount (1.0 × 10 -7 M) of both hydronium (H + ) and hydroxyl or hydroxide (OH ) ions. Their concentrations are inversely proportional, as determined by the ionic product of water (K w ).

These concentrations play an important role in determining the properties of a solution, and the chemical behaviour of its solutes. If a solution contains an equal concentration of H + and OH ions, it is neutral . If it contains a greater concentration of H + ions, it is acidic in nature. And similarly, if it has a higher concentration of OH ions, it is basic in nature.

Quantities which span large orders of magnitude and are difficult to express in the standard form are often expressed conveniently on a logarithmic scale. The pH scale is one such widely used scale is based on the p-function, as shown below:

pH = -log [H 3 O + ]

Here, “log” is the base-10 logarithm and “[H 3 O + ]” is the molar concentration of hydronium ions in the solution (H + ions tend to exist in combination with water molecules, rather than freely in solution). We can obtain the hydronium ion concentration by taking the antilogarithm of the above equation, as shown below:

[H 3 O + ] = 10 -pH

Similarly, the hydroxide ion concentration is expressed as the pOH of the solution:

pOH = -log [OH ] or [OH ]=10 -pOH

Based on the equilibrium concentrations of H + and OH in water, the given relationships hold true for any aqueous solution at 25 o C:

pH = −log[H 3 O + ] = −log(1.0 × 10 −7 ) = 7.00

pOH = −log[OH ] = −log(1.0 × 10 −7 ) = 7.00

Kw = [H 3 O + ][OH ]

−logK w = −log([H 3 O + ][OH ]) = −log[H 3 O + ] + −log[OH ]

pK w = pH + pOH = 14

It is important to remember that at temperatures above 25 o C, the molarity of H + and OH ions increases due to an increase in the dissociation of water molecules, leading to an overall lowering in the pH scale. The reverse holds true for temperatures lower than 25 o C. The pH scale plays a very important role in chemistry, biology, medicine, pharmacy, agronomy, water treatment, and even our daily lives.

What is the pH Calculator, and what are its advantages?

As described above, measuring the pH of a solution involves some complicated calculations involving logarithms and antilogarithms. These can be time-consuming and quite vulnerable to human errors. The pH scale is highly sensitive, and even a small calculation mistake can lead to a vast difference. For example, the change of a couple of decimal points in the pH of the blood can potentially kill a person. Similarly, minute differences in the pH can lead to a drug getting inactivated or an enzyme getting denatured.

Therefore, accuracy is extremely important when calculating the pH of a solution. The pH calculator is a helpful online tool designed for this very purpose. It can calculate the pH of a solution in a fast and error-free manner, displaying the result within a few seconds. You do not need to have any prior knowledge of the concerned calculations to use this tool. The pH calculator is programmed with a reliable algorithm to measure the pH with pinpoint precision.

How to Use the pH Calculator?

You can easily measure the pH of a solution using the pH calculator by following the steps given below:

  • Open the calculator and enter the name of the chemical solution and its concentration value in the corresponding input fields.
  • Click the “Calculate” button.
  • Soon, the calculated pH value will be shown in a fresh popup window.

The pH calculator is highly recommended to students, teachers, and professionals alike, particularly in situations where limited time is available for calculations.

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