The pH Scale and Acid-Base Indicators

Secondary 3-4

The pH Scale

Secondary 3

  • The pH, short for potential of hydrogen, is a measure used to determine the acidity, neutrality or basicity (alkalinity) of a solution. The pH has no unit of measurement.

  • The pH scale is used to compare the acidity, neutrality or basicity (alkalinity) of solutions. The pH scale generally ranges from 0 to 14.

On the pH scale, 0 is the most acidic value, 7 is neutral and 14 is the most basic, or alkaline, value.

Acidic substances have pH values below 7. A pH value of 7 indicates a neutral substance. Basic, or alkaline, substances have pH values above 7.

Secondary 4

An aqueous solution always contains hydrogen ions |(\text{H}^+)| and hydroxide ions |(\text{OH}^-).| The pH value of an aqueous solution depends on the concentration of the |(\text{H}^+)| ions relative to the concentration of the |(\text{OH}^-)| ions.

  • When the concentration of |(\text{H}^+)| ions is higher than the the concentration of |(\text{OH}^-)| ions, the pH is below 7 and the solution is acidic.

  • When the concentration of |(\text{H}^+)| ions is equal to the concentration of |(\text{OH}^-)| ions, the pH is 7 and the solution is neutral.

  • When the concentration of |(\text{H}^+)| ions is lower than the concentration of |(\text{OH}^-)| ions, the pH is above 7 and the solution is basic, or alkaline.

The pH scale can be used to assess the degree of acidity or basicity (alkalinity) of an aqueous solution.

  • An acid is a substance that allows the release of |\text{H}^+| ions in an aqueous solution.
  • A base is a substance that allows the release of |\text{OH}^-| ions in an aqueous solution. Basic substances are also often called alkaline.
  • The pH, short for potential of hydrogen, is a measure used to determine the acidity, neutrality or basicity (alkalinity) of a substance. The pH has no unit of measurement.
  • The pH scale is used to compare the acidity, neutrality or basicity (alkalinity) of substances. The pH scale generally ranges from 0 to 14.

On the pH scale, 0 is the most acidic value, 7 is neutral and 14 is the most basic, or alkaline, value. The following image illustrates the approximate pH values of some common substances.

The substances and their pH values are: battery acid pH 0, stomach acid pH 1, lemon juice pH 2, soft drink pH 3, tomato juice pH 4, coffee pH 5, milk pH 6, pure water pH 7, seawater pH 8, egg white pH 9, laundry detergent pH 10, hair styling product for permanent straightening pH 11, toilet cleaner pH 12, bleach pH 13, and drain cleaner pH 14.

Important!

A difference of one unit on the pH scale causes the acidity or basicity (alkalinity) of a solution to change by a factor of 10.

  • A decrease by one unit on the pH scale means that the acidity is increased by a factor of 10.

  • An increase of one unit on the pH scale means that the basicity (alkalinity) is increased by a factor of 10.

On the pH scale, a decrease of one unit means that the acidity is increased by a factor of 10, while an increase of one unit means that the basicity (alkalinity) is increased by a factor of 10.

Tomato juice (pH 4) is 1 unit below coffee (pH 5) on the pH scale. Therefore, tomato juice is 10 times more acidic than coffee.

Tomato juice (pH 4) is 2 units below milk (pH 6) on the pH scale. Therefore, tomato juice is 100 times more acidic than milk |(10\ \times 10=100).|

To go from a pH 5 to a pH 4, it takes one jump to the left on the pH scale. A change of one pH unit corresponds to a 10-fold change in acidity. To go from pH 6 to pH 4, it takes two jumps to the left on the pH scale. A change of two pH units corresponds to a 100-fold change in acidity.

The comparison of acidity of tomatoes, coffee and milk

Answer the following questions to compare laundry detergent (pH 10) and bleach (pH 13).

  1. Which of the two substances is more basic?

  2. What is the variation in basicity between the two substances?

See solution

The pH Scale

The pH Scale

Exercise

The Molar Concentration of H+ Ions and the pH (EST)

The pH of an aqueous solution can be used to determine the molar concentration of the |\text{H}^+| ions present. The following formula is used.

|[\text{H}^+]=10^\text{-pH}|
where
|[\text{H}^+]:| concentration of |\text{H}^+| ions in moles per litre |(\text{mol/L})|
|\text{pH}:| pH value

An aqueous solution of hydrochloric acid |(\text{HCl})| has a pH value of |2.5.| Here is the dissociation equation of hydrochloric acid in water.

||\text{HCl}_\text{(aq)}\rightarrow\text{H}^+_\text{(aq)}+\text{Cl}^-_\text{(aq)}||

What is the molar concentration of |\text{H}^+| ions in this solution?

See solution

Tip

Acid-Base Indicators

Acid-base indicators, commonly referred to as pH indicators, are substances that change colours depending on the pH.

Some of the application of acid-base indicators in laboratories are:

The following image shows the colours of acid-base indicators depending on the pH.

Bromothymol blue, thymol blue, methyl yellow, phenol red, methyl orange, bromocresol green, phenolphthalein and the universal indicator are acid-base indicators. The main colours obtained by acid-base indicators are red, orange, yellow, green, blue, pink and fuchsia.

The colour range of some acid-base indicators depending on the pH

Phenolphthalein is an indicator that can be used to determine if the solution is basic. When a few drops of phenolphthalein are added to the solution in question, a colour change may occur.

  • If phenolphthalein remains colourless, the solution is either acidic (pH below 7), neutral (pH 7), or basic (pH 7-8.2).

  • If the indicator turns pink, the solution is basic with a pH between 8.2 and 10.

  • If the indicator turns fuchsia, the solution is basic with a pH above 10.

In short, if phenolphthalein turns pink or fuchsia when mixed with a solution, the solution is definitely basic.

Phenolphthalein is colourless when the pH is between 0 and 8.2. It is pink when the pH is between 8.2 and 10 (transition interval) and fuchsia when the pH is above 10.

The phenolphthalein colour depending on the pH

A few drops of an acid-base indicator thymol blue are added to a test tube filled with lemon juice (pH 2). Thymol blue is thoroughly mixed with lemon juice and a colour change occurs.

Referring to the image The colour range of some acid-base indicators depending on the pH, determine the colour of thymol blue after it is mixed with lemon juice.

Using a dropper, a few drops of thymol blue are added into the test tube filled with lemon juice.

Adding thymol blue to lemon juice

See solution

A few drops of methyl yellow are added to an unidentified substance and the solution turns orange. In a second test tube, bromocresol green is added to the same unidentified substance and it turns green.

Referring to the image The colour range of some acid-base indicators depending on the pH, determine the pH interval of the unidentified substance.

The solution in Test Tube 1 is orange and the solution in Test Tube 2 is green.

The reaction of methyl yellow and bromocresol green with an unidentified substance

See solution

Exercise

Exercise

pH and the pH Scale

Science and Technology Secondary3-4