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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.
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.
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.
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.
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).|
The comparison of acidity of tomatoes, coffee and milk
Answer the following questions to compare laundry detergent (pH 10) and bleach (pH 13).
Which of the two substances is more basic?
What is the variation in basicity between the two substances?
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?
When the concentration of |\text{H}^+| ions in a solution is expressed in scientific notation where the coefficient is 1, the pH of that solution can be determined by identifying the exponent.
|\bf[\text{H}^+]| in |\bf\text{mol/L}| | pH |
---|---|
|1\ \times\ 10^{-\color{#7CCA51}{1}}| | |\color{#7CCA51}1| |
|1\ \times\ 10^{-\color{#7CCA51}{2}}| | |\color{#7CCA51}2| |
|1\ \times\ 10^{-\color{#7CCA51}{3}}| | |\color{#7CCA51}3| |
|1\ \times\ 10^{-\color{#7CCA51}{4}}| | |\color{#7CCA51}4| |
|1\ \times\ 10^{-\color{#7CCA51}{5}}| | |\color{#7CCA51}5| |
|1\ \times\ 10^{-\color{#7CCA51}{6}}| | |\color{#7CCA51}6| |
|1\ \times\ 10^{-\color{#7CCA51}{7}}| | |\color{#7CCA51}7| |
|1\ \times\ 10^{-\color{#7CCA51}{8}}| | |\color{#7CCA51}8| |
|1\ \times\ 10^{-\color{#7CCA51}{9}}| | |\color{#7CCA51}9| |
|1\ \times\ 10^{-\color{#7CCA51}{10}}| | |\color{#7CCA51}{10}| |
|1\ \times\ 10^{-\color{#7CCA51}{11}}| | |\color{#7CCA51}{11}| |
|1\ \times\ 10^{-\color{#7CCA51}{12}}| | |\color{#7CCA51}{12}| |
|1\ \times\ 10^{-\color{#7CCA51}{13}}| | |\color{#7CCA51}{13}| |
|1\ \times\ 10^{-\color{#7CCA51}{14}}| | |\color{#7CCA51}{14}| |
This tip reflects the fact that the pH is a logarithmic function. To find out more about calculating the pH, you can consult the following concept sheet.
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:
To determine the acidity, neutrality or basicity (alkalinity) of a solution.
To determine the pH value of a solution.
The following image shows the colours of acid-base indicators depending on the pH.
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.
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.
Adding thymol blue to lemon juice
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 reaction of methyl yellow and bromocresol green with an unidentified substance