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Properties of Acids and Bases | The Basics

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pH stands for “power of hydrogen”

The pH scale is a measure of the H⁺ ion concentration of a substance in water.

Explain qualitatively the pH range of 0 to 14

Below is a strip of Universal Indicator:

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Formation of carbonic acid

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Optimal functioning of myosin at pH 6

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Indicators are WEAK ACIDS which indicate the acidity/alkalinity of a substance by changing colour.

Examples:

Litmus

Universal indicator

Phenolphthalein

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Factors affecting electrical conductivity of a acid or alkali

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Factors affecting electrical conductivity of a acid or alkali

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How well a substance forms ions in solution, determines its conductivity.

Strong acids and alkalis ionize (almost) completely, therefore they have a large concentration of free ions in solution which makes them highly conductive.

Weak acids and alkalis ionize only partially, therefore have a low concentration of free ions in solution which gives them poor conductivity.

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PhET simulation of acids and bases pH with universal indicator
Click to Run

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Neutralization = The reaction of an acid with a base to produce a salt and water.

Acids release H+  into solution.

Bases release OH- into solution.

If we were to mix an acid and base together, the H⁺ ion would combine with the OH⁻ ion to produce the molecule H₂O.

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and other reactions

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GCSE Science Revision Chemistry "Three Reactions of Acids

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North Carolina School of Science and Mathematics

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Double Displacement Calcium Carbonate and HCl

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DEF OF TITRATION = A technique for determining the concentration of an acidic or basic solution. The solution with known concentration is added to the solution of unknown concentration in a very controlled way to neutralise it by forming a salt and water.

A salt = A substance in which the hydrogen of an acid has been replaced by a cation, e.g. NaCl