Write an equation to show the number of ions produced by tetraoxophosphate(v) acid on dissociation
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Answer:
Activity:
Take about 1 g solid NaCI in a clean and dry test tube and add some concentrated sulphuric acid to it. Fit a rubber cork with a small delivery tube in the mouth of the test tube. Concentrated sulphuric acid reacts with sodium chloride to form hydrogen chloride gas. The hydrogen chloride gas starts coming out of the open end of the glass tube.
Now, hold a 'dry' blue litmus paper in HCI gas. There is no change in colour of the 'dry' blue litmus paper. This shows that HCI gas does not behave as an acid in the absence of water. However, when we hold a 'moist' blue litmus paper turns red. This indicates that HCI gas shows acidic behaviour in the presence of water as hydrogen ions are formed.
This proves that acids produce ions only in aqueous solutions or in the presence of water.
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Hydrogen ion, strictly, the nucleus of a hydrogen atom separated from its accompanying electron. The hydrogen nucleus is made up of a particle carrying a unit positive electric charge, called a proton. The isolated hydrogen ion, represented by the symbol H+, is therefore customarily used to represent a proton. Because the bare nucleus can readily combine with other particles (electrons, atoms, and molecules), the isolated hydrogen ion can exist only in a nearly particle-free space (high vacuum) and in the gaseous state.
Related Topics: Acid–base reaction Proton Ion Hydronium ion
In common usage, the term hydrogen ion is used to refer to the hydrogen ion present in water solutions, in which it exists as the combined molecule H+·H2O.
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acid–base reaction: Hydrogen and hydroxide ions
…compounds that give rise to hydrogen ions (H+) in aqueous solution. It was also realized...
The formula H+·H2O is also commonly written as H3O+ and denotes the hydronium or oxonium ion. The amount of hydrogen ion present in a water solution is used as a measure of the acidity of a substance; the higher the concentration of hydrogen ion the more acidic the solution and the lower the pH. See also pH.
The Editors of Encyclopaedia Britannica
This article was most recently revised and updated by Adam Augustyn, Managing Editor, Reference Content.
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