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| Summary |
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| Rate of a Reaction |
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| Rate of a reaction is defined as the speed at which the reactants are converted into products. |
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| Slow Reaction |
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| Slow reactions are reactions that can be measured in the laboratories. e.g., hydrolysis of ester |
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| Fast Reactions |
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| Fast reactions are generally ionic reactions. It is difficult to measure their rates. |
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| Reversible Reactions |
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| The reactions in which the products can react with one another under suitable conditions to give back the reactants are called reversible reactions. |
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| Irreversible Reactions |
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| The chemical reactions where the products do not combine to give the reactants are called irreversible reactions. |
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| Arrhenius Acid |
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| A substance which dissociates in aqueous solution to give hydrogen ions is an Arrhenius acid. |
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| Arrhenius Base |
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| A substance which dissociates in aqueous solution to give hydroxyl ions is called an Arrhenius base. |
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| Lewis Acid |
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| A substance which can accept a pair of electrons is termed Lewis acid. |
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| Lewis Base |
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| A substance which can donate a pair of electrons is called Lewis base. |
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| Bronsted-Lowry Acid |
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| A substance which can donate a proton is a Bronsted-Lowry acid. |
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| Bronsted-Lowry Base |
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| A substance that can accept a proton is a Bronsted-Lowry base. |
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| pH |
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| pH is the negative logarithm of H3O+ ion concentration in moles/litre |
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| pH of water = 7 at 298 K |
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| pH of acids = less than 7 |
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| pH of bases = greater than 7 |
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| Exothermic Reactions |
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| The chemical reactions which proceed with the evolution of heat energy DH = -ve. |
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| Endothermic Reactions |
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| The chemical reactions which proceed with the absorption of heat energy, DH = +ve. |
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