1. How is acid strength defined? What dictates the strength of an acid? 2. Expla
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Question
1. How is acid strength defined? What dictates the strength of an acid? 2. Explain the trend in acid strength for a binary acid. Justify your answer. 3. Explain the trend in acid strength for an oxo acid. Justify your answer Explain the trend in acid strength for a carboxylic acid. Justify your answer 5. What is meant by the leveling effect of water? 6. Explain in your own words why HC(g) is named hydrogen chloride but HCI (aq) is referred to as hydrochloric acid. The leveling effect may help here. 7. What is meant by an amphoteric salt? 8. Compare and contrast the Bronsted-Lowery and Lewis acid/base theoriesExplanation / Answer
1. The acid strength is defined as the ability to loose proton. Thus a strong acid is one which completely ionized in water thus readily giving a proton. The strength of the acid depends on polarity of the H—A bond and the size of atom A.
2. The trend of binary acid’s strength depends on the H-A bond’s strength thus the weaker the bond is the stronger is the acid. In binary acid the hydrogen is combined with certain non metallic element.
When we see an example of HCl and HF we find that the HCl is strong acid and HF is weak acid. This is because H-F bond is more stronger than the HCl bond thus HF does not readily gives a proton.
3. Oxo acid are those acid which consist of hydrogen, oxygen, and another element. The strength of oxo acid depend on bond strength of the O-H bond in the acid and the stability of the conjugate base. Thus as the number of oxygen atom increased the acid strength increases. For example chlorous acid HClO2 has more acidic strength as compared to hypochlorous acid HClO.
4.The strength of the carboxylic acid is related to the stability of its conjugate base, the carboxylate anion. The carboxylic acid and the carboxylate anion are in equilibrium with one another, and the relative acidity of carboxylic acids depends upon the position of this equilibrium. Electron releasing groups also called +I effect, destabilise, by increasing the electron density around the carboxylate group, and make it less favourable for the carboxylic acid to lose a proton and hence makes it less acidic
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