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This organic chemistry video tutorial provides a basic introduction into acids and bases. It explains the effect of electronegativity on acid strength as well as atomic size. It also explains the effect of hybridization, resonance stabilization of the conjugate base, and the inductive effect of an electron withdrawing group on acid strength.
What is Acid Strength?
Acid strength is the measure of the ability of the acid to lose its H+ ion.
It depends on several factors which we will discuss in the subsequent sections.
What are Strong and Weak Acids?
• A strong acid is the one that completely ionizes in a solution whereas, a weak acid only partially ionizes.
• Strong acids are corrosive in nature and cause severe burns when they come in contact with skin.
• But the weak acids are only mildly corrosive and are even present in our food and body.
• Hydrochloric acid and sulphuric acid are examples of the strong acid.
• Ethanoic acid, citric acid (present in citric fruits) and acetic acid (present in vinegar) are a few examples of weak acids.
Factors Determining Acid Strength
As already discussed different acids have different acid strengths. An acid having greater degree of dissociation behaves as a stronger acid. Now let us understand the factors on which strength of an acid depends. The degree of dissociation of an acid depends on the following two factors.
1. Strength of H-A bond
2. Polarity of H-A bond
In general weaker the strength of H-A bond, stronger is the acid. Similarly greater the polarity of H-A bond, stronger is the acid. Both these factors make the dissociation of acid molecules into H+ and A- easier thereby increasing the acidity.
It may be mentioned here that while comparing elements in the same group of the periodic table the strength of H-A bond is a more important factor in deciding the acidity than its polarity. As the size of A increases on descending a group, H-A bond strength decreases and therefore the acid strength increases. For example, the acid strengths of hydrides of group-17 elements increases in the order.
HF is less than HCl is less than HBr is less than HI
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