Is Atomic Size the Key Factor in Determining Acidity Levels?

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The discussion centers on the acidity of two acids, HX and HZ, where X is smaller than Z. It is initially assumed that HX would be more stable due to X's higher charge density, leading to the expectation that HX would be more acidic. However, the teaching assistant clarifies that HZ is actually more acidic. This is attributed to the stability of the conjugate base; larger anions, like Z-, are more stable than smaller ones, which favors the dissociation of HZ into H+ and Z-. The comparison of acidity among HF, HCl, HBr, and HI supports this conclusion, demonstrating that larger anions correlate with increased acidity.
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Suppose I have two acids HX and HZ. Say X is smaller then Z in atomic size. So then one would think that HX would be a more stable molecule then HZ since X has a higher charge density then Z (Both have same electronegativity) . HZ being a weaker molecule would dissociate more rapidly. Now my TA says that due to this HZ is more acidic then HX. Is this correct?
 
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Pretty much. Compare the acidity of HF, HCl, HBr and HI.
 
Correct. Acidity is a related to the stability of the conjugate base. A larger anion is more stable on its own than a small one, so the equilibrium favors the dissociated H+ and Z-.
 

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