Using your knowledge of how molecular structure can influence acid strength, explain the following statements.H3AsO4 is a stronger acid than H3AsO3.H2Te is a stronger acid than H2OCH3CH2COOH is a stronger acid than CH3CH2CH2OH

The acidic strength of any acid is directly proportional to the stability of anion formed after removing the acidic H from the acid. Hence more is the stability of the -ve charge, more will be the acidic strength of the acid. 1) The structure of H3AsO4 and H3AsO3 along with the ions forming after removing acidic H is as shown below. From the above structures we can see that the anion is more stable in case of H3AsO4 because it will have more electron withdrawing effect due to more number of O atoms attached to the central atom As. Hence the acid H3AsO4 is stronger acid than H3AsO3.2) The structure of H2Te and H2O along with the ions forming after removing acidic H is as shown below. Since the size of Te is much more than O. Hence the -ve charge will be more delocalised on Te compared to O. Hence the stability of -ve charge is more in case of H2Te compared to H2O. Hence H2Te is stronger acid than H2O.3) The structure of CH3CH2COOH and CH3CH2CH2OH along with the ions forming after removing acidic H is as shown below. Since in case of CH3CH2COOH, the -ve charge will have a resonance with C=O. Hence it will stabilise the -ve charge. But in case of CH3CH2CH2OH, there is no such resonance. Hence the stability of -ve charge is more in case of CH3CH2COOH due to resonance with another O. Hence CH3CH2COOH is stronger acid than CH3CH2CH2OH.