Hence, iodide ion is a better leaving group. Predict the stronger acid in each pair: (a) HNO 3 or HNO 2; (b) H 2 S or H 2 O; (c) H 2 SO 4 or H 2 SeO 4; (d) CH 3 COOH or CCl 3 COOH.
Let me share something not just about the answer but how to reach the answer. The bond energy of H2Se is less than H2S, making it easier for the hydrogen atom to leave the molecule.
> For oxyacids with the same central atom, the acidity increases as the number of atoms bonded to the central atom increases. The direction of equilibrium in an acid-base reaction is always in the favor of the reaction of the stronger acid with the stronger base to form the weaker acid and the weaker base. So, in terms of the original acids: H2Se > H2S > H2O in terms of acid strength. a. HBr, HF HBr is the stronger acid because Br is larger than F. Thus, the H-BR bond is weaker than the H-F bond and Dr- is more stable than F-. The Polarity of the X H Bond. When all other factors are kept constant, acids become stronger as the X H bond becomes more polar.
the weakest conjugate base came from the strongest acid) Hope this helps you! Explain. (i.e. 11 Ag + + 2NH 3 ==== Ag(NH 3) 2 +-A Bronsted acid-base reaction is an exchange of a Lewis acid between two Lewis bases. b. H2Se, H2S H2Se is the stronger acid because Se is larger than S. Thus, the H-Se bond is weaker
(a) CO2 OCS (b)NH4Cl NH4 (c) PF3 PF5 (d) H2O H2S Someone please help me with this I don't understand it at all.
Thus, we predict that "HBrO"_2 should be a stronger acid than "HBrO".
The quantity is the measure of the acidity of the acids and bases quantitatively.
Predict which substance in each of the following pairs would have the stronger intermolecular forces. (i.e. In water molecule oxygen has two lone pair and it is more electronegative than sulfur. Is nitric acid stronger than H2S?
Sulfur is bigger, so the overlap between hydrogen orbit and sulfur orbit is less efficient.
Using the table below, identify the stronger acid in each of the following pairs HCO−3 or H2CO3 H2CO3 When sodium carbonate dissolves in water, the carbonate ion CO2−3 acts as a base. By definition, the pK a value tells us the extent to which an acid will react with water as the base, but by extension we can also calculate the equilibrium constant for a reaction between any acid-base pair.
a. HBr, HF HBr is the stronger acid because Br is larger than F. Thus, the H-BR bond is weaker than the H-F bond and Dr- is more stable than F-.
The second-row nonmetal hydrides, for example, become more acidic as the difference between the electronegativity of the X and H atoms increases. "HBrO"_2 has K_a = 1.2 × 10^-5, while "HBrO" has K_a = 2 × 10^-9. Therefore, H2Se is expected to be a stronger acid than H2S. Finally, acid-base conjugate pairs are related as I first mentioned. HF is the strongest of these four acids, and CH 4 is one of the weakest Brnsted acids known.
In each ofthe following pairs choose the compound that is the stronger acid. Therefore, H2Se is expected to be a stronger acid than H2S.
For this reason, the H-S bond is weaker than H-O bond.
Explain your answers. H2Se is a stronger acid than H2S.
The explanation is the size of sulfur compared with the oxygen.
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