which of the following statements are true?

Question

a) For an acid H-A : the greater the electronegativity of A, the stronger the acid HA

b) For an acid H-A : the stronger the H-A bond, the stronger the acid H-A

c) HBr is a stronger acid than HF

d) H2SO3 is a weaker acid than H2SO4

e) HClO is a stronger acid than HBrO

f) For carboxylic acids : the greater the electronegativities of the atoms in the group bonded to the carboxyl group, the stronger the acid

i tried
bcd
bcdf
acd
d

btw i only have 1 more try

Answer 1

a) True. The more electronegative A is, the more the H-A bond is polarized toward A, making the hydrogen more acidic.
b) False. The stronger the HA bond is, the weaker the acid is.
c) True. HBr is a strong acid, HF is a weak one, despite the greater electronegativity of F vs. Br.
d) True. H2SO3 is a weak acid, H2SO4 is a strong acid.
e) True. Ternary acids are stronger with the increasing electronegativity of the central atom.
f) True. Conductive effect, as the atoms bonded to the carbon pull electron density from it, which pulls it from the hydroxy oxygen, which makes the hydrogen more acidic. Thus, CF3CO2H is a much stronger acid than CH3CO2H.

Answer 2

C is true, as it is less electronegative and a bigger atom.

D is true as well, has H2SO3 is the conjugate base of H2SO4 (one of the strongest acids period)

Answer 3

It's been awhile but I think a,c,d, and f are true