Which of the following statements are true?...?

Question

Which of the following statements are true?...?

a) For binary acids HA in the same row of the periodic table, the greater the electronegativity of A
the weaker the acid HA

b) For binary acids HA in the same column of the periodic table, the weaker the H-A bond
the stronger the acid HA

c) HBr is a stronger acid than HCl

d) H2SO3 is a weaker acid than H2SO4

e) HBrO is a stronger acid than HClO

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

Gervald F, the reason I reposted this is because the answer I got before was wrong and I forgot to entend the time.

Answer 1

B, C, D and F

A- the more electronegative, the easier it should be to remove hydrogen (false)
B- the weaker the bond, the easier it is to remove hydrogen (true)
C- the conjugate base is more stable for Br- because it is larger and more polarizable
(true)
D- H2SO3 does not have as many ways to delocalize the charge of the conjugate base
(true)
E- the more electronegative halide should weaken the OH bond (false)
F- the conjugate base of a carboxylic acid has the negative charge delocatlized over
the -COO partion. If you have an electronegative atom next door (alpha position) you
will have a partial positive charge next to a negative one. (ture)

Answer 2

I answered this exact question within the last 48 hours. Why do we get so many multiple postings?

Have a look through recent answers.