In: Chemistry
Which of the following statements is false?
(a) An Arrhenius base increases the concentration of OH- in water.
(b) A Brønsted-Lowry base is a proton acceptor.
(c) Water can act as a Brønsted–Lowry acid.
(d) Water can act as a Brønsted–Lowry base.
(e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.
First, define all tyes of acid/bases
Arrhenius acid/base is the first theory on acid/base definitions, it is mostly true for general applications.
Arrhenius acid is any type of substance that will dissociate in water to form hydrogen ions [H+]. That is, an acid increases the concentration of H+ ions in an aqueous solution.
Arrhenius base is any type of substance that will form hydroxide [OH−] ions. It typically must increase pH since OH- increases in concentration.
Bronsted Lowry acid: any species that will donate H+ (protons) in solution, and makes pH lower (i.e HCl)
Bronsted Lowry base: any species that will accept H+ (protons) in solution, and makes pH higher (NH3 will accept H+ to form NH4+)
Typically, acid/bases are shown in the left (reactants)
when we write the products:
Bronsted Lowery conjugate base = the base formed when the B.L. acid donates its H+ proton ( i.e. HCl -> Cl-
Bronsted Lowery conjugate acid = the acid formed when the B.L. base accept its H+ proton ( i.e. NH4+ has accept H+ proton)
now..
A)
this is true, OH- is directly related --> NaOH --> Na+ + OH-
b)
also true, examples is NH3 + H2O = NH4+ + OH-
c)
true, it can donate H+ --> H2O = H+ + OH-
d)
also true
H2O + H+ --< H3O+
e)
FALSE not every group
example --< CH3-OH
will only donate H+ partially