Chemical Equilibrium and Acid-Base Theories

Given the equation representing a system at equilibrium: NH3(g) + H2O(l) ⇌ NH4+(aq) + OH−(aq), in this system, the H2O(l) acts as

• an acid, because it accepts an H+

• an acid, because it donates an H+

• a base, because it accepts an H+

• a base, because it donates an H+

One acid-base theory states that a base is an

• H− donor

• H+ acceptor

• H+ donor

• H+ acceptor

One acid-base theory states that an acid is an

• electron donor

• neutron donor

• an H+ donor

• an OH− donor

According to "alternative theory" of acids and bases, an acid is any species that

• releases hydroxide ions into solution

• releases oxide ions into solution

• donates protons to another species

• accepts protons from another species

According to an "alternative theory", H2O is considered to be a base when it

• donates an electron

• accepts an electron

• donates a proton

• accepts a proton

According to an alternative theory, an acid is any species that can

• donate a proton

• donate an electron

• accept a proton

• accept an electron

According to one acid-base theory, a base is an

• H2 acceptor

• H2 donor

• H+ acceptor

• H+ donor

Given the balanced equation representing a reaction: HCl + H2O → H3O+ + Cl−, the water molecule acts as a base because it

• donates an H+

• accepts an H+

• donates an OH−

• accepts and OH−

According to one acid-base theory, NH3 acts as a base when an NH3 molecule

• accepts an H+ ion

• donates an H+ ion

• accepts an OH− ion

• donates an OH− ion

According to one acid-base theory, a base is an

• H+ acceptor

• H+ donor

• Na+ acceptor

• Na+ donor