Given the equation representing a reversible reaction:

NH₃(g) + H₂O(ℓ) ⇌ NH₄⁺(aq) + OH (aq)

According to one acid-base theory, the reactant that donates an H⁺ ion in the forward reaction is

(1) NH₃(g)

(2) H₂O(ℓ)

(3) NH₄⁺(aq)

(4) OH (aq)

Given the diagram representing a reaction:

According to one acid-base theory, the water acts as

(1) a base because it accepts an H⁺

(2) a base because it donates an H⁺

(3) an acid because it accepts an H⁺

(4) an acid because it donates an H⁺

Given the balanced equation representing a reaction:

H₂O(ℓ) + HCl(g) → H₃O⁺(aq) + Cl⁻(aq)

According to one acid-base theory, the H₂O(ℓ) molecules

(1) accept H⁺ ions

(2) accept OH⁻ ions

(3) donate H⁺ ions

(4) donate OH⁻ ions

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

(1) donates an H⁺ ion

(2) accepts an H⁺ ion

(3) donates an OH⁻ ion

(4) accepts an OH⁻ ion

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

(1) accepts an H⁺ ion

(2) donates an H⁺ ion

(3) accepts an OH⁻ ion

(4) donates an OH⁻ ion

Given the equation representing a reaction at equilibrium:

H₂S(aq) + CH₃NH₂(aq) ⇌ HS⁻(aq) + CH₃NH₃⁺(aq)

According to one acid-base theory, the forward reaction is classified as an acid-base reaction because

(1) H₂S is a H⁺ donor and CH₃NH₂ is a H⁺ acceptor

(2) CH₃NH₂ is a H⁺ donor and H₂S is a H⁺ acceptor

(3) HS⁻ and CH₃NH₃⁺ are both H⁺ donors

(4) CH₃NH₃⁺ and HS⁻ are both H⁺ acceptors

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

(1) accepts an H⁺

(2) accepts an OH⁻

(3) donates an H⁺

(4) donates an OH⁻

Given the balanced equation representing a reaction:

HSO₄⁻(aq) + H_{2O(ℓ) → H3O}+(aq) + SO₄2−(aq)

According to one acid-base theory, the H₂O(ℓ) molecules act as

(1) a base because they accept H⁺ ions

(2) a base because they donate H⁺ ions

(3) an acid because they accept H⁺ ions

(4) an acid because they donate H⁺ ions

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

(1) H⁺ acceptor

(2) H⁺ donor

(3) Na⁺ acceptor

(4) Na⁺ donor

Which statement describes one acid-base theory?

(1) An acid is an H⁺ acceptor, and a base is an H⁺ donor.

(2) An acid is an H⁺ donor, and a base is an H⁺ acceptor.

(3) An acid is an H⁻ acceptor, and a base is an H⁻ donor.

(4) An acid is an H⁻ donor, and a base is an H⁻ acceptor.

According to one acid-base theory, a water molecule acts as a base when it accepts

(1) an H⁺ ion

(2) an OH⁻ ion

(3) a neutron

(4) an electron

One acid-base theory defines an acid as an

(1) H⁻ acceptor

(2) H⁻ donor

(3) H⁺ acceptor

(4) H⁺ donor

Given the equation representing a reversible reaction:

HCO₃(aq) + H₂O(ℓ) ⇌ H₂CO₃(aq) + OH⁻(aq)

Which formula represents the H⁺ acceptor in the forward reaction?

(1) HCO₃(aq)

(2) H₂O(ℓ)

(3) H₂CO₃(aq)

(4) OH⁻(aq)

Given the balanced equation representing a reaction:

HCl + H₂O → H₃O⁺ + Cl⁻

The water molecule acts as a base because it

(1) donates an H⁺

(2) accepts an H⁺

(3) donates an OH⁻

(4) accepts an OH⁻

Given the equation representing a reversible reaction:

CH₃COOH(aq) + H₂O(ℓ) ⇌

CH₃COO⁻(aq) + H₃O⁺(aq)

According to one acid-base theory, the two H⁺ donors in the equation are

(1) CH₃COOH and H₂O

(2) CH₃COOH and H₃O⁺

(3) CH₃COO⁻ and H₂O

(4) CH₃COO⁻ and H₃O⁺