Acid Base Definitions

C. it is a proton acceptor

Ca(OH)₂ is a Brønsted-Lowry base because A. it can dissolve in water B. it is a hydroxide donor C. it is a proton acceptor D. it is a polar molecule

D. HCN, CH₃NH₃⁺

Consider the reaction shown. Which species are the Brønsted-Lowry acids? A. CN⁻, CH₃NH₃⁺ B. HCN, CH₃NH₂ C. CH₃NH₂, CH₃NH₃⁺ D. HCN, CH₃NH₃⁺

C. PO₄³⁻, NO₂⁻

Consider the reaction shown. Which species are the Brønsted-Lowry bases? A. PO₄³⁻, HNO₂ B. HPO₄²⁻, NO₂⁻ C. PO₄³⁻, NO₂⁻ D. NO₂⁻, HNO₂

A. it produces hydronium ions in solution

HBr is an Arrhenius acid because A. it produces hydronium ions in solution B. it produces hydroxide ions in solution C. it is a polar molecule D. it an dissolve in water

A. Cr³⁺

In the reaction shown, which reactant is the Lewis acid? A. Cr³⁺ B. H₂O C. Cr(H₂O)₆³⁺ D. None of these are Lewis acids.

D. H₂SO₃

The conjugate acid of HSO₃⁻ is A. SO₃²⁻ B. HSO₄⁻ C. HSO₃²⁻ D. H₂SO₃

C. CO₃²⁻

The conjugate base of HCO₃⁻ is A. HCO₃²⁻ B. H₂CO₃ C. CO₃²⁻

C. The carbon carries partial positive charge so it can accept a pair of electrons

The reason CO₂ is a Lewis acid is A. The oxygen carries a partial negative charge so it can donate a pair of electrons. B. The oxygen reacts with water to form hydroxide ions. C. The carbon carries partial positive charge so it can accept a pair of electrons. D. The carbon releases the oxygen to the water forming H₂O₂.

A. NH₃

Which of the following could NOT behave as a Lewis acid? A. NH₃ B. AlCl₃ C. BBr₃ D. None of these are Lewis acids

B. CH₃NH₂, CH₃NH₃⁺

Which of the following is a conjugate acid-base pair? A. CH₃NH₂, OH⁻ B. CH₃NH₂, CH₃NH₃⁺ C. H₂O, CH₃NH₃⁺ D. OH⁻, CH₃NH₃⁺

A. OH⁻, H₂O

Which of the following is a conjugate acid-base pair? A. OH⁻, H₂O B. NH₃, OH⁻ C. OH⁻, NH₄⁺ D. H₂O, NH₄⁺

B. HS⁻

Which of the following is an amphoteric species? A. NH₃ B. HS⁻ C. S²⁻