An aqueous solution of carbonic acid (H₂CO₃) contains H₂CO₃, HCO₃^–, and CO₃^2– in different concentrations. Identify the amphoteric species in the solution. Ignore the water present in the solution.

Write equations that show the amphoteric species, NH₃ and HSO₄^-, acting as both an acid and a base.

Of the following compounds, determine whether they are Arrhenius acid, Arrhenius base, or neither 

Ca(OH)₂

RbOH

C₆H₁₄

H₂SO₃

HNO₂

KBr

H₂S

HF

CH₃COOH

Fe(OH)₃

Identify the strongest Lewis acid among the following: BCl₃, BF₃, BI₃, BBr₃.

Rank the following oxyanions in order of increasing basicity based on the acid-dissociation constants (K_a) given below: SeO₃^2–, AsO₄^3–, SeO₄^2–, and CrO₄^2–.

H₂SeO₃: K_a1 = 2.3×10^–3, K_a2 = 5.3×10^–9

H₃AsO₄: K_a1 = 5.6×10^–3, K_a2 = 1.0×10^–7, K_a3 = 3.0×10^–12

H₂SeO₄: K_a1 = very large, K_a2 = 2.2×10^–2

H₂CrO₄: K_a1 = 1.8×10^–1, K_a2 = 3.0×10^–7

Arrange the following in increasing acid strength based on their Ka.

HBr (Ka = 1.0x10⁹)

HI (K_a = 3.2x10⁹)

H₃BO₃ (Ka = 5.8x10^-10)

H₂SO₄ (Ka = 1.0x10³)

H₂SO₃ (Ka = 1.3x10^-2)

CH₃COOH (Ka = 1.8x10^-5)

At 25 °C, the K_a of HXO₃ is less than the K_a of HZO₃. Which of the following is correct?

Rank the solutions of the following substances from least basic to most basic.
Assume the solutions are of equal concentrations.
CH₃COOH, LiOH, NaOCl, NH₄NO₂, KNO₃

Classify the aqueous solution formed from the substances as acidic, basic, or neutral

KBrO 

[CH₃NH₃]ClO₄

Cs₃PO₄ 

NaCl

AlI₃ 

Determine whether increasing the acidity will increase the solubility of the following

Ca(OH)₂,  AgCl, SrCO₃, CdF₂, NiS, Mg₃(PO₄)₂