Buffer Solutions and Acid-Base Concepts

Which combinations of compounds cannot make a buffer? Assume aqueous solutions.

• CH₃COOH and CH₃COONa

• NH₄Cl and NH₃

• HCl and NaCl

• H₂CO₃ and NaHCO₃

Identify the sets that doesn't contain acid-base conjugate pairs.

• HNO2, NO2−

• HCO3-, CO32−

• HCl, ClO4−

• HS−, H2S

What is the pOH of a 0.05 M HCl solution?

• 1.3

• 12.7

• 2

• 11.3

What is [H⁺] in a 0.0015 M solution of Ba (OH)₂?

• 3.33×10⁻¹²M

• 0.0015M

• 2.52M

• 1.0×10⁻⁷M

What volume of a 3.00% (m/v) NaCl solution can be prepared by diluting 20.0 mL of a 12.0% (m/v) NaCl solution?

• 60.0 mL

• 80.0 mL

• 100.0 mL

• 120.0 mL

What is the molarity of a solution prepared by dissolving 17.55 g of KCl (MM = 74.5 g/mol) in 500 mL of solution?

• 0.25 M

• 0.47 M

• 0.35 M

• 0.60 M

What is the conjugate base of HCO₃-?

• HCO₃⁻

• CO₃²⁻

• CO₃⁻

• H₂CO₃

In the reaction below, identify the Brønsted-Lowry acid: HCO₃−+OH−→CO₃²⁻+H₂O

• OH⁻

• CO₃²⁻

• HCO₃⁻

• H₂O