Question

What is the net ionic equation for the neutralization reaction between a HI with NH3?

HI (aq) + NH₃ (aq) ⇌ NH₄I (aq),

HI (aq) + OH^- (aq) ⇌ H₂O (l) + I^- (aq),

H₃O⁺ (aq) + OH^- (aq) ⇌ 2 H₂O (l)

H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l)

Which statement about buffers is NOT true?

		A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid, as long as the amount of strong acid is less than the amount of weak base.
		A buffer can be made by mixing a weak acid with its conjugate weak base at similar concentrations.
		Buffers resist change in pH upon addition of small amounts of strong acid or strong base.
		A buffer does not change pH on addition of a strong acid or strong base

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate a 50.00 mL solution of 5.00 × 10^-3 M Mg(OH)₂ to the equivalence point?

		200 mL
		25 mL
		100 mL
		50 mL

Which is the best acid to use in the preparation of a buffer with pH = 3.3?

		HOI (Ka = 2.0 × 10-11)
		H3PO4 (Ka = 5.9 × 10-2)
		HN3 (Ka = 1.9 × 10-5)
		HSCN (Ka = 1.0 × 10-4)