Acid-Base Equilibria

According to the Brønsted-Lowry definition, a base is a:

• Proton donor

• Electron pair acceptor

• Proton acceptor

• Electron pair donor

In the reaction HCl + H₂O → H₃O⁺ + Cl⁻, the conjugate base of HCl is:

• HCl

• H₃O⁺

• H₂O

• Cl⁻

The ion-product constant for water (Kw) at 25°C is:

• 1.0 x 10^⁻7

• 1.0 x 10^⁻14

• 1.0 x 10^⁻1

• 1.0 x 10^⁻10

Tags

NGSS.HS-PS1-3

An amphiprotic substance is one that:

• Can only act as an acid.

• Can only act as a base.

• Can act as both an acid and a base

• Is always neutral

A solution with a pOH of 3 is considered:

• acidic

• basic

• neutral

• impossible to determine

The pOH of a solution with a hydroxide ion concentration [OH⁻] of 1.0 x 10^⁻5 M is:

• 5

• 9

• -5

• 10^-5

A weak acid has a:

• Large K_a value.

• Small K_a value.

• K_a value equal to 1.

• K_a value equal to K_w.

Write the products for the reaction between ammonia (NH₃) and water.

Calculate the hydronium ion concentration [H₃O⁺] in a solution with a hydroxide ion concentration [OH⁻] of 2.0 x 10^⁻4 M at 25°C.

Explain why the hydrogen carbonate ion (HCO₃⁻) is considered amphiprotic.