Reactivity 3.1—Proton transfer reactions - pKa/pKb, buffers HL

What is the formula to calculate pOH from [OH–]?

• pOH = -log10[OH–]

• pOH = [OH–] / 10

• pOH = 14 - pH

• pOH = log10[OH–]

If the pOH of a solution is 3, what is the [OH–] concentration?

• 0.001 M

• 0.0001 M

• 0.1 M

• 0.01 M

How do you convert pH to pOH?

• pOH = 7 - pH

• pOH = pH - 14

• pOH = pH + 14

• pOH = 14 - pH

What is the relationship between pKa and Ka for a weak acid?

• pKa = Ka

• pKa = -log(Ka)

• pKa = log(Ka)

• Ka = -log(pKa)

If a weak acid has a Ka of 1.0 x 10^-5, what is its pKa?

• 7

• 5

• 4

• 6

Explain the significance of the Kw value in acid-base chemistry.

• Kw value indicates the concentration of carbon dioxide in water.

• Kw value is the ion product of water, essential for determining pH and the balance of H+ and OH- in solutions.

• Kw value is the measure of acidity in organic compounds.

• Kw value is the boiling point of water at different altitudes.

For a conjugate acid-base pair, what is the relationship between Ka and Kb?

• Ka + Kb = Kw

• Ka * Kb = Kw

• Ka / Kb = Kw

• Ka - Kb = Kw

If Kb for a weak base is 2.0 x 10^-6, what is its pKb?

• 7.50

• 6.10

• 5.70

• 4.30

How can you determine if a salt solution will be acidic, basic, or neutral?

• The solution will be basic if it contains any salt, regardless of the acid or base used.

• The solution will always be neutral regardless of the parent acid and base.

• The solution will be acidic, basic, or neutral depending on the strength of the parent acid and base.

• The solution's pH is determined solely by the temperature of the solution.

Write the hydrolysis equation for the salt formed from a strong acid and a weak base.

• K+ + H2O ⇌ KH + H3O+

• Ca2+ + H2O ⇌ Ca(OH)2 + H3O+

• NH4+ + H2O ⇌ NH3 + H3O+

• Na+ + H2O ⇌ NaOH + H3O+