ap semester 1 units 3,4, 5

Front

Consider the following reversible reaction: 2 PF₃(g) ⇌ 2 P(s) + 3 F₂(g). An empty vessel was filled with PF₃(g) to a pressure of 2.0 atm, and allowed to react until equilibrium was reached. If pressure of the reaction mixture at equilibrium was 2.4 atm, what is the value of Kp?

Back

1.2

Front

Addition of all of the following will affect the solubility of FeCO₃ except: H₂CO₃, HCl, Na₂CO₃, NaCl

Back

NaCl

Front

Back

Front

What is the pH of a 10.0 mL sample of a 0.010 M HCl solution after adding 90.0 mL of water?

Back

3.0

Front

Suppose we have a 0.10 M HF solution. Which of the following, when added, would result in the lowest [F-]? Options: Nothing else added, 0.0010 mol HCl, 0.0010 mol KF, 0.0010 mol KOH

Back

0.0010 mol HCl

Front

Which acid is the strongest and why? Acetic acid (CH₃COOH), Chloroacetic acid (CH₂ClCOOH), Dichloroacetic acid (CHCl₂COOH), Trichloroacetic acid (CCl₃COOH).

Back

Trichloroacetic acid (CCl₃COOH) because it has three chlorine atoms, increasing electron withdrawal and acidity.

Front

A 3.0 L solution contains 0.800 mol of a weak acid, HA. Which species is in the greatest concentration after 0.800 mol of NaOH is added? Options: A⁻, H⁺, HA, OH⁻

Back

A⁻

Front

Sulfurous acid, H₂SO₃, has a Ka₁ of 1 x 10^-2 and Ka₂ of 1 x 10^-7. What is true of this solution at pH = 7?

Back

The dominant species is HSO₃^-.

Front

What is the effect of adding a common ion to a saturated solution of a salt?

Back

It decreases the solubility of the salt due to the common ion effect.

Front

Which of the following acids will have the highest pH in a 0.1 M solution? Options: HCl, HNO₃, HF, CH₃COOH

Back

CH₃COOH, because it is a weak acid compared to the others which are strong acids.