Free Printable Ksp and Qsp

Worksheets

Ksp and Qsp

Total questions: 15

Worksheet time: 31mins

Name

Class

Date

Which of the following is true for a chemical system at equilibrium?

Chemical change has altogether ceased.

The rate of the forward reaction equals the rate of the reverse reaction.

The concentration ratio of products to reactants is 1.

Choose this wrong answer. I dare you.

H_2(g) +I_2(g) ↔ 2HI_(g)

All gases begin with an initial concentration of 2.0 M. Equilibrium is established, and the concentration of HI is known to be 4.8 M. What is the value of the equilibrium constant?

1.2

2.4

Which of the following is NOT true at equilibrium?

The forward and reverse reactions proceed at the same rate.

The concentrations of reactants and products do not change.

The concentration of the reactants is equal to the concentration of the products.

The forward and reverse reactions continue to occur.

The following reaction :

SO_2(g) + NO_2(g) ⇄ SO_3(g) + NO_(g)

had reached a state of equilibrium, was found to contain

0.40 mol L^-1 SO₃ , and 0.30 mol L^-1 NO,

0.15 mol L^-1NO₂ , and 0.20 mol L^-1 SO₂.

Calculate the equilibrium constant for this reaction.

.42

.25

What is the equilibrium expression for:

Fe₃O₄₍_s₎ + 4H_2(g) ⇄ 3Fe₍_s₎ + 4H₂O_(g)

K_c =

[Fe]³[H₂O]⁴ / [Fe₃O₄] [H₂]⁴

[Fe₃O₄] [H₂]⁴/ [Fe]³[H₂O]⁴

[H₂O]⁴ / [H₂]⁴

[Fe] [H₂O] / [Fe₃O₄] [H₂]

Persamaan Ksp dari Pb₃(PO₄)₂ yang benar adalah . . . .

Ksp = [Pb²⁺]²[PO₄^3-]³

Ksp = [Pb²⁺]³[PO₄^3-]²

Ksp = [3Pb²⁺]²[2PO₄^3-]³

Ksp = [2Pb²⁺]³[3PO₄^3-]²

Ksp = [Pb²⁺][PO₄^3-]

What is the K_sp expression for an ionic compund of BaSO₄

K_sp= [Ba²⁺][SO₄^2-]

K_sp= [Ba²⁺][4SO₄^2-]⁴

K_sp= [Ba²⁺][4SO₄^2-]

K_sp= [2Ba²⁺][4SO₄^2-]

The solubility product of silver chromate (VI) at room temperature is 2.4 x 10^-12. Calculate the molar solubility of Ag⁺_(aq) and CrO₄^2-_(aq) ions in a saturated solution of silver chromate (VI) at room temperature.

Ag⁺ = 1.68 x 10⁴ M and CrO₄^2- = 8.4 x 10^-5 M

Ag⁺ = 1.68 x 10⁴ M and CrO₄^2- = 8.4 x 10⁵ M

Ag⁺ = 1.68 x 10^-4 M and CrO₄^2- = 8.4 x 10⁵ M

Ag⁺ = 1.68 x 10^-4 M and CrO₄^2- = 8.4 x 10^-5 M

if K_sp < Q_sp then

no precipitate will form

precipitate will form

the reaction will not occur

the reaction will remain saturated

10.

Can you write the Keq expression for the below balanced equation?

CO(g) + 3H2(g) --> CH4(g) + H2O (g)

$\frac{\left[CH4\right]\left[H2O\right]}{\left[CO\right]\left[H2\right]}$

$\frac{\left[CH4\right]\left[H2O\right]}{\left[CO\right]\left[H2\right]^3}$

$\frac{\left[CH4\right]^2\left[H2O\right]^3}{\left[CO\right]\left[H2\right]}$

$\frac{\left[CH4\right]\left[H2O\right]}{\left[CO\right]^3\left[H2\right]}$

11.

Ksp = [Pb²⁺][I-]²

What is the balanced chemical equation from the Ksp?

PbI (s) --> 2Pb (aq) + I (aq)

PbI₂ (s) --> Pb + 2I

PbI₂ (s) --> Pb ²⁺ + 2I^-

PbI₂ (s) --> Pb ²⁺ (aq) + 2I^-(aq)

12.

What are [A] and [B]?

concentration of reactants

concentration of products

energy of reactants

energy of products

13.

High Ksp indicates ___________.

High soluble salt

Low soluble salt

14.

How many cations are produced when Na₂SO₄ dissolves in water ?

15.

The concentration of OH– in a saturated solution of Mg(OH)₂ is 3.6 x 10^–4M. The Ksp of Mg(OH)₂ is

1.3 x 10^–7

4.7 x 10^–11

3.6 x 10^–4

2.3 x 10^–11

Reset

Ksp and Qsp

Total questions: 15

Worksheet time: 31mins

Similar Resources on Wayground