Chemistry 30

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Solutions Practice Question Answers

Practice Questions 2.5: The Concentration of Ions in Solution
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1.

Write balanced reaction equation that show which ions are produced when the following substances are dissolved in water.


 

Solution:

a. lithium hydroxide LiOH(s) → Li+(aq) + OH-(aq)

b. potassium phosphate K3PO4 (s) → 3 K+(aq) + PO43-(aq)

c. strontium chloride SrCl2(s) → Sr2+(aq) + 2 Cl-(aq)

d. chromium(III) sulfate Cr2(SO4)3 (s) → 2 Cr3+(aq) + 3 SO42-(aq)

2.

Iron(III) nitrate has a solubility of 0.15 M. Find concentration of the ions in solution.


 

Solution:

Begin by writing a balanced dissociation equation:

Fe(NO3)3 → Fe3+(aq) + 3 NO3-(aq)

The concentration of the ions can be determined from the balancing coefficients from the equation:

[Fe3+] = 1× [Fe(NO3)3] = 1 × 0.15 = 0.15 M

[NO3-] = 3× [Fe(NO3)3] = 3 × 0.15 = 0.45 M


3.

Calculate ion concentrations in a 2.00 L solution containing 17.1 g aluminum sulfate, Al2(SO4)3

 


 

Solution:

Before calculating the concentration of the ions, we must first calculate the concentration of the aluminum sulfate solution.

We will need to find the molar mass of Al2(SO4)3:

2 Al = 2 × 27.0 = 54.0 g·mol-1
3 S = 3× 32.0.0 = 96.0 g·mol-1
12 O = 12 × 16.0 = 192.0 g·mol-1

Al2(SO4)3 = 342.0 g·mol-1

Calculate the concentration of Al2(SO4)3:

mol

L
=
17.1 g
×
1 mol

342.0 g
×
1

2.0 L
=
0.0249 mol

L

Write a balanced equation for the dissociation reaction:

Al2(SO4)3 → 2 Al3+(aq) + 3 SO42-(aq)

Using the balanced equation, calculate the concentration of the individual ions:

[Al3+] = 2× [Al2(SO4)3] = 2 × 0.0249 = 0.0498 M or 4.98 ×10-2M

[SO42-] = 3× [Al2(SO4)3] = 3 × 0.0249 = 0.0747 M or 7.47×10-2M


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Credits | Central iSchool | Sask Learning | Saskatchewan Evergreen Curriculum | Updated: 22-May-2006