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SOLUBILITY

1 Salt Name: Sodium Chloride
2 Salt Formula: NaCl
3 Balanced dissociation reaction:  

 

NaCl(aq)à Na+(aq) +Cl–(aq)

 
4 How many cations (+ ions) are in this salt (from formula of salt) 1
5 Did the temperature of the solution (surroundings) increase or decrease as the salt was dissolving? Decrease
6 Based on that observation, the solution process for this salt is (endothermic or exothermic)? Endothermic
7 The ΔHrxn is a positive or negative number? Positive
  Temperature (0C)

 

 M of cation

(Reading from virtual lab monitor without scientific notation)

 M dissolved salt

Eqn 1

 Grams/L dissolved salt

Eqn 2
  Graph: x axis     Graph: y axis
1 20 0.6183

 
0.6183
36.10872

 
2 40 0.6309

 

 0.6309 36.84456

 
3 60 0.6439 0.6439 37.60376

 


Data Sheet: Trial 2

1 Salt Name: Potassium dichromate
2 Salt Formula: K2Cr2O7
3 Balanced dissociation reaction:  

 

K2Cr2O7à 2K+(aq) + Cr2O7–(aq)

 
4 How many cations (+ ions) are in this salt (from formula of salt) 2
5 Did the temperature of the solution (surroundings) increase or decrease as the salt was dissolving? Decrease
6 Based on that observation, the solution process for this salt is (endothermic or exothermic)? Endothermic
7 The ΔHrxn is a positive or negative number? Positive
  Temperature (0C)

 

 M of cation

(Reading from virtual lab monitor without scientific notation)

 M dissolved salt

Calculate using Eqn 1

 Grams/L dissolved salt

 
  Graph: x axis     Graph: y axis
1 20
0.0496
0.0248
7.29578
2 40 0.087 0.0435 12.79705
3 60 0.1388 0.0694 20.41644

 


Data Sheet: Trial 3

1 Salt Name: Cerium(III) sulfate
2 Salt Formula: Ce2(SO4)3
3 Balanced dissociation reaction: Ce2(SO4)3 (aq)à 2Ce3+ (aq)+ 3SO42-(aq)

 

 

 
4 How many cations (+ ions) are in this salt (from formula of salt) 2
5 Did the temperature of the solution (surroundings) increase or decrease as the salt was dissolving? increase
6 Based on that observation, the solution process for this salt is (endothermic or exothermic)? Exothermic
7 The ΔHrxn is a positive or negative number? negative
  Temperature (0C)

 

 M of cation

(Reading from virtual lab monitor without scientific notation)

 M dissolved salt

Calculate using Eqn 1

 Grams/L dissolved salt

 
  Graph: x axis     Graph: y axis
1 20 0.02269

 

 0.011345

 

 6.448722631

 
2 40 0.01694

 

 0.00847

 

 4.814515706

 
3 60 0.00878 0.00439 2.495362922


 General Questions:

 

  1. Based on your data (and common knowledge), what is generally true of the solubility of most solids in liquid solvents as the temperature of the solvent rises?

The solubility of a salt increases as the temperature of the solvent increases until a saturation point is reached.

 

 

 

  1. How does this general trend for solids compare with the solubility of gases in liquid solvents as the temperature of the solvent rises? (Consult your textbook if necessary.)

The solubility of solids increases while that of gases decrease with the increase in the temperature of the solvent.

 

 

 

  1. Based on your observations of surroundings temperature (increasing or decreasing for the 3 salts as they dissolved) and how much salt dissolved as the temperature changed, can you hypothesize a relationship between the endo/exothermicity (∆Hrxn) of the dissolving reaction and the resulting pattern of solubility (increasing or decreasing) for the salts?

Solubility is higher in an endothermic reaction than in an exothermic dissociation reaction.

 

From your graph (Include the graph in your report (copy/paste or pdf))

  1. Using your graph, find the solubility of salt (you used) in Trial 2 at 300C _10_________ g/L
  2. Which of your 3 salts was most soluble in water at 600C? ________NaCl____________________
  3. Which of your 3 salts had its solubility least affected by the temperature of the solvent? ___NaCl_____

 

 

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