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Lab 3 Solubility
Concentration and Conductivity ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Increasing Conductivity ,[object Object],+ + + + + + + - - - - - - - - - - - - + + + + + Least concentrated Most concentrated Compare the number of ions in the same volume
Graph to compare conductivity and concentration conductivity concentration Increasing concentration  — Increasing conductivity Conductivity no longer increases
Eventually Constant Conductivity ,[object Object],[object Object],[object Object],[object Object],[object Object]
Lab Procedures ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Calculating the concentration of the saturated solution ,[object Object],[object Object],[object Object],MOLARITY moles of solute liter of solution
Sample Data
EOS The attractions of water dipoles for ions pulls the ions out of the crystalline lattice and into aqueous solution
Equilibrium in a Saturated Solution ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Dynamic Nature of Equilibrium When a system reaches  equilibrium , the forward and reverse reactions continue to occur … but at equal rates. We are usually concerned with the situation  after  equilibrium is reached. After equilibrium the concentrations of reactants and products remain constant.
Dynamic Equilibrium Illustrated NaCl dissolves and recrystallizes continuously. After a time, the solution contains radioactive Na +  … NaCl containing radioactive Na +  is added to a saturated NaCl solution. …  and the added salt now contains some stable Na + .
Calculating an Equilibrium Constant ,[object Object],[object Object],[object Object],[object Object],[object Object]
Ksp-  the equilibrium constant for saturated solutions of ionic compounds ,[object Object],[object Object],[object Object],[object Object],[object Object]
Calculating Concentration given the Ksp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Given the Concentration  calculate the Ksp ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Ksp and solubility ,[object Object],[object Object],[object Object]
 
Calculating the Concentration of Calcium fluoride in a saturated solution ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Preparing a solution of known molarity ,[object Object],[object Object]
Again, a molar solution The volume is exactly 1.0 L Note that not all of the initial 1.0 L of water was used to prepare the solution
Dilution of a solution ,[object Object]
Other Units of Concentrations ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Mole Fraction and Mole Percent The  mole fraction  ( x i ) of a solution component  i  is the fraction of all the molecules in the solution that are molecules of  i EOS The  mole percent  of a solution component is its mole fraction multiplied by 100 Sum of  x i  must equal 1
Calculating other concentrations ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Dilution The desired molarity solutions are often prepared from concentrated stock solutions (routinely used solutions prepared in concentrated form) by adding water. This process is called dilution. Moles of solute before dilution  = moles of solute after dilution   M 1 V 1  = M 2 V 2
Figure 4.11 (a) A Measuring Pipet    (b) A Volumetric (transfer) Pipet
Example:  What volume of 16 M sulfuric acid must be used to prepare 1.5 L of 0.10 M H 2 SO 4 solution? V 1  = Volume before dilution = ? M 1  = Concentration before dilution = 16 M V 2  = Volume after dilution = 1.5 L M 2  = Concentration after dilution = 0.10 M M 1 V 1  = M 2 V 2 V 1  =M 2 V 2  / M 1  = (0.10 M x 1.5 L)/ 16 M    = 0.0094 L = 9.4 mL
 
 

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Lab 3

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  • 4. Graph to compare conductivity and concentration conductivity concentration Increasing concentration — Increasing conductivity Conductivity no longer increases
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  • 9. EOS The attractions of water dipoles for ions pulls the ions out of the crystalline lattice and into aqueous solution
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  • 11. Dynamic Nature of Equilibrium When a system reaches equilibrium , the forward and reverse reactions continue to occur … but at equal rates. We are usually concerned with the situation after equilibrium is reached. After equilibrium the concentrations of reactants and products remain constant.
  • 12. Dynamic Equilibrium Illustrated NaCl dissolves and recrystallizes continuously. After a time, the solution contains radioactive Na + … NaCl containing radioactive Na + is added to a saturated NaCl solution. … and the added salt now contains some stable Na + .
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  • 21. Again, a molar solution The volume is exactly 1.0 L Note that not all of the initial 1.0 L of water was used to prepare the solution
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  • 24. Mole Fraction and Mole Percent The mole fraction ( x i ) of a solution component i is the fraction of all the molecules in the solution that are molecules of i EOS The mole percent of a solution component is its mole fraction multiplied by 100 Sum of x i must equal 1
  • 25.
  • 26. Dilution The desired molarity solutions are often prepared from concentrated stock solutions (routinely used solutions prepared in concentrated form) by adding water. This process is called dilution. Moles of solute before dilution = moles of solute after dilution M 1 V 1 = M 2 V 2
  • 27. Figure 4.11 (a) A Measuring Pipet (b) A Volumetric (transfer) Pipet
  • 28. Example: What volume of 16 M sulfuric acid must be used to prepare 1.5 L of 0.10 M H 2 SO 4 solution? V 1 = Volume before dilution = ? M 1 = Concentration before dilution = 16 M V 2 = Volume after dilution = 1.5 L M 2 = Concentration after dilution = 0.10 M M 1 V 1 = M 2 V 2 V 1 =M 2 V 2 / M 1 = (0.10 M x 1.5 L)/ 16 M = 0.0094 L = 9.4 mL
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  • 30.