Molarity of Saturated Salt

In this lab, I will be able to find two things. First, I will determine the molarity of saturated salt solutions and secondly I will calculate the Ksp and percent error. I am should prove that the concentration of a solid does not change and also I will get the Keq. The Ksp will be for both sodium chloride and potassium chloride. Three previously massed samples of KCl (wate softner salt), three previously massed samples of NaCl (Rock salt), mortal and pestle, two 50 ml beakers, 10.0 ml Graduated cylinder, 2 Styrofoam cups, a thermometer, a stirring spoon, distilled water, and crushed ice 1. Start off with the preparation

2. (for steps 2 and 3 precision is a must) First calibrate the dropper pipette. This is done by measuring how many drops of distilled water from the pipette it takes to fill a 10.0 ml graduated cylinder to the 1.00 ml mark 3. Record how many drops of vinegar it takes to fill 1.00 ml 4. Record the trial

5. Repeat steps 2, 3, and 4 until you have 3 different trials 6. Print out the data table
7. Prepare two ice water baths by filling up a Styrofoam cup with crushed water and just enough water to cover up the ice 8. In one water bath, place a 50 ml beaker three fourths full of distilled water. This will be the solvent and should be as close to 0°C as possible. 9. In the second water bath, place an empty 50ml beaker, which will be the vessel in the experiment. (You’re ready to experiment) 10. Record mass of KCl sample

11. Place the entire sample in the mortar and pestle and grind into a fine powder 12. Pour the sample in the 50ml beaker
13. Using the 10.0 ml graduated cylinder and dropper pipette measure out exactly 2.0 ml of the chilled distilled water and add to the mortar. 14. Swirl the water in mortar in order to get the salt that remained. Then pour the water into the 50ml beaker where the rest of the powder solution is 15. Record the volume of water added

16. Add drops of the chilled water in two drop increments and swirl for the solution to dissolve 17. Continue to add two drop increments until entire solid is dissolved. (Keep track of total chilled water. 18. Repeat steps 10-17 but with the KCl and then for the NaCl (remember to clean mortar and pestle)

Calculation

2. KCl= K+ + Cl-
NaCL completely dissociates
3. NaCl= .15M
KCl= .5M
4. H2Cl + KO
Na + (aq) + Cl- (aq)
5. KCl= 7.9006
NaCl= 38.65

Discussion
1. NaCl about 20%
KCl about 30%
2. As we know a colder temperature will slow down a reaction. Maybe if we used room temperature water then the reaction would be too fast 3. I think that the Ksp values would change. As the temperature changes so does will the Ksp values.