I titrated Ca(OH)2 with HCL. (HCL in burette) and (CaOH2 in the flask). Known In

Question

I titrated Ca(OH)2 with HCL. (HCL in burette) and (CaOH2 in the flask).

Known Information:
Ca(OH)2 = 25 mL
HCl = 10.00mL used
HCL = 0.01M
Temp: 25 degrees Celcius

1. Write a balanced, net ionic equation for the titration reaction. Use this equation to perform the calculations.
2. CALCULATE THE [OH-] in the saturated Ca(OH)2 solution.
3. Determine the experimental solubility of the Ca(OH)2 at your experimental temperature.
4. Determine the experimental Ksp of Ca(OH)2 at the observed temperature



What I got so far:

I got my balanced net ionic equation to be :

2H2 + 2OH --> 2H2O


HOw can I do #2,3,4 with the equation above?

Explanation / Answer

1. Ca(OH)2 +2HCl -- > CaCl2 + 2H20

2.M of Ca(OH)2 = 0.002M
So [OH-] = 0.004M

3.Solubility of Ca(OH)2 is 0.002M

4. Ksp = 4s^ 3 = 3.2 * 10 ^ -8

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