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Part 1: Ksp and Molar Solubility of Ca(OH)2 ww Trial 1 Trial 2 Trial 3 Buret reading, final (mL) 24.2 47.4 64.3 Buret reading, initial (mL) 0.0 24.2 47.4 Volume HCl used (mL) Concentration of standard HCl solution (M) Mole HCl added Mole OH in saturated Ca(OH), solution Volume of saturated Ca(OH), solution (L) [OH'] at equilibrium (mol/L) [Ca +21 at equilibrium (mol/L) Kp of Ca(OH)2 from the titration Average Ksp of Ca(OH), from the titration Molar solubility of Ca(OH), from the titration

Part 1: Ksp and Molar Solubility of Ca(OH)2 ww Trial 1 Trial 2 Trial 3 Buret reading, final (mL) 24.2 47.4 64.3 Buret reading, initial (mL) 0.0 24.2 47.4 Volume HCl used (mL) Concentration of standard HCl solution (M) Mole HCl added Mole OH in saturated Ca(OH), solution Volume of saturated Ca(OH), solution (L) [OH'] at equilibrium (mol/L) [Ca +21 at equilibrium (mol/L) Kp of Ca(OH)2 from the titration Average Ksp of Ca(OH), from the titration Molar solubility of Ca(OH), from the titration

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Can you please please please not reject this question. I really need to know this. AND THIS IS NOT A GRADED QUESTION.  So can someone please answer this without rejecting this everytime. I really need to learn how to do the calculations for this becuse I have my exam within 2 weeks. So please someone and this is not a graded question. Okay this time I have included all the information. Molarity is included. 

An experiment was conducted by following the procedure below.

 

  1. Prepare a 50-mL burette for titration. Rinse the clean burette and tip with two 5-mL portions of standardized 0.005 M HCl solution and discard. Fill the burette with standardized   HCl, remove the air bubbles in the tip, and record the initial volume (± 0.01mL).     
  2. Record the molarity of the HCl solution, which is 0.005M
  3. Cover the flask with parafilm to avoid contact with carbondioxide from air.
  4. Rinse a 25 mL pipet with 1 or 2 mL of the saturated Ca(OH)2 solution and discard.
  5. Pipet 25 mL of the filtrate into a clean 125-mL Erlenmeyer flask and add 2 drops of bromocresol green indicator. Record the solution's temperature. Titrate with the standard HCl solution.
  6. Record the finaL volume (± 0.01mL) needed to just turn the solution color.
  7. Repeat the titration with two new samples of Ca(OH)2.

Repeat Part I, steps 1 - 3, using the saturated Ca(OH)2 solution to which 0.100M Ca+2 has been added.

 

Using the information in the above proceudre, fill the two tables in the pictures and please show your working.

 

Please please please dont reject this. I have asked everyone i know and nobody was able to do it :( :

Part 1: Ksp and Molar Solubility of Ca(OH)2 Trial 1 Trial 2 Trial 3 Buret reading, final (mL) 24.2 47.4 64.3 Buret reading, initial (mL) 0.0 24.2 47.4 Volume HCl used (mL) Concentration of standard HCl solution (M) Mole HCl added Mole OH- in saturated Ca(OH), solution Volume of saturated Ca(OH), solution (L) [OH'] at equilibrium (mol/L) [Ca +21 at equilibrium (mol/L) K, of Ca(OH)2 from the titration Average Kp of Ca(OH), from the titration Molar solubility of Ca(OH), from the titration
Transcribed Image Text:Part 1: Ksp and Molar Solubility of Ca(OH)2 Trial 1 Trial 2 Trial 3 Buret reading, final (mL) 24.2 47.4 64.3 Buret reading, initial (mL) 0.0 24.2 47.4 Volume HCl used (mL) Concentration of standard HCl solution (M) Mole HCl added Mole OH- in saturated Ca(OH), solution Volume of saturated Ca(OH), solution (L) [OH'] at equilibrium (mol/L) [Ca +21 at equilibrium (mol/L) K, of Ca(OH)2 from the titration Average Kp of Ca(OH), from the titration Molar solubility of Ca(OH), from the titration
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