Complete the following table and answer the questions, showing all of your calculations. Trial Equivalence point (mL) 1 10.5 ml 2 10 ml 3 11.8 ml Questions: 1. Calculate the [OH-] in the saturated solution from the results of your titrations. 2. Calculate the [Ca2+] in the saturated solution. 3. Calculate the Kp for calcium hydroxide. 4. Find the accepted value of the Kp for calcium hydroxide and compare it with your value. Discuss the discrepancy and suggest possible sources of experimental error.

C Determine the pH of each solution at the equivalence point. pH (NaOH titrant) pH (Ca(OH)2 titrant) Submit =

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Determine the [H3O+H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2HCH3CO2H (HAc), is 4.745. You will also need this information in your post-lab. It is highly suggested you write these calculations down (both unrounded and rounded values) to use later. Solution 1.10 M Acetic Acid (mL) 0.900 M Sodium acetate (mL) [H3O+H3O+] (M) 1 8.00 2.00 Solution 1 Concentration 2 7.00 3.00 Solution 2 Concentration 3 6.00 4.00 Solution 3 Concentration 4 5.00 5.00 Solution 4 Concentration 5 4.00 6.00 Solution 5 Concentration 6 3.00 7.00 Solution 6 Concentration 7 2.00 8.00 Solution 7 Concentration 8 1.00 9.00 Solution 8 Concentration Solution 1 Concentration:   M Solution 2 Concentration:   M Solution 3 Concentration:   M Solution 4 Concentration:   M…

Calculate the pH of NH3/NH4Cl 1- The 0.2M NH3/0.2M NH4Cl buffer.  2- After the addition of 0.08 mol NaOH Given: Ka (NH4+/NH3) = 5.6 * 10-6

Identify the equivalence point volume (mL) of NaOH from the titration curve shown. • 14 6.0 mL 34 mL 15 mL 8.0 mL O 27 mL volume of NaOH added (mL)