We did a lab experiment in class and it was about the Chemical Equilibrium - The

Question

We did a lab experiment in class and it was about the Chemical Equilibrium - The Solubility Product of Ca(OH)2. I believe that the answers I have filled in are correct, but I need help on finding the other parts that are blank. The purpose of the experiment was to tittate calcium hydroxide with EDTA solution.
Additional info: In this experiment we had 10.00 mL of Ca(OH)2 in a flask and were instructed to use the buret that was filled with the EDTA to titrate. We completed 3 trials as seen in the data sheet above. Help would be appreciated, please show work, thanks in advance! Experimental Results Trial #2 Trial #1 Initial Burette Reading (mL) 0 mL Final Burette Reading (mL) Volume of EDTA solution (mL) mL 0.7 lo, l ML Molarity of the EDTA Solution (M) 0. 0 IS98n. O. 015 93 n Moles of EDTA (1 point) Moles of Ca (1 point) Ca concentration (M) (2 points) OH concentration (M) (2 points) xperimental Kop (2 points) Average Experimental Ksp (2 points) Trial #3 lo, 7ml 10 AL

Explanation / Answer

Chemical equation,

Ca2+ + EDTA <===> CaEDTA^2-

From the data table

From trial 1,

moles of EDTA = 1.614 x 10^-4 mol

moles of EDTA = moles of Ca2+

moles of Ca2+ = 1.614 x 10^-4 mol

molarity of Ca2+ solution = moles/L

                                         = 1.614 x 10^-4 mol/0.01 L

                                         = 0.01614 M

molarity of [OH-] = 2 x 0.01614 M

                           = 0.0323 M

Experimental Ksp = [Ca2+][OH-]^2

                             = (0.01614)(0.0323)^2

                             = 1.68 x 10^-5

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