Please help me answer questions 3, 4, and 5. Please show step by step solutions.

Question

Please help me answer questions 3, 4, and 5. Please show step by step solutions.

Experimental Resuits Trial #1 Trial #2 Trial #3 Initial Burette Reading (ml.) Final Burette Reading (mL) Volume of EDTA solution (mL) Molarity of the EDTA Solution (M) |.ONG (2M |.OIdol2M |.O(2M Moles of EDTA (1 point) Moles of Ca+ (1 point) Volume of Ca(OEH)z solution (ni)0-00ml .00m 10.00m Ca + concentration (M) (2 points) 00 O-ONG13 0.01372 OH concentration (M) (2 points) Experimental Ksp (2 points) |Average Experimental Ksi) (2 points) |"58*16 6.000 lo 0.000613 6.0001222 .000 0.0001(43 0-000322 moi mol mol 05210086 0024 1 924 True hsp

Explanation / Answer

3)

Ksp exprimental = 1.65*10^-5

find solubility in NaOH = 0.3 M

so

Ksp = [CA+2][OH-]^2

assume S = Ca+2

[OH-] = 0.3

so

1.65*10^-5 = S*(0.3)^2

S = (1.65*10^-5) / ((0.3)^2) = 0.00018333333 M

then

Solublity of Ca(OH)2 --> 0.00018333333 M

4)

In water Mg(OH)2 dissociates as,
   Mg(OH)2 ---------> Mg+2 + 2OH-
   Ksp = [Mg+2] [OH-]2
   Ksp = 5*10-11
   Assume that [Mg+2] = X and [OH-] = 2X
  [X] [2X]2 = 5*10-11
  solve for X,
  4X3 = 5*10-11
   [X] = 2.3207*10-4 mol/L = solubility of Mg(OH)2 in water

5)

Cr(OH)3 ----------> Cr+3 + 3OH-
   Ksp = [Cr+3] [OH-]3
   given that [Cr+3] = 4*10-6M
   [OH-] = [3*4*10-6]3 = 1.728*10-15
   Ksp = 4*10-6 *  1.728*10-15 = 6.912*10-21

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