Calculate the solubility of CuX(Ksp=[Cu2+][X2−]=1.27×10−36) in a solution that is 0.120 M in NaCN.
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Calculate the solubility of CuX(Ksp=[Cu2+][X2−]=1.27×10−36) in a solution that is 0.120 M in NaCN.
Part A Calculate the solubility of CuX (Kg= Cu2+]x-1.27 x 10-3) In a solution that is 0.120 M in NaCN Express your answer using two significant figures м Submit Reauest Anewer Provide Feedback
Calculate the molar solubility of CuX(Ksp=1.27×10−36) in the following. 0.28 M CuCl2 Express your answer using two significant figures.
Calculate the molar solubility of CuX (K_sp = 1.27 times 10^-36) in each of the following. 0.28 M CuCl_2 0.23 M Na_2X
a. 0.23 MM CuCl2 b. 0.22 MM Na2X Calculate the molar solubility of CuX (Ksp = 1.27 x 10–36) in each of the following.
Iculate the molar solubility of MX (Ksp = 1.27 x 10-36) in: 68. Calculate the molars a. pure water b. 0.25 M MCI, c. 0.20 M Na X lata tha molar cal..
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5 points) A substance MX has a Ksp of 1.27 x 10-36. a. What is it's molar solubility in pure water? (hint: ICE Table-reminder: MX(s) will fall out of your equilibrium expression) b. What is it's molar solubility in 0.25 MBrz? (hint: ICE Table-but what is M2+ initial?)
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