Question 12 Establish the following value of KD. v KD = 0.56 A. The concentration is higher in the Aqueaous layer v KD = 1.2 B. The concentration is equal to both Aquaous and organic layer v KD = 1 C. The concentration is higher in the organic layer v Kp = 0.35
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- Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.What is the solubility, in moles per liter, of Fe(OH)2 (Ksp=6.5x10-16) in 0.0569 molar NaOH solution? Report answer in scientific notation with 2 places past the decimal point.slove Part BFor the same procedure described in the chemical equilibrium lab handout for determining K, 27.0 mL of organic solution was added to 65.0 mL of KI aqueous solution at 317.1 K. Both the aqueous and organic solutions were prepared at 298.15 K with the apparent concentration of 0.0796 M for the I-(aq) and 0.0065 for the I2(org) solutions, respectively. After mixing these immiscible solutions, the final concentration of I2 in the organic layer was determined to be 0.0006 M through UV-Vis spectroscopy. In a separate experiment, the partition coefficient was found to be k = 0.01 at 317.1 K. a) Determine the approximate equilibrium constant, K, without making any temperature correction, for the reaction: I2(aq) + I-(aq) ⇌ I3-(aq) at 317.1 K. K = 5294.4 b) Now, make the temperature correction for volume expansion in the calculation of K assuming the solvent is Cyclohexane. What is the percentage error for using the non-corrected K rather than the corrected K?
- If 30.0 mL of 0.10 M AgNO3 is added to 60.0 mL of 0.10 M Na2SO4, will Ag2SO4 precipitate? The Ksp of Ag2SO4 is 1.2 x 10-5. Select one: a. Yes. The dissolution equilibrium must shift to the left, so precipitation occurs. b. Yes. The dissolution equilibrium must shift to the right, so precipitation occurs. c. Yes. The dissolution equilibrium does not shift, so precipitation occurs. d. No. The dissolution equilibrium must shift to the left, so precipitation does not occur. e. No. The dissolution equilibrium must shift to the right, so precipitation does not occur. f. No. The dissolution equilibrium does not shift, so precipitation does not occur.The solubility of Ni(OH)2 in a pH = 7.64 solution is___. Ksp Ni(OH)2 = 1.6 × 10-16. Enter the result in scientific notation to 1 decimal. e.g. enter 5.6x10-5 as 5.6E-5.What is the solubility of La(IO3)3 in a solution that contains 0.150M of La3+ ions? Ksp of La(IO3)3 is 7.5x10^-12
- Ksp for AgCl is 1.77 × 10-10 and Kf for Ag(NH3)2+ is 1.7 × 107. Is AgCl more or less soluble in ammonia compared to pure water? Explain.A) The generic metal hydroxide M(OH)2 has a ksp= 5.25x10^-12 what is the solubility of M(OH)2 in pure water? B) what is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2 ? (Please type answer note write by hend)5.1 Calculate the solubility of CaF2 (g/L) in pure water. Show full reasoning. DATA: Ksp = 3.9 x 10^-11
- The solubility of Ni(OH)2 in a pH = 10.64 solution is___. Ksp Ni(OH)2 = 1.6 × 10-16Calculate the solubility of Ba(IO3)2 in pure water, Ksp=1.5x10^-9. Then calculate the solubility of the same Ba(IO3)2 in a 0.0025M Al(NO3)3 solution. Assume there is no other interatcion between any of the ionic componets of the 2 molecules. (do an activity coeffiecient problem using the neatest u value to determine f from the table)A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). What is the identify of the solid species? Write out the balanced equation for the solubility of the insoluble solid. Uses physical state symbols, an equal sign instead of a reaction arrow, and spaces where necessary. Example: (AgCl(s) = Ag+(aq) + Cl-(aq)) What is the value of the Qsp? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). THIS IS PART 1 WILL POST OTHER QUESTIONS AS PART 2