22 0For the aqueous+[Ni(NH3) 6 ]²* complex K₁ = 5.50 × 10³ at 25 °C.Suppose equal volumes of 0.0062M Ni(NO3), solution and 0.78M NH3 solution are mixed. Calculate the equilibrium.2+molarity of aqueous Ni²+ ion.Round your answer to 2 significant digits.2☐ M☐ x10☑EلهAག IncorrectFirst Step: Your answer is incorrect.?+In aqueous solution the Ag ion forms a complex with two cyanide anions.Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex.Under that, write the balanced chemical equation for the first step in the formation of the complex.K₁=[Ag(CN)2]Ag HO[[^8 (10)]] [CN]*TIE000Write the First Step:☑First Step:[Ag(H₂O)(CN)](aq) + CN˜¯(aq) → [Ag(CN)2]¯ (aq) + H₂O(1)|ローロ☑GBo18Ar

Alswer-1How to approach this problem:Since, formation constant is very large, therefore, in order to…

Answered: 0 For the aqueous + [Ni(NH3) 6 ]²*…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.91QE

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A Boric acid and glycerin form a complex B(OH)3(aq) + glycerin(aq) B(OH)3 glycerin(aq) with an equilibrium constant of 0.90. If the concentration of boric acid is 0.10 M, how much glycerin should be added, per liter, so that 60.% of the boric acid is in the form of the complex?
The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide salt? [Ksp for Mg(OH)2 = 8.9 1012.]
Each pair of ions below is found together in aqueous solution. Using the table of solubility product constants in Appendix J, devise a way to separate these ions by adding a reagent to precipitate one of the ions as an insoluble salt and leave the other in solution. (a) Cu2+ and Ag+ (b) A13+ and Fe3+
Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr2O72 , and the yellow chromate ion, CrO42 . (See the following photos.) The equilibrium reaction between the two ions is Cr2O72(aq)+H2O(l)2CrO42(aq)+2H+(aq) Explain why orange dichromate solutions turn yellow when sodium hydroxide is added.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Magnesium hydroxide, Mg(OH)2, is the active ingredient in die antacid TUMS and has a Ksp value of 8.9 1012. If a 10.0-g sample of Mg(OH)2 is placed in 500.0 mL of solution, calculate the moles of OH ions present. Because the Ksp value for Mg(OH)2 is much less than 1, not a lot of solid dissolves in solution. Explain how Mg(OH)2 works to neutralize large amounts of stomach acid.
Each pair of ions below is found together in aqueous solution. Using the table of solubility product constants in Appendix J, devise a way to separate these ions by adding a reagent to precipitate one of the ions as an insoluble salt and leaving the other in solution. (a) Ba2+ and Na+ (b) Ni2+ and Pb2+
Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.
You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
When 250 mg of SrF2, strontium fluoride, is added to 1.00 L of water, the salt dissolves to a very small extent. SrF2(s)Sr2+(aq)+2F(aq) At equilibrium, the concentration of Sr2+ is found to be 1.03 103 M. What is the value of Ksp for SrF2?
You will often work with salts of Fe3+, Pb2+, and Al3+ in the laboratory. (All are found in nature, and all are important economically.) If you have a solution containing these three ions, each at a concentration of 0.10 M, what is the order in which their hydroxides precipitate as aqueous NaOH is slowly added to the solution?
Calcium hydroxide, Ca(OH)2, dissolves in water to the extent of 1.78 g per liter. What is the value of Ksp for Ca(OH)2? Ca(OH)2(s)Ca2+(aq)+2OH(aq)

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