lodine is sparingly soluble in pure water. However, itdoes 'dissolve' in solutions containing excess iodide ionbecause of the following reaction:|¯ (aq) + 1₂(aq) --> 13¯ (aq) K = 699.For each of the following cases calculate the equilibriumratio of [13] to [1₂].2.00×10-2 mol of l2 is added to 1.00 L of 2.00×10-¹ M KIsolutionThe solution above is diluted to 6.00 L.

The equilibrium constant (Keq) of a reaction is the ratio of the product of the molar concentration…

lodine is sparingly soluble in pure water. However, it does 'dissolve' in solutions containing excess iodide ion because of the following reaction: I¯ (aq) + 1₂(aq) --> 13¯ (aq) K = 699. For each of the following cases calculate the equilibrium ratio of [13] to [1₂]. 2.00×10-² mol of l2 is added to 1.00 L of 2.00×10-¹ M KI solution The solution above is diluted to 6.00 L.

lodine is sparingly soluble in pure water. However, it does 'dissolve' in solutions containing excess iodide ion because of the following reaction: I¯ (aq) + 1₂(aq) --> 13¯ (aq) K = 699. For each of the following cases calculate the equilibrium ratio of [13] to [1₂]. 2.00×10-² mol of l2 is added to 1.00 L of 2.00×10-¹ M KI solution The solution above is diluted to 6.00 L.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Solve it please...
Which of the following is more likely to precipitate the hydorxide ion?(a) Cu(OH)2(s) = Cu2+(aq) + 2OH-(aq) K = 1.6 x 10-19 (a) Ca(OH)2(s) = Ca2+(aq) + 2OH-(aq) K = 7.9 x 10-6
Determine the concentrations of each zinc-containing species in a solution saturated with solid Zn(OH), and having a fixed OH concentration of 6.1 x 107 M. The equilibrium constants for the equilibria that occur in the solution are given in the table. Zn(OH)₂ (s) Ksp = 3.0 × 10-16 [Zn²+] = [Zn(OH)*] = [Zn(OH)]= [Zn(OH)]= Zn(OH)* (aq) P₁ = 2.5 x 104 Zn(OH), (aq) B3 = 7.2 x 10¹5 Zn(OH)2 (aq) B4 = 2.8 x 10¹5 M M M M
The formation constant* of [M(CN)4]2− is 7.70×1016, where M is a generic metal. A 0.130 mole quantity of M(NO3)2 is added to a liter of 0.890 M NaCN solution. What is the concentration of M2+ ions at equilibrium?
1. Which salt would you expect to dissolve more readily in acidic solution cobalt (II) fluoride, CoF2 or cobalt (II) iodide, Col2? Explain. (Write all possible reactions for both salts.) 2. What is the concentration of Co2+ (aq) ion in a 0.010 M Co(C1O4)2 (soluble salt) solution that also contains 1.57 M NH3? Kf for [Co(NH3)6] 2+ =1.3 x10³. 3. What is the molar solubility of silver bromide AgBr in a 0.25 M solutions of sodium bromide NaBr? (Ksp of silver bromide is 5.0 x 10-13). Which is more soluble AgBr or AgBr with the addition of NaBr?
0.1 mL of 1.0 M Cd(NO3)2 is added to 1.0 L of 0.5 M NH3. Relevant equilibria in the solution are:Cd(OH) 2 (s) ⇌ Cd 2+ (aq) + 2OH- (aq) Ksp = 5.9 x 10-15Cd 2+ (aq) + 4NH 3 (aq) ⇌ Cd(NH3) 4 2+ Kf = = 1.0 x 107NH 3 (aq) + H 2 O ⇌ NH 4+ + OH- Kb = 1.8 x 10-5a) What is [OH-] in the ammonia solution (before addition of cadmium nitrate). What isthe concentration of NH3 considering that by 0.5 M NH3 solution is meantthe sum of the concentrations of NH3 and NH4+?b) Will the OH concentration change significantly when you add to the solution thatcontains Cd(NO3)2. A good justification in words is enough.c) Calculate the equilibrium constant for the reaction where Cd(OH)2(s) is converted toCd(NH3) 42+
Write a balanced net ionic equation to show why the solubility of AIPO4 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Consider only the FIRST STEP in the reaction with strong acid. Be sure to specify states such as (aq) or (s). AIPO (s) + 3H₂O*(aq) K= Al³+ (aq) + H₂PO (aq) + 3H₂O(1)
Calculate the concentration of ammonium ion that is required to prevent the precipitation of Mg(OH)2 in a solution with [Mg2+] = 0.10 M and [NH3] = 0.10 M.
Calculate the concentration of silver in a solution at equilibrium when 15.0 mL of 0.20 M K2CrO4 is added to 30.0 mL of 0.100 M AgNO3. Will the precipitation of Ag2CrO4 be quantitative? A= 5.8 x 10-6 M, yes it is quantitative
The formation constant of [M(CN), is 5.30 x 1018, where M is a generic metal. A 0.130 mole quantity of M(NO3) is added to a liter of 0.490 M NaCN solution. What is the concentration of M+ ions at equilibrium? IM2+1- M
Solid Ag2CO3 is added to water until no more solid Ag2CO3 dissolves. What is the silver ion concentration for the saturated solution of Ag2CO3, if the Ksp for Ag2CO3 is 8.39x10-12? (Ignore any ion hydrolysis.) 4.06 x 10-4 M 2.03 x 10-4 M 2.90 x 10-6 M 1.28 х 104 м 2.56 x 10-4 M None of these
The equilibrium concentration of sulfide ion in a saturated zinc sulfide solution is M. (Assume that Ksp (ZnS) = 2.0 × 10-25.)