[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Explain why the addition of water changes the equilibrium position even though the concentration of water is essentially constant and normally not included in the equilibrium constant expression. What are two functions that water performs in this reaction?

[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Explain why the addition of water changes the equilibrium position even though the concentration of water is essentially constant and normally not included in the equilibrium constant expression. What are two functions that water performs in this reaction?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section14.9: Lewis Acids And Bases

Problem 14.27E

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[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O 3. Does the value of the equilibrium constant (K) for this reaction increase, decrease, or remain the same as the concentration of chloride increases? Explain your answer incorporating the definition of an equilibrium constant.
In the following chemical reaction what is the concentrations of [H3O+] in a solution that is 0.00045 M [Al(H2O)6]3+. Assume that the [Al(H2O)6]3+ dissociates 100% completely and assume 1 Liter of solution. [Al(H2O)6]3+ + 3H2O ↔ [Al(H2O)3(OH)3]2+ + 3H3O+
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The formation of a complex between cobalt (III) cation and six ammonia (NH3) ligands is very favorable (K₁= 2.3 x 1033). Given an initial cobalt concentration of 0.0235 M and an initial ammonia concentration of 0.206 M, what will be the concentration of free cobalt ion (Co3+) at equilibrium? 1.2 x 10-27 M 1.6 x 10-34 M 3.3 x 10-41 M 4.3 x 10-34 M 1.4 x 10-28 M Cobalt (II) carbonate is slightly soluble in water (Ksp = 1.0 x 10-10). In the presence of an excess of ammonia, Co²+ forms a complex with six ammonia ligands that is somewhat favorable (K₁ = 1.3 x 105). What is the value of the equilibrium constant (Koverall) for the overall reaction that occurs? COCO3 (s) +6 NH3 (aq) → Co(NH)32+ (aq) + CO32- (aq) 1.3 x 10-5 3.6 x 10² 7.7 x 10-16 1.3 x 105 1.0 x 10-10
A weak acid, HA, has a pKa = 6.2. If a solution of NaA(aq) is prepared, what does the pH of the solution need to be adjusted to in order to achieve the following ratios of deprotonated to protonated species? 1) [A-] / [HA] = 0.01 2) [A-] / [HA] = 10 3) [A-] / [HA] = 1 4) [A-] / [HA] = 106 Note: NaA is the sodium salt of , the conjugate base of HA. Assume NaA completely dissociates in water.
A) The color of the solution changed from blue to pink, because lowering the temperature increased the collision frequency between CoCl2−4CoCl42−and H2OH2O. B) The color of the solution changed from blue to pink, because cooling caused the equilibrium to shift to form the pink-colored Co(H2O)2+6Co(H2O)62+. C)The color of the solution did not change, because more water was not added to the solution. D)The color of the solution did not change, because heat is not released from this reaction.
2. When a metal complex ion is formed in solution, what are the metal ion and ligands acting as? * O a) The ligand is a Lewis base, and the metal ion is its conjugate acid. O b) The metal ion is a Lewis acid, and the ligand is its conjugate base. c) The metal ion acts as a Lewis base, and the ligand acts as a Lewis acid d) The ligand is a Lewis base, and the metal ion is its conjugate acid.
Using Le Chateliers Principle, aan you help me understand what are the net ionic equations for the reactions below? the overall reaction is: [CoCl4]2– (alc) + 6 H2O (l) ⇌ [Co(H2O)6]2+ (aq) + 4 Cl¯ (aq) Note: ‘alc’ means an alcoholic solution. The ion, [CoCl4]2– (alc), is blue in color and [Co(H2O)6]2+ (aq) is pink. We have a well filled with add 0.10M CoCl2 and add some deioinized water with stirring until a color change from blue to pink (to products). Next, we add a few drops of concentrated HCl and found color change to blue (to reactants).
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An aqueous solution of K2[Pt(OH)6] has a pH greater than 7. Explain this fact by writing an equation showing the Pt(OH)62- ion acting as a Brønsted–Lowry base and accepting a hydrogen ion from water
[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Is this reaction endothermic or exothermic?