You have a test tube in which the following equilibrium is established.Fe* (aq) + SCN (aq) = FESCN* (ag)Describe how concentrations of Fe*, SCN and FeSCN* will change if a crystal KSCNis added to the mixture above? What would stay constant? Consider a beaker containing a saturated solution of CaF2 in equilibrium withundissolved CaF: (s).(a) If solid CaCla is added to this solution, will the amount of solid CaF2 at the bottomof the beaker increase, decrease or remain the same?(b) Will the concentration of Ca+ ions in solution increase or decrease?

Since, the equilibrium is established so by adding common ion will disturb the equilibrium. We have…

You have a test tube in which the following equilibrium is established. Fe* (aq) + SCN (ag) = FESCN* (aq) Describe how concentrations of Fe*, SCN' and FeSCN+ will change if a crystal KSCN is added to the mixture above? What would stay constant?

You have a test tube in which the following equilibrium is established. Fe* (aq) + SCN (ag) = FESCN* (aq) Describe how concentrations of Fe*, SCN' and FeSCN+ will change if a crystal KSCN is added to the mixture above? What would stay constant?

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

The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Magnesium ion Mg2+(aq) in Molarity at equilibrium? 3.89 x 10-6 4.07 x 10-6 3.47 x 10-6 2.45 x 10-6 2.81 x 10-6 3.28 x 10-6 2.64 x 10-6 3.69 x 10-6 3.01 x 10-6 4.29 x 10-6
Consider the insoluble compound cobalt(II) carbonate, COCO3 . The cobalt(I) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of COCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction For Co(NH3), Kf= 7.7×104. Be sure to specify states such as (aq) or (s). 2+ K =
Given the following reactions and their equilibrium constants,calculate the value for the overall formation constant forAg(NH3)2+. In addition, write the equilibrium expression forthe formation of Ag(NH3)2+.½Ag+(aq) + ½Cl–(aq) ⇋ ½AgCl(s) K1 = 7.45 x 104Ag(NH3)2+(aq) + Cl–⇋ AgCl(s) + 2NH3(aq) K2 = 323Ag+(aq) + 2NH3(aq) ⇋ Ag(NH3)2+(aq) Kf = ?
Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×10¹5. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 2 more group attempts remaining
The equilibrium constant for the acid ionization of mercaptoethanol (HSCH2CH2OH) is HSCH2CH2OH(aq) = H+(aq) + SCH2CH2OH-(aq) k= 1.91 x 10-10 Which of the following is/are true regarding this equilibrium? And why? 1. The reaction is product-favored. 2. The reaction is reactant-favored. 3. Equilibrium lies far to the right. 4. Equilibrium lies far to the left.
When Fe(OH)3 is added to 1.0 M HSCN, the following reaction occurs. Given that the pKa of HSCN is 1.1 and Kf for Fe(SCN)3 is 2.0x10^6, Fe(OH3)3(s)+ 3HSCN(aq)⇌Fe(SCN)3(aq)+ 3H2O(l) a.Calculate K for the reaction. b.Calculate the molar solubility of Fe(OH)3 in 1.0 M HSCN. c.Calculate the equilibrium [HSCN] and [Fe(SCN)3].
The solubility of silver chloride can be increased by dissolving it in a solution containing ammonia. AGCI (s) S Ag * (aq) + Cl ¯ (aq) K 1 = 1.6 x 10 -10 Ag * (aq) + 2NH 3 (aq) S Ag(NH 3) 2 * (aq) K 2 = 1.5 x 10 7 What is the value of the equilibrium constant for the overall reaction? AGCI (s) + 2NH 3 (aq) S Ag(NH 3) 2 * (aq) + CI (aq) K net = ? 1.5 x 10 7 2.4 x 10 -3 3.1 x 10 -3 2.3 x 10 14 2.4 x 107
Write a balanced net ionic equation to show why the solubility of Mg(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). Mg(OH)2(s) + 2HCl(aq) MgCl2(aq) + 2H2O(l) K =
Consider the insoluble compound zinc sulfide, ZnS . The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnS (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×1015. Be sure to specify states such as (aq) or (s). K= + +
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M, [C]=0.0230 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. Kf = 155367729.8 The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.152 M. What is the Ksp of AB? Ksp = ?
Express the equilibrium constant for the following reaction. 2 NH 3(3) = N2g) + 3H2(g) N2][H2]1/3 K = [NH 3]1/2 [NH 316 K N21H219 [NH 312 K = [N2][H2]3 K = [NH3]2 [NH 311/2 K = [N2][H2]l/3
5. At 298 K, the following reaction occurs 2 Fe³+ (aq) + Hg2²+ (aq) = 2 Fe²+ (aq) + 2 Hg²+ (aq) a. What will be the ion concentrations at equilibrium given the following initial concentrations: [Fe³+] = [Hg₂²+] = 0.5000 M; [Fe²+] = [Hg²+] = 0.03000 M Kc = 9.14 x 10-6