22. In a saturated solution of MgF2 at 18°C, the concentration of Mg2* is 2.10 X 103 M. The equilibrium isrepresented by the following equation: MGF2S) = Mg?*+ 2F (aq).Write the expression for thesolubility-product constant, Kgp, and calculate its value at 18°C. Note: Show all calculations, follow therules of significant figures, and box your final answer.

Answered: Image /qna-images/answer/09a36197-a956-41bc-bf22-dad4771e1e03.jpg

22. In a saturated solution of M9F2 at 18°C, the concentration of Mg2* is 2.10 X 10³ M. The equilibrium is represented by the following equation: MGF2(s) = Mg*(aq) + 2F (aq)· Write the expression for the solubility-product constant, Ksp, and calculate its value at 18°C. Note: Show all calculations, follow the rules of significant figures, and box your final answer.

22. In a saturated solution of M9F2 at 18°C, the concentration of Mg2* is 2.10 X 10³ M. The equilibrium is represented by the following equation: MGF2(s) = Mg*(aq) + 2F (aq)· Write the expression for the solubility-product constant, Ksp, and calculate its value at 18°C. Note: Show all calculations, follow the rules of significant figures, and box your final answer.

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

What is the symbolic expression for the equillibrium constant for the reaction: 2C2H6(g) + 7 O2(g) = 4CO2(g)+6H2O(g)?
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. 2.9x10¹5. Be sure to specify states such as (aq) or (s). For Zn(OH)4²-, Kf = K = + Submit Answer + Retry Entire Group 1 more group attempt remaining
1. What is the equilibrium constant expression for the following reaction? (Pay careful attention to the phase indicators!) 2 HCl (g) + Mg(OH)2 (s) ? MgCl2 (aq) + 2 H2O (l)
The reaction of hydrazine (N,H4) with chlorine trifluoride (CIF3) has been used in experimental rocket motors. N2H4(g) + 4/3 CIF3(g)=4 HF(g) + N2(9) + 2/3 Cl,(g) (K) How is the equilibrium constant, K, for this reaction related to K,' for the reaction written this way? 3 N2H4(g) + 4 CIF3(9)= 12 HF(g) + 3 N2(g) + 2 Cl,(g) (K,') O Ko = Kg O K = (K,' )3 O 3 K, = K, O (K = K,
Given the following values of equilibrium constants: (Hg(NH,)4] = Hg²* (aq) + 4NH3 (ag) K = 5.6 x 10-0 HgBr,(s) Hg (ag) + 2Br (aq) K= 6.2 x 10 20 What is the value of the equilibrium constant for the following reaction? HgBr2 (s) + 4NH3(aq) = [Hg(NH,),+ + 2Br (aq)
Write the expressions for K, for the following reactions. In each case indicate whether the reaction is homoge- neous or heterogeneous. (a) 203(g) = 302(8) (b) Ti(s) + 2 Cl2(8) = TIC14(I) (c) 2 C,H,(8) + 2H,0(g) = 2 C,H¿(8) + O2(8)| (d) C(s) + 2 H2(8) = CH4(8) (e) 4 HCI(aq) + Oz(8) = 2 H20(1) + 2 Cl2(8) (f) 2 C3H18(1) + 25 O2(g) = 16 CO2(8) + 18 H20(g) (g) 2 C3H18(1) + 25 O2(8) 16 CO2(8) + 18 H20(I)
For the following reaction: SÜCI; (g) = SbCl3 (9) + Cl2 (g) the equilibrium concentrations for SÜC15, SbCl3, and Cl2 are measured to be 0.55 M, 1.25 M and 0.12 M respectively. What is the value of the equilibrium constant, K, for the reaction? (Give your answer to 2 decimal places. If Canvas removes trailing zeros from your answer it will still be marked correct)
The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service.Solve the following problem:MgF2(s) ⇌ Mg2+(aq) + 2F−(aq)In a saturated solution of MgF2 at 18 °C, the concentration of Mg2+ is 1.21 × 10–3 M. The equilibrium is represented by the preceding equation.(a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 °C.(b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 °C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible.(c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00 × 10–3-M solution of Mg(NO3)2 is mixed with 200.0 mL of a 2.00 × 10–3-M solution of NaF at 18 °C. Show the calculations to support your prediction.(d) At 27 °C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17 × 10–3 M. Is the dissolving of MgF2 in…
How could I find this using the given information ?
Determine the molar solubility for Cr(OH)₃ (Ksp = 6.3 × 10⁻³¹) in an aqueous solution that has a pH of 11.90 at 25 °C. Give an ice table
Consider the following equilibrium reaction: PBr5(g) + 1/2 O2(g) = POB13(g) + Br2(g) Kc = 5.6 x 102 at 512 K Calculate K. for the reaction 2 PBr5(g) + O2(g) = 2 POBR3(g) + 2 Br2(g) at the same temperature. 24 1.1 x 103 280 5.6 x 102 O None of these 3.2 x 105
A student ran the following reaction in the laboratory at 651 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.43×102 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.115 M. Calculate the equilibrium constant, K, she obtained for this reaction. Ke =