It is found that up to 0.0110 g of SrF2 dissolves in 100 mLof aqueous solution at a certain temperature. Determinethe value of Ksp for SrF2.( PREV12Based on the set up of your lCE table, construct the expression forKsp and then evaluate it. Do not combine or simplify terms.KspCRESET[0][0.0110][8.76 x 10-1[8.76 x 10-4][1.75 x 10-41[1.75 x 10][0.0110]?[8.76 x 10-8.76 x 10-5(8.76 x 10-5 -[8.76 x 10-41 [1.75 × 10-41[1.75 х 10-4 +2x[1.75 x 101[x][2x]?(1.75 x 10-4 -2x2.68 x 10-91.53 x 10-62.68 x 10 12 It is found that up to 0.0110 g of SrF2 dissolves in 100 mLof aqueous solution at a certain temperature. Determinethe value of Ksp for SrF2.12NEXT>Based on the given values, fill in the ICE table to determineconcentrations of all reactants and products.SFF2(s)Sr** (aq)2 F (aq)+Initial (M)Change(М).Equilibrium|(M)RESET0.01108.76 x 10-58.76 x 10-41.75 x 10-41.75 x 103-0.0110-8.76 x 10-5-8.76 x 10-4-1.75 x 10-4-1.75 x 103+x+2x-2х-x1.75 x 10-4 +2x1.75 x 10-4 -2x8.76 x 10-5 +8.76 x 10-5 - x

Answered: Image /qna-images/answer/878b2728-ce40-4e87-8d04-89a8af301932.jpg

1 2 he set up of your ICE table, construct the expression for en evaluate it. Do not combine or simplify terms. sp CRESET [8.76 x 10-] [8.76 x 104] [1.75 × 10-] [1.75 × 10] [0.0110]? [8.76 x 10-1 (8.76 х 10-5 + x] (8.76 x 10-5 - x] (1.75 x 10-4 + 2x [1.75 x 1012 [x] [2x]? 1.53 x 10-6 2.68 x 10-12 II II

1 2 he set up of your ICE table, construct the expression for en evaluate it. Do not combine or simplify terms. sp CRESET [8.76 x 10-] [8.76 x 104] [1.75 × 10-] [1.75 × 10] [0.0110]? [8.76 x 10-1 (8.76 х 10-5 + x] (8.76 x 10-5 - x] (1.75 x 10-4 + 2x [1.75 x 1012 [x] [2x]? 1.53 x 10-6 2.68 x 10-12 II II

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.ACP

See similar textbooks

Similar questions

Write the expression of the reaction quotient for the ionization of HOCN in water.
Write the mathematical expression for the reaction quotient, QC, for each of the following reactions (a) N2(g)+3H2(g)2NH3(g) (b) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (C) N2O2(g)2NO2(g) (d) CO2(g)+H2CO(g)+H2O(g) (e) NH4CI(s)NH3(g)+HCI(g) (f) 2Pb( NO3)2(s)2PbO(s)+4NO2(g)+O2(g) (g) 2H2(g)+O2(g)2H2O(g) (h) S8(g)8S(g)
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
What are homogeneous equilibria? Heterogeneous equilibria? What is the difference in writing K expressions for homogeneous versus heterogeneous reactions? Summarize which species are included in the K expression and which species are not included.
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
12.42 The following reaction is in equilibrium in lake water: HCO,_(aq) + H+(aq)«=*H,CO,(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. NaHCOj is added to the lake. H,CO}is added. NaOH is added.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.