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What is Kb for the equilibrium rreacton: CN- + H2O <=> HCN + OH- ? Ka value of 6.23 x10-10
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- 6-82 (Chemical Connections 6C) A solution contains 54 mEq/L ofCI- and 12 mEq/L of HCO3-. If Na+ is the only cation present in the solution, what is the Na+ concentration in milliequivalents per liter?Given the following reactions and equilibrium constants: (1) HCN(g) + OH* — CN- + H₂O (g) K₁ =4.9 x 104 (2) H₂O(g) H¹(g) + OH- K₂ = 1.0 x 10-14 - What will be the equilibrium constant for: HCN(g) → CN- + H* (g) ? um constant 5.9 x 104 4.9 x 10-10 5.0 x 10-10 4.9 x 10-40 4.9 x 1018agy-m ince Mo atalyst- is catal aw (sin tion of di of gas tv int fors of Co₂ find s :3 S PM" marin what! @ 259 -075 10) The following reaction is known as the Fischer Esterification. The equilibrium constant is 1.0. سال H3C H = + CH₂OH H3C CH3 methylacetate + H₂O a) Write the equilibrium equation for this reaction. However, keep H₂O in the equation. b) With an equilibrium constant of 1.0, what is the maximum yield of the methylacetate product? c) Describe how using Le Chatelier's principle one can increase the yield of the reaction by removing water. 8
- Predict the position of equilibrium and explain your choice. 0=1 || The equilibrium is ✔ [Select] product reactant [Select] ||| IV -favored because compound e base.(a) Calculate the percent lonization of 0.00820 M hydrosulfuric acid (K,- 9.5e-08). % lonization - % (b) Calculate the percent lanization of 0.00820 M hydrosulfuric acid in a solution containing 0.0810 M sodium hydrogen sulfate. % lonization = %AH = - 1.2 kcal/mol; Kp = 16 nM OH 1 НО AH = - 6.0 kcal/mol; Kp = = 76 nM OH HOllio AH = - 5.5 kcal/mol; Kp = 0.5 nM OH 3 (ii) What is the significance of Kp? Hence, arrange the three molecules in terms of decreasing affinity to their target. O=
- (a) Prepare the log C-pH diagram for Fe(OH);3 precipitation. Use the following equilibrium reactions. Fe(OH)3, + 3H Fe(OH);,3 + 2H" Fe(OH)3, + H Fe(OH):,s - Fe* + 3H:O - Fe(OH)* + 2H;O - Fe(OH)2* + H;O - Fe(OH); - Fe(OH); + H Ko = 1035 K1 = 1015 K2 = 10-25 K3 = 10120 K4 = 10*185 %3D %3D Fe(OH)3, + H;O %3D Start your answer by writing the equilibrium equation of each reaction and show the detailed mathematical manipulation steps on how you plot each of the equilibrium lines. Use the given grid paper and do not use spreadsheet software. Note that the given equilibrium constants are different from those used in the lecture.The pka of ethanoic acid, (CH3COOH) (0.1 M), is 2.6 at 25°C. Write the balanced chemical equation for the ionisation of CH3COOH. a. b. C. Ka = Write the expression for the equilibrium constant, Ka Complete the initial-change-equilibrium table for the species in the reaction Conc (mol L-1) CH³COOH CH³COO¯ H³O+ Initial 0.100 Change Equilibrium CH3COOH + H3O+ 0.1-x +X CH3COO- 0 OH- [CH3COOH] [CH3COO-] + 0.2 -0.1 -X H3O+ H₂O H₂OCalculate AHo for the reaction: 20:Helg) + 70:(g) 4 CO(g) + 6 H2O(g) If. C:Halg) + 302(g)-2 COg) + 2 H2O (g) CaHi(g) + Hz(g) - CzHs(g) H2(g) + % Oz(g) - H2O(g) AH = -1323 kJ AH =-137 KJ AH = -242 kJ
- Identify the correct equation for the equilibrium constant K, for the weak acid dissociation of acetic acid. HC,H;O, (aq) + H,0 (1) H;0+ (aq) + C,H;O,¯ (aq) Select one: [H,O*|[C,H,0, [HC,H3O2|[H2O] HC,H,O,] [H,O"|C,H,0, K. K. [HC,H;O2|[H2O) [H;O*|[CH,O2 K = O Ka = [H,O*|[C,H,0,) [HC;H,O2]The following equilibrium constants have been determined for hydrosulfuric acid at 25oC ; H2S(aq) ↔ H+(aq) + HS-(aq) Kc’ = 9.5x10-8 HS-(aq) ↔ H+(aq) + S2-(aq) Kc’’ = 1.0x10-19 Calculate the equilibrium constant Kc for the following reaction at the same temperature. H2S(aq) ↔ 2H+(aq) + S2-(aq) 8x10-18 5x10-27 4x10-16 8x10-25 9x10-24For the reaction 4 PH; (g) = 6 H,(g) + P¿(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H,] = 0.370 M, and [P] = 0.750 M. What is the equilibrium constant for this reaction? K.