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Chemistry
- 34. For a generic acid equilibrium: HA (aq) H*(aq) + A (aq) which of the following statements are true? (a) If you add a strong acid to a solution of HA that is at equilibrium, the concentration of A- would decrease. (b) If you add a strong acid to a solution of HA that is at equilibrium, the concentration of HA would decrease. (c) If you a strong acid to a solution of HA that is at equilibrium, the pH of the solution would increase. (d) The equilibrium constant for this reaction changes as the pH changes. (e) If you add a strong acid to a solution of HA that is at equilibrium, the concentration of H* of the solution would decrease.arrow_forwardWhich of the following statements is FALSE? When K>> 1, the forward reaction is favored and essentially goes to completion. When K= 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium. O When K1 implies that the reaction is very fast at producing products. None of the above.arrow_forwardFor the equilibrium: A ↔ B, if [A]o = 0.162, [B]o = 0.569, and Keq = 47.8, what are [A]eq and [B]eq? Only show the algebraic expression with final [A]eq and [B]eqarrow_forward
- C=a4bc46ac4 Part A X Given the two reactions 1. H₂S(aq) = HS (aq) + H+ (aq), K₁=9.46x10-8, and 2. HS- (aq) = S²-(aq) + H+ (aq), K2 = 1.31x10-19, what is the equilibrium constant Kfinal for the following reaction? DO Enter your answer numerically. ► View Available Hint(s) Kfinal Submit W LIVE ΑΣΦ MacR Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions Contact Us D P Pearson zoom S² (aq) + 2H+ (aq) = H₂S(aq) t O ? Reviewarrow_forwardCalculate Kp for the following reactions at the indicated temperature. (a) H₂(g) + 1₂(g) 2 HI(g) K = 61.0 at 664 K Кр (b) NH3(g) + HCI(g) ? = NH4CI(S) K = 92.6 at 587 K Кр =arrow_forwardGiven the following information: N2 (g) + 3H2 (g) ⇄ 2NH3 (g) Kc = 1.8x10-9 2H2 (g) + O2 (g) ⇄ 2H2O(g) Kc = 3.6x10-8 2N2 (g) + 2O2 (g) ⇄ 4NO(g) Kc = 2.0x1011 What is the equilibrium constant for the reaction 4NH3 (g) + 5O2 (g) ⇄ 4NO(g) + 6H2O(g) a) 3.65x1021 b) 5.87x104 c) 9.82x1015 d) 2.88x106 e) 5.56x108arrow_forward
- AP 298K, the equilibrium constant for the following reaction is 7.90x10-5: H¿C¿H,O6(aq) + H2O=H;0*(aq) + HC,H,O6 (aq) The equilibrium constant for a second reaction is 1.60x10-12: HC;H,O6 (aq) + H2O=H;0*(aq) + CgH¿O6²(aq) Use this information to determine the equilibrium constant for the reaction: H,CGH,O6(aq) + 2H2O=2H3O*(aq) + C6H&O6²(aq) K =arrow_forwardConsider the following equilibrium reaction: 2 CH3OH + CH2O ⇌CH2(OCH3)2+ H2O ΔH = + 46 indicate the direction that the equilibrium will shift when the following changes are made.(No states are provided because the solvent for the reaction is not water, so aq for aqueous would not be appropriate.) (a)Concentration of CH3OH increases (b)H2O is removed from the reaction (c)Reaction is heatedarrow_forwardIndicate whether the following reactions are reactant favored or product favored? (a)A (aq) ⇌B (aq) Keq= 1.9 x 10 –5 (b)A (aq) ⇌B (aq) + C (g) Keq= 6.3 x 10 2arrow_forward
- AgBr(s) ⇄ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13Ag+(aq) + 2NH3(aq) ⇄ Ag(NH3)2+(aq) Kf = 1.5 x 107 When NH3 is added to AgBr(s), a combination of these reactions result:AgBr(s) + 2NH3(aq) ⇄ Ag(NH3)2+(aq) + Br-(aq)What mass of AgBr will dissolve in a 5.0 L container of 2.7 M NH3 solution? * 8.6×100 g * 2.8×10-2 g * 5.2×100 g * 9.2×10-3 g * 4.6×10-2 garrow_forwardWrite the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 HCN (aq) + H20(1) =H30+(aq) + CN¯ (aq) K =-arrow_forwardThe acetate ion, CH3COO–, reacts with water as a weak base: CH3COO–(aq) + H2O(l) ⇄ CH3COOH(aq) + OH–(aq), with K = 5.7 x 10-10 at 25°C. If sodium acetate were dissolved in water to make a 0.35 M solution, what would be the resulting concentration of OH–? (M) (no scientific notation)arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning