Consider the following equilibrium. HS^- + HC_2O_4 H_2S + C_2O_4^2-. For oxalic acid the first and...
Consider the following equilibrium, For oxalic acid the first and second acid dissociation constants are 5.6 times 10^-2 and 5.4 times 10^-5, respectively, and for hydrosulfuric acid the first and second acid dissociation constants are 9.5 times 10^-8 and 1.0 times 10^-19, respectively. Calculate the equilibrium constant, K_eq.
need help with both questions 7. Consider the following equilibrium, HS- + HC204- 5 H2S + C202-For oxalic acid the first and second acid dissociation constants are 5.6 x 102 and 5.4 x 10, respectively, and for hydrosulfuric acid the first and second acid dissociation constants are 9.5 x 108 and 1.0 x 10-19, respectively. Calculate the equilibrium constant, Keq. 12. A buffer with pH = 10.15 is to be prepared by addition solid sodium hydrogen carbonate to 1.00 L...
The following equilibrium constants have been determined for oxalic acid at 25 degree C. H_2C_2O_4(aq) rightarrowoverleftarrow H^+(aq) + HC_2O_4^-(aq) K_1 = 6.5 times 10^-2 HC_2O_4^-(aq) rightarrowoverleftarrow H^+(aq) + C_2O_4^2- (aq) K_2=6.1 times 10^-5 Calculate the equilibrium constant for the following rxn at the same temperature. H_2C_2O_4(aq) rightarrowoverleftarrow H^+(aq) + C_2O_4^2- (aq)
Please answer and show all work. thank you!!!!!! 6. The following equilibrium constants have been determined for hydrosulfuric acid at 25°C: H2S(aq)<> H(aq) + HS (aq) K. = 9.5 x 10-8 HS (aq) → H+ (aq) + S2 (aq) K". = 1.0 x 10-19 Calculate the equilibrium constant for the following reaction at the same temperature: H2S(aq) → H(aq) + S2- (aq)
Oxalic acid, H2C2O4 has acid dissociation constants of ?a1=5.90×10−2 and ?a2=6.40×10−5. Calculate the pH and molar concentrations of H2C2O4 , HC2O−4 , and C2O2−4 at equilibrium for each of the solutions. A 0.117 M solution of H2C2O4 A 0.117 M solution of Na2C2O4
Oxalic acid (HOOC-COOH) is a simple diprotic acid. It is used commercially in bleaching straw and leather and removing rust and ink stains. a. Write each dissociation step for the acid including the K values from appendix C. b. What are the equilibrium concentrations of [H2C2O4], [HC2O4- ], and [C2O42- ] in a 0.150M H2C2O4 solution. (Hint: the concentrations of [H2C2O4], [HC2O4- ] are found together and used to find concentration of [C2O42- ].) c. What is the pH of...
Oxalic acid, H2C2O4H2C2O4, has acid dissociation constants of ?a1=5.90×10−2Ka1=5.90×10−2 and ?a2=6.40×10−5Ka2=6.40×10−5. Calculate the pH and molar concentrations of H2C2O4H2C2O4, HC2O−4HC2O4−, and C2O2−4C2O42− at equilibrium for each of the solutions. A 0.2030.203 M solution of H2C2O4H2C2O4. A 0.2030.203 M solution of Na2C2O4Na2C2O4.
Calculate the pH and the equilibrium concentration of S2- in a 7.90×10-2 M hydrosulfuric acid solution, H2S (aq). For H2S, Ka1 = 1.0×10-7 and Ka2 = 1.0×10-19
15.35 The following equilibrium constants have been determined for oxalic acid at 25°C. H.C204(aq) = H*(aq) + HC2O2(aq) K' = 6.5 x 10-2 HC2O2(aq) 2 H +(aq) + C202 (aq) K" = 6.1 x 10-5 Calculate the equilibrium constant for the following reaction at the same temperature. H,C,04(aq) 2 2H+(aq) + C202 (aq) re
*2.4 Consider a 1M water-solution of acetic acid. a) Given the dissociation constant of acetic acid, K=1.75*10--M, calculate the concentration of non-dissociated acetic acid at equilibrium. Hint The dissociation process is described as a first order process relative to each of the components: CH3COOH CH3COO- + H+