The following equilibrium constants have been determined for oxalic acid at 25 degree C. H_2C_2O_4(aq) rightarrowoverleftarrow...
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
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)
Consider the following equilibrium. HS^- + HC_2O_4 H_2S + C_2O_4^2-. 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.
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.
What is the pH of a solution of 0.750 M KH2PO4, potassium
dihydrogen phosphate? thanks!!
At 25 C phosphoric acid, H3PO4, has the following equilibrium constants: H30+ (aq) + H2 PO4 (aq) H30+ (aq) + HP042-(aq) Kal 7.5 x 10-3 Ka2=6.2×10-8 Kas4.2 x 10-13 H, PO4 (aq) + H20(1) H,PO4-(aq) + H2O(1) 근 HPO(a)+H2O()HO (a)P (aq) ▼ Part A
At 25 C phosphoric acid, H3PO4, has the following equilibrium constants: H30+ (aq) + H2 PO4 (aq) H30+ (aq) + HP042-(aq)...
It has been found that in acid solution (greater than 1 M H^+) the rate expression for the reaction of H_2O_2 with I' is of the form rate = k_2[H_2O_2][T] where k_2 = 0.25 L^2 mol^-2 s^-1 at 25 degree C Therefore the rate law over the whole range of acidity from very acid solutions to a neutral solution is given by a two-term rate expression: rate = k_1[H_2O_2)[I^-] + k_2[H_2O_2)[I^-)[H^+) where k_j has the value of 0.0115 L mol'1...
Consider the following reaction at 25 degree C: 2HNO_3 (aq) + NO(g) rlhar 3 NO_2(g) + H_2O(l) Calculate Delta G degree rxn using the following information HNO_3 (aq) NO(g) NO_2(g) H_2O(l) Delta H^degree (kJ/mol) -207 91.3 33.2 -285. 8 S^degree (J/mol K) 146 210.8 240.1 70.0 Calculate the value of the equilibrium constant, K, at 25 degree C At 25 degree C does the above reaction favor reactant or product formation? What evidence supports your conclusion? Procedure: Obtain the five...
The vapor pressure of water at 25 degree C is o.0313 atm. Calculate the values of K_p and K_c at 25 degree C for the equilibrium: H_2O (l) H_2O(g). Vinegar contains acetic acid, a weak acid that is partially dissociated in aqueous solution: CH_3COOH(aq) H^+(aq) + CH_3CO^-_2 (aq) a) Write the equilibrium constant expression for K_c. b) What is the value of K_c if the extent of dissociation of 1.0 M CH_3COOH is 0.42%? Determination of an Equilibrium Constant
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 standard reduction potentials have been determined for the aqueous chemistry of ytterbium: Yb3+(aq) + e- -----> Yb2+(aq) E° = -1.050 V Yb2+(aq) + 2e- -----> Yb(s) E° = -2.760 V Calculate the equilibrium constant (K) for the disproportionation of Yb2+(aq) at 25 °C. 3Yb2+(aq) <----->Yb(s) + 2Yb3+(aq) K =