Please check the calculations.
Like if find it helpful
18.) The acid dissociation constant for a we free energy of formation for X (aq) at...
C2 T11HW Question 10 Homework. Unanswered Fill in the Blanks The acid dissociation constant for a weak acid HX is 3.2x10-9 at 25°C. Calculate the standard free energy of formation for X (aq) at 25°C. The standard free energies of HX(aq) and H (aq) are -203.1 kJ/mol and 0, respectively. AG= kJ/mol Unanswered Submit Fullscreen .. C2 TL1HW Question 11 Hmk .Unanswered
The Gibb's Free Energy change (kJ/mol) for the aqueous dissociation of a weak acid at 50.0 °C is-22.5 kJ/mol. What is the acid dissociation constant for that acid? Answer in X.XXex format! 4.41e3
Question 10 10 pts The Gibb's Free Energy change (kJ/mol) for the aqueous dissociation of a weak acid at 50.0 °C is -22.5 kJ/mol. What is the acid dissociation constant for that acid? Answer in X.XXeX format!
The following equation represents the dissociation of propionic acid in water. HC3H502(aq) + H20(1) = H30+(aq) + C3H502 (aq) The value for the acid-dissociation constant for propionic acid (HC3H502) is 1.3x10-5 at 25°C. Calculate the hydronium ion concentration present in a propionic acid solution that has the following equilibrium concentrations. 3.24x10-2 mol/L HC3H502 3.06x10-4 mol/L for propionic acid's conjugate base, C3H5027 The general form of the acid-dissociation constant is Ka = [H30'A ], where Ka is the acid-dissociation constant, [HA]...
HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.055 M in A-(aq)? The temperature is 25oC.
A reaction A(aq) + B(aq) = C(aq) has a standard free-energy change of -3.06 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? How would your answers change if the reaction had a standard free-energy change of +3.06 kJ/mol? O There would be less A and B but more C. All concentrations would be higher. There...
#3 (a) HA (aq) is a weak acid with a dissociation constant, Ka, of 2.0 x 10-15. What is the pH of a 0.04 M solution in A- (aq)? The temperature is 25oC. (b) For the reaction A (g) ⇋ B (g) + C (g), the equilibrium constant is 2 at 25.0oC and 3 at 75.0oC. Making the approximation that ΔH and ΔS do not change with temperature, calculate the value of the equilibrium constant at 50.0oC as well as...
A reactionA(aq) + B(aq) <==> C(aq)has a standard free-energy change of -5.13 KJ/mol at 25℃What are the concentrations of A, B, and C at equilibrium if at the beginning of the reaction their concentrations are 0.30M, 0.40M and 0 M respectively?
A reaction A(aq) + B(aq) = C(aq) has a standard free-energy change of -3.38 kJ/mol at 25°C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and OM, respectively? [A] = [B] = 1C) = How would your answers change if the reaction had a standard free-energy change of +3.38 kJ/mol? There would be no change to the answers. O All concentrations would be...
A reaction A (aq) + B(aq) C(aq) has a standard free-energy change of-5.16 kJ/mol at 25 degree C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? How would your answers above change if the reaction had a standard free-energy change of +5.16 kJ/mol? There would be less A and B but more C. All concentrations would be lower. All...