QUESTION 1 The Ka for HCHO2 is 1.77 x 10-4 What is the value of the...
QUESTION 4 The Ka of HCHO2 is Ka=1.8 x 10-4. What is the value of Kb for CHO2"? Please enter answer in format 1E-2
A buffer solution is to be formed using HCHO2 and NaCHO2. Ka for HCHO2 is 1.77 x 10-4. a. Find the mass of NaCHO2 that must be dissolved in 250. mL of 1.40 M of HCHO2 to prepare a buffer solution with pH = 3.36. b. What will be the pH of the solution following the addition of 15.0 mL of 0.0100 M NaOH?
#4 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.061 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.14 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
What is the hydronium concentration of a 0.0895 M formic acid, HCHO2, solution. Ka (HCHO2) = 1.8 x 10-4
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.066 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.36 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.065 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.00 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.068 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.95 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.065 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.14 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
Given the following acid dissociation constants, Ka (HNO2) = 4.0 x 10-4 Ka (HCN) = 4.0 x10-10 determine the equilibrium constant for the reaction below. HCN(aq) + NO2 - (aq) CN- (aq) + HNO2(aq)
9) What is the H+ ion concentration in a 4.8 x 10–2 M KOH solution? A) 4.8 x 10–2 M B) 1.0x 10–7 M C) 2.1 x10–13 M D) 4.8 x 10–11 M 10) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-? A) HA (aq) + H2O (l) H2A+ (aq) + OH-(aq) B) A- (aq) + H3O+ (aq) C) HA (aq) + OH- (aq) H2O (l) + H+ (aq) HA (aq) + H2O...