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)
Given the following acid dissociation constants, Ka (HNO2) = 4.0 x 10-4 Ka (HCN) = 4.0...
HNO2 has an acid dissociation constant of Ka = 4.0 x 10-4. What is the pH of a 0.25 M NO2- solution? a. 2.00 b. 4.30 c. 8.40 d. 10.25 e. 14.00
For the following equation: The Ka value of HNO2 is 4.0 x 10-4. If the equilibrium concentration of HNO2 is 0.54 M. what is the equilibrium concentration of NO2/H30? 2 points HNO, + H, O NO + H20+ Your answer
If nitrous acid (HNO2) has a Ka 4.0 x10-4 at 25 degrees C, what is the percent dissociation of nitrous acid in a 0.40 M solution?
The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to reference(Pages 833 - 836) Section19.7 while completing this problem. Part A Write the chemical equation for the equilibrium that corresponds to Ka. Write the chemical equation for the equilibrium that corresponds to . H+(aq)+NO2−(aq)⇌HNO2(aq) HNO2(aq)⇌H+(aq)+NO2−(aq) HNO2(aq)⇌H−(aq)+NO2+(aq) HNO2(aq)+H+(aq)⇌H2NO2+(aq) HNO2(aq)+H−(aq)⇌H2NO2+(aq) Part B Using the value of Ka, calculate ΔG∘ for the dissociation of nitrous acid in aqueous solution. Express your answer using three significant figures. ΔG∘...
QUESTION 12 Based on the acid dissociation constants (Ka) given, which of these acids is the weakest? о HNO2 (ka = 5.1 x 10-4) NH4+ (Ka = 6.3 x 10-10) HCO3- (Ka = 5.0 x 10-11) = CH3COOH (Ka 1.7 x 10-5) О H2PO4- (Ka = 6.3 x 10-8)
4 3 points Consider the given acid ionization constants listed below, identify the strongest conjugate base: Compound HNO2 HCHO2 HCIO HCN Ka 4.6x104 1.8x10-4 2.9x10-8 4.9x10-10 CN CIO CHO2 NO2
(1) Given the following information: hydrocyanic acid HCN Ka = 4.0×10-10 diethylamine (C2H5)2NH Kb = 6.9×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium will the reactants or products be favored? (3) Will the pH of the resulting solution be greater than, less than, or roughly equal to 7?...
Use the following acid ionization constants to identify the correct decreasing order of base strengths for the conjugate bases. HF: Ka = 7.2 ´ 10-4 HCN: Ka = 6.2 ´ 10-10 HNO2: Ka = 4.5 ´ 10-4 A. NO2- > F->CN- B. CN- > NO2- > F- C. F- > NO2- > CN- D. NO2- > CN- > F- E. F-> CN- > NO2- F. CN- > F->NO2 -
#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.
Use the following table to answer question below. ка Acid HCN HNO2 HCHO2 HCIO 4.0 x 10-10 4.5 x 10-4 1.8 x 104 3.0 x 10-8 Which one of the following solutions will have the lowest pH? a) 1.0 MHCN b) 1.0 M HNO2 c) 1.0 MHCHO2 d) 1.0 MHCIO