Reaction of nitrous acid in water: HNO2(??) + H2O(?) ⇌ H3O+(??) + NO-(??). The ?a at 25°C is 5.2×10^-4 M
Calculate the value of the equilibrium constant at 25°C for the reaction: HNO2 (??) + OH-(??) ⇌ H3O+(?) + NO-(??)
Reaction of nitrous acid in water: HNO2(??) + H2O(?) ⇌ H3O+(??) + NO-(??). The ?a at...
1. A certain amount if nitrous acid is dissolved in water at 25 celcius. At equilibrium, the pH of the solution is 2.33. What is the concentration of H3O+ and NO2-? 2. Calculate the valye if the equilibriym constant at 25 celcisus for the reaction: HNO2+OH- -> H2O + NO2-
Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2 (aq) + H2O (l) <--------------> H3O+ (aq) + NO2- In which direction will the equilibrium shift if a) NaOH is added? b) NaNO2 is added? c) HCl is added? d) The acid solution is made more dilute?
Nitrous acid, HNO2, has a Ka of 7.1 × 10−4. What are [H3O+], [NO2−], and [OH−] in 0.54 M HNO2?
calculate the value of the equilibrium constant at 25 Celcius, for the reaction: HNO2 + OH- -> H2O + NO2- H3O+ and NO2-= 4.67 x 10^-3 M Ka of HNO2= 7.2 x 10^-4 M
In a 7.50 M nitrous acid (HNO2) solution, calculate (H+). Nitrous acid is a weak acid with K = 4.00 x 10 at 25°C. 3.98 x 102 M-
Consider a buffer solution whose acid component is nitrous acid, HNO2 a) what is a conjugate base component of this buffer? b) write a reaction that takes place when a small amount of H3O+ is introduced to this buffer solution. c) write a reaction that takes place when a small amount of OH- is introduced to this buffer solution
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M
Write the K, expression for an aqueous solution of nitrous acid , HNO2 : Kg The value of K, for nitrous acid is 4.50x104. What is the value of Kb, for its conjugate base, NO2? Submit Answer K, for nitrous acid, HNO2, is 4.50x10-4. Kfor benzoic acid, CH3COOH, is 6.30x10-5. K, for phenol (a weak acid), CH,OH, is 1.00×10-10. What is the formula for the weakest conjugate base? Submit Answer
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∘...
A student determines that an aqueous solution that contains 0.196 M potassium fluoride and 0.206 M hydrofluoric acid, also has an H3O+concentration of 8.48×10-4 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HF(aq) + H2O H3O+(aq) + F-(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K = and A student determines that an aqueous solution that contains 0.365 M potassium nitrite and 0.125 M nitrous...