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
HNO2 --> H+ and NO2-
a)
then the conjugate base is NO2-
b)
H3O+ + NO2- --> HNO2 + H2O
c)
OH- + HNO2 --> H2O + NO2-
Consider a buffer solution whose acid component is nitrous acid, HNO2 a) what is a conjugate...
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 nitrous acid/sodium nitrite conjugate pair has been chosen to prepare a buffer solution. What should the concentration ratio of NO2-/HNO2 be if the desired pH of this buffer is 4.00? (Ka of HNO2 = 4.27 x 10-4)
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-(??)
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?
what is the pH of a buffer solution containing 0.23 M HNO2 and 0.15 M NO2 Nitrous acid has a Ke of 4.5 x 10-4. Part A What is the pH of a buffer solution containing 0.23 M HNO2 and 0.15 M NO? Express your answer using two decimal places. 19 AEO ? pH = Submit Request Answer Provide Feedback Google Drive @ Quinet C Chego Coinmame R PL Access SIUE CHW11 Chapter 11 Homework Problem 25 25 of 25...
1.A 25.00 ml smaple of 0.523 M nitrous acid, HNO2, solution is titrated with a 0.213 M NaOH. For HNO2, Ka = 4.0 X 10^-4 a) What is the pH before any NaOH is added? b) Write the reaction that takes place as KOH solution is added to the HNO2 solution. c) write the reaction that determines the pH at the equivialnce point. -What is the pH at the equivilance point -what is the pH at the 1/2 equivilance point...
A solution of nitrous acid and potassium nitrite acts as a buffer due to reactions that occur within the solution when a strong acid or a strong base is added. Write the net ionic equation for the reaction that occurs in this buffer to react away any added HCl (aq). Write the net ionic equation for the reaction that occurs in this buffer to react away any added NaOH (aq). 3. A solution of nitrous acid and potassium nitrite acts...
What would be the pH of a buffer that contains 0.987 grams of Nitrous acid (HNO2) and 1.242 grams of sodium Nitrite (NaNO2), in 250ml of solution?(Ka of Nitrous acid = 4.5X10-4)
Which is the conjugate base of nitrous acid, HNO2? NO2- NO4+ HNO3 H2NO2
Calculate the base/acid ratio that should be used to prepare a buffer from nitrous acid (HNO2) with a pH of 4.00. The Ka Value of HNO2 is 4.5 * 10^-4