N.B.: As per Chegg guidelines we have to answer first question out of multiple questions. Though we tried to answer the 2nd too, but there is some type mistakes. Without proper question and adequate data we can't answer. But we expect you can solve the rest part. Others reupload it woth proper expression. All the best.
1. A certain amount if nitrous acid is dissolved in water at 25 celcius. At equilibrium,...
A certain amount of nitrous acid is dissolved in water at 25℃. At equilibrium, the pH of the solution is 2.33. What is the concentration of H30+ (aq) and NO2-(aq)?
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-(??)
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
You know that the ionization constant for nitrous acid is 7.1x10^-4 (0.00071) at 25 degrees Celcius. You want to prepare a solution that has a pH=1.53. What should the concentration of the HNO2 be?
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
1. A 1.00 liter solution contains 0.46 M nitrous acid and 0.35 M sodium nitrite. If 30.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water.) _______TrueFalseA. The concentration of HNO2 will remain the same. _______TrueFalseB. The concentration of NO2- will decrease. _______TrueFalseC. The equilibrium concentration of H3O+ will remain the same. _______TrueFalseD. The pH will increase. _______TrueFalseE. The ratio of...
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?
A solution of nitrous acid, HNO2 is 6.3x10^-3 M, which is a weak acid with Ka=7.2x10^-4. Calculate: [HNO2] [NO2] pH What is the concentration of a nitrous acid solution with a pH of 2.21
1- Calculating [H+] for Pure Water: In a certain acidic solution at 25 ∘C, [H+] is 100 times greater than [OH −]. What is the value for [OH −] for the solution? In a certain acidic solution at 25 , [] is 100 times greater than [ ]. What is the value for [ ] for the solution? 1.0×10−8 M 1.0×10−7 M 1.0×10−6 M 1.0×10−2 M 1.0×10−9 M 2. ± Acid-Base Relationships in Water: Water ionizes by the equation H2O(l)⇌H+(aq)+OH−(aq)The...
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...