calculate the value of the equilibrium constant at 25 Celcius, for the reaction: HNO2 + OH-...
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calculate the value of the equilibrium constant at 25 Celcius, for
the reaction: HNO2 + OH-...
1. A certain amount if nitrous acid is dissolved in water at 25 celcius. At equilibrium,...
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-
Reaction of nitrous acid in water: HNO2(??) + H2O(?) ⇌ H3O+(??) + NO-(??). The ?a at...
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-(??)
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2...
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2 k1? NH4+ + H2O -> H3O+ + NH3. ka = 5.6 x 10^-10 NO2- + H2O -> HNO2 + OH- kb =2.2 x 10^-11 2H2O -> H3O+ + OH- kw = 1.0 x10^-14 Write symbolic expression for equilibrium constants for each reaction. Derive expression for k1 in terms of ka, kb, and kw; find numerical value of k1.
Nitrous acid, HNO2, has a Ka of 7.1 × 10−4. What are [H3O+], [NO2−], and [OH−]...
Nitrous acid, HNO2, has a Ka of 7.1 × 10−4. What are [H3O+], [NO2−], and [OH−] in 0.54 M HNO2?
For the following equation: The Ka value of HNO2 is 4.0 x 10-4. If the equilibrium...
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
Calculate the equilibrium constant K for the following reaction at 25 degrees celcius from standard electrode...
Calculate the equilibrium constant K for the following reaction at 25 degrees celcius from standard electrode potentials for the following reaction: Sn^4+(aq) + 2Hg(l) = Sn^2+(aq) + Hg2^2+(aq)
4.(4 points) What is the value of equilibrium constant for the system shown below at 25°C...
4.(4 points) What is the value of equilibrium constant for the system shown below at 25°C in terms of Ka HNO2 and Kb C5H5N? No2 (ag) + C6H5NH*(ag) = C6H5N(ag) + HNO2(ag) (а) Ка+ Kb (b) Ka - Kb (c) Ka/ Kb (d) Kw / (Ka Kb) (e) -Ka Kb) ОООО
The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to...
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∘...
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka...
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)
The equilibrium constant for the equation HNO3(aq) + H2O(l) = H, 0+ (aq) + NO2 (aq) is Kg = 5.6 x 10-4 M at 25.0 °C. Ca...
The equilibrium constant for the equation HNO3(aq) + H2O(l) = H, 0+ (aq) + NO2 (aq) is Kg = 5.6 x 10-4 M at 25.0 °C. Calculate the value of AGixn at 25.0 °C for nitrous acid when [NO2] = [H3O+] = [HNO2] = 1.00 M. AGixn = kJ/mol Will the acid spontaneously dissociate under these conditions? O no O yes Calculate the value of AGrxn for nitrous acid when [NO, ] = [H,O+] = 7.13 x 10- M and...
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
4.(4 points) What is the value of equilibrium constant for the system shown below at 25°C in terms of Ka HNO2 and Kb C5H5N? No2 (ag) + C6H5NH*(ag) = C6H5N(ag) + HNO2(ag) (а) Ка+ Kb (b) Ka - Kb (c) Ka/ Kb (d) Kw / (Ka Kb) (e) -Ka Kb) ОООО
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)
The equilibrium constant for the equation HNO3(aq) + H2O(l) = H, 0+ (aq) + NO2 (aq) is Kg = 5.6 x 10-4 M at 25.0 °C. Calculate the value of AGixn at 25.0 °C for nitrous acid when [NO2] = [H3O+] = [HNO2] = 1.00 M. AGixn = kJ/mol Will the acid spontaneously dissociate under these conditions? O no O yes Calculate the value of AGrxn for nitrous acid when [NO, ] = [H,O+] = 7.13 x 10- M and...
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