PART A is already solved. It is provided for context for you :)
PART A: If you have a initial conc. 0.10M NH4NO2, make an ICE table, solve for concentration of NH4+, NO2-, NH3 and HNO2.K1 value is 1.23e-6
NH4+NO2<=>NH3+HNO2
[NH4] and [NO2] both are 9.99e-2 M
[NH3] and [HNO2] were found to be 1.11e^-4 M
PART B (the part I need help with): Using the values you found in part A (conc. of NH4 and NH3), find the value of the concentration of H3O+.
NH4+(aq)+H2O(l)<=>H3O+(aq)+NH3(aq)
Ka value is 5.6e^-10
Thank you in advance!
PART A is already solved. It is provided for context for you :) PART A: If...
If we have a initial concentration of H4NO2 (aq) at .10 M, make an ICE table for the following reaction, and solve for the concentration of NH4, NO2, NH3 and HNO2 NH4+(aq)+NO2-(aq)<=>NH3(aq)+HNO2(aq) (not sure if this helps, but the value of K1 is 1.23e-6)
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.
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