If the pH is 7.1 and the pE is 5.6, what will be the ratio of [NH4 + ] to [NO2 - ]? If the pH if 8.0, at what pE value w...
If the pH is 7.1 and the pE is 5.6, what will be the ratio of [NH4 + ] to [NO2 - ]? If the pH if 8.0, at what pE value will the ratio of [NH4 + ] to [NO2 - ] be 1000:1?
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If the pH is 7.1 and the pE is 5.6, what will be the ratio of [NH4 + ] to [NO2 - ]? If the pH if 8.0, at what pE value w...
. If the pH is 7.1 and the pE is 5.6, what will be the ratio of [NH4 + ] to [NO2 - ]? d. If the pH if 8.0, at what pE va...
. If the pH is 7.1 and the pE is 5.6, what will be the ratio of [NH4 + ] to [NO2 - ]? d. If the pH if 8.0, at what pE value will the ratio of [NH4 + ] to [NO2 - ] be 1000:1?
For the portion of the pE-pH diagram where the reduction of NO2 - to NH4 + is the relevant reaction, use the expression...
For the portion of the pE-pH diagram where the reduction of NO2 - to NH4 + is the relevant reaction, use the expression (NO2- + 8H+ + 6e- → NH4+ + 2H20 and pE=15.14-log([NH44]⅙ /[NO2- ]⅙ [H+]4/3])) to find the equation for the line that will separate the two species. Remember that the line will be where the species are equal in concentration. (Hint: your equation should be in the form y = mx + b where y = pE...
What is the buffer component ratio, (NO2-)/(HNO2) of a nitrite buffer that has a pH of...
What is the buffer component ratio, (NO2-)/(HNO2) of a nitrite buffer that has a pH of 2.96. Ka of HNO2 is 7.1 x 10-4.
For a PE-pH diagram, derive the function for the boundary at which [NH*] = [NO2] for...
For a PE-pH diagram, derive the function for the boundary at which [NH*] = [NO2] for pH <7. The relevant half-reaction to consider is NO2 + NHA (not balanced) En° = 0.893 V
For the following reaction: NO2 - (aq) → NH4 + (aq) Balance the reaction as a one-electron process in acid solution and...
For the following reaction: NO2 - (aq) → NH4 + (aq) Balance the reaction as a one-electron process in acid solution and Given a E° value of 0.895 V, write the expression for pE in terms of pE° and the relevant ion concentrations.
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.
For the following reaction: NO2-+6H+NH4+H2O Balance the reaction as a one-electron process in acid solution and Given a...
For the following reaction: NO2-+6H+NH4+H2O Balance the reaction as a one-electron process in acid solution and Given a E° value of 0.895 V, write the expression for pE in terms of pE° and the relevant ion concentrations.
What is the ratio of [NH4Cl]/[NH3] in order to make a NH3/NH4Cl buffer solution with pH=8.70....
What is the ratio of [NH4Cl]/[NH3] in order to make a NH3/NH4Cl buffer solution with pH=8.70. (Kb for NH3 is 1.8 x 10^–5)
(a) What is the pKbof NO2−? ( Ka of nitrous acid is 7.1 × 10−4 )...
(a) What is the pKbof NO2−? ( Ka of nitrous acid is 7.1 × 10−4 ) pKb= (b) What is the pKaof the hydrazinium ion, H2N-NH3+? ( Kb of hydrazine = 8.5 × 10−7 ) pKa=
You need to make a buffer solution with pH of 8.0. You have the following reagents...
You need to make a buffer solution with pH of 8.0. You have the following reagents on your shelf: HC3H5O3 Ka=1.4*10-4 NaF HF Ka=6.6*10-4 Tris-base HC2H3O2 Ka=1.8*10-5 NH3 HClO Ka=2.9*10-8 NaC2H3O2 Tris-HCl Ka=8.3*10-9 NaClO NH4Cl Ka=5.6*10-10 NaC3H5O3 a) Which reagents would you use to make the buffer solution. Briefly explain why you would choose these. b) In what ration of molar concentrations would you combine them?
For a PE-pH diagram, derive the function for the boundary at which [NH*] = [NO2] for pH <7. The relevant half-reaction to consider is NO2 + NHA (not balanced) En° = 0.893 V
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