I need help with just the last part where it asks to find the pH.
A solution containing 0.1 7 M Pb". 1.5 x 10-6 М РЬ". 1.5 x 10-6 M Mn". 0.17 M MnO-, and 0.88 M HN...
A solution containing 0.190.19 M Pb2+Pb2+ , 1.5×10−61.5×10−6 M Pb4+Pb4+ , 1.5×10−61.5×10−6 M Mn2+Mn2+ , 0.190.19 M MnO−4MnO4− , and 0.900.90 M HNO3HNO3 was prepared. For this solution, the balanced reduction half‑reactions and overall net reaction shown can occur. 5[Pb4++2e−↽−−⇀Pb2+]5[Pb4++2e−↽−−⇀Pb2+] ?∘+=1.690 VE+°=1.690 V 2[MnO−4+8H++5e−↽−−⇀Mn2++4H2O]2[MnO4−+8H++5e−↽−−⇀Mn2++4H2O] ?∘−=1.507 VE−°=1.507 V 5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO−4+16H+5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO4−+16H+ A. Determine ?∘cellEcell∘, Δ?∘ΔG∘, and ?K for this reaction. ?∘cell=Ecell∘= V Δ?∘=ΔG∘= J ?=K= B. Calculate the value for the cell potential, ?cellEcell, and the free energy, Δ?ΔG, for the given conditions....
A solution containing the following was prepared: 0.15 M Pb2. 1.5% 10.6 M Pb4t, 1.5x 106 M Mn2. 0.15 M MnO4, and 0.88 M HNO3. For this solution, the following balanced reduction half-reactions and overall net reaction can occur E-1.690 V E1.507 v A) Determine Eocell. AG®, and K for this reaction Number Number Number cell B) Calculate the value for the cell potential, Ecel, and the free energy, AG, for the given conditions Number Number cell Scroll down for...
6.(12pts) Should a precipitation of Pb(IOs)2(s) form when 55.0 ml of 0.0450 M Pb(NO:)2 (aq) solution is added to 48.0 ml of 0.215 M NalOs(ag) solution? Assume that at the temperature at which the experiment is performed, Ks of Pb(IOs)2(s) is 2.8 x 10-13 All work must be shown- a guess is not sufficient Calculate the solubility of Cr(OH)s in grams per liter in a system buffered at pH 10.6. Data:Kn of Cr(OH)3(s) = 6.3 x 10-31 . The molar...
Suppose a chemist starts with an aqueous buffer that contains 0.05 mol of HCN and 0.07 mol of NaCN in a total volume of 1.00 L. What is the pH after 0.03 mol of OH is added to the buffer? a. 2.01 b. 9.46 c. 10.92 d. 10.01 e. 8.61 Calculate Eºcell for the following balanced redox reaction in acidic solution: 35024+ 2Cr(s) + 12 H+ + 3 SO2 (g) + 2Cr+3 + 6 H2O (acidic) a. +1.945 V b....
6. Given a total dissolved lead concentration of 2.0x10-5 M, a total dissolved NTA concentration of 2.0x10-2 M, and a pH of 12.3 (note extreme pH) a. Under these conditions, what is the dominant form of NTA? b. Write an equation for total dissolved NTA and for total dissolved Pb. What assumptions can you make? c. Calculate the predicted [Pb2+], considering NTA complexation only? d. What is the [Pb2+] as predicted by the solubility of Pb(OH)2(s) at pH 12.3? e....