Cell Zn | Zn²+ (1.0 M) || Cu²+ (1.0 M) Cu Zn | Zn²+ (1.0 M) || Cu²+ (0.10 M) Cu Eºcell = Ecell= Calculation

Topics: Cells and equilibrium; Competing equilibrium in cells Use general chemistry rules for significant figures. 2. Ecell for the cell below is 0.150 V. [H+] in the anode is unknown but kept constant by a buffer consisting of 0.10 F HA and 0.10 F A– . (These components are not shown in the cell notation but are present in the anode nonetheless.) Pt(s) | H+ (? M) | H2(g) (1.00 atm) || H+ (1.00 M) | H2(g) (1.00 atm) | Pt(s) Find the pH of the buffer and Ka for the monoprotic weak acid HA.

6. Fill in the following table. Hint: the cell diagram as written contains spectator ions! Once you've picked them out, do NOT include them in the net ion equation. Ag(s), Ag:CrO4(s) | Na₂CrO4(aq) (2.00 M) | Mn(NO³)2(aq) (0.100 M), HNO:(aq) (2.00 M) | MnO₂(s) ** Ag:CrO4(s) + 2c¯ → Ag(s) + CrO² (aq) &°red=+0.45 V Net ionic equation: cell: Q: Ecell: Oxidizing agent:

If the concentration of Sn2+ ions in a solution of Sn(OH)2 was measured to be (1.60x10^-3), what is the Ksp value for Sn(OH)2? Note: Your answer is assumed to be reduced to the highest power possible.

Write the net ionic equations that occur in the following cells: Pb| Pb(NO3)2 ||AGNO3 | Ag Zn | ZnCl, || Pb(NO;)2 | Pb Pb| Pb(NO3)2 || NiCl, | Ni

The equilibrium constant K for the overall reaction that takes place in the cell Pt|Sn2+, Sn4+||Ag+|Ag at 298 K is?

A soluion of 10.0 mL of 0.0500 mol/L AgNO3 is titrated with 0.0250 mol/L NaBr in the cell: VKE||onbekende oplossing||Ag(s) Calculate the potential of the cell after adding 0.1 mL, 10.0 mL, 20.0 mL and 30.0 ml of titrant. E\deg (Ag+, Ag = 0.799 V; E(VKE = 0.244 V; Ksp(ABr) = 5.0*10-13