4) For the Zn|Zn²*(1M)||Cu²*(1M)|Cu battery discussed in class (6°=1.1V), answer the following (assume activity of ions are equal to their concentration): a) What is the cell potential & for ion concentrations [Zn²+]=0.0001M and [Cu²+]=0.5M? b) What is the equilibrium coefficient K, for the cell? c) What external Voltage must be applied to the cell so that a cell with concentrations [Zn2+]=0.1M , [Cu²+]=0.0005M is at equilibrium?

The voltaic cell Cd(s)|Ca?t (ag) || Ni²+ (1.0 M)|Ni(s) has a cell potential of 0.310 V at 25°C. What is the concentration of cadmium ion? (Eell = 0.170 V.) %3D Concentration M

Consider the following cell. Cr | Cr³+ (1.00 M) || Ni²+(1.00 M) | Ni & = 0.68 V (a) How many milligrams of metallic nickel would be plated on the cathode if a current of 0.16 A is drawn for 1.3 hrs? 4.0 2.3e2 mg (b) What is the Cr³+ concentration when the Ni²+ concentration has dropped to 1.0 × 10-4 M? 4.0 33 X M What is the cell potential at this point? 4.0 0.666 X V

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.