(c)At 10C,suppose [VO2]=2.0 M,[VO]=0.010 M,[H']=0.50 M and [Zn2]=0.10 M Calculate the cell potential under these conditions(V). Q=0✉Zn-0o10010=40x10 [V02aHa广(2.0'(0.50) E=E-RTIn(Q) nF -1.76J-83141K-mor273+10K1n40x10 c2(96487Cmol） =1.76J 1s82 =1.88V 2.Calculate the pH and the concentrations(mol L)ofall species present(except water)in a 1.0 M solution of carbonic acid,H2CO)For this acid,Ka=4.3x 107 and K2=5.6x 10 H2CO3a)+H2O)I HCO3)+H3O(aQ) [HCO,H,O'] H,C0】 H2CO3)HCO3()H30(a) Initial 10 0 0 Change +x +x Equilibrium 1.0-x Thus at equilibrium,(c) At 10o C, suppose [VO2 + (aq)] = 2.0 M, [VO+2 (aq)] = 0.010 M, [H+ (aq)] = 0.50 M and [Zn+2] = 0.10 M. Calculate the cell potential under these conditions (V). 22 2 2 (aq) (aq) 5 2 4 24 2 (aq) (aq) 0 1 1 5 1 [VO ] [Zn ] (0.010) (0.10) Q 4.0 10 [VO ] [H ] (2.0) (0.50) RT E E ln(Q) nF J 8.314J K mol (273 10)K 1.76 ln(4.0 10 ) C 2(96487 C mol ) J J 1.76 ( 0.12 ) C C J 1.88 C 1.88 V + + − + + − − − − = == = − + = − × = −− = = × 2. Calculate the pH and the concentrations (mol L-1) of all species present (except water) in a 1.0 M solution of carbonic acid, H2CO3(aq). For this acid, Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. H2CO3(aq) + H2O(l) ∏ HCO3 - (aq) + H3O+ (aq) 1 3 (aq) 3 (aq) a 2 3(aq) [HCO ][H O ] K [H CO ] − + = H2CO3(aq) HCO3 - (aq) H3O+ (aq) Initial 1.0 0 0 Change -x +x +x Equilibrium 1.0-x x x Thus at equilibrium, 4