To calculate the new equilibrium concentration of the complex ion formed between Cu and NH aq , we first need to write the balanced chemical equation for the reaction:Cu aq + 4NH aq Cu NH aq Next, we will set up an ICE Initial, Change, Equilibrium table to determine the changes in the concentrations of the reactants and products as the reaction proceeds:| | Cu aq | NH aq | Cu NH aq ||---------------|----------|---------|---------------|| Initial M | 0.10 | 0.05 | 0 || Change M | -x | -4x | +x || Equilibrium M | 0.10-x | 0.05-4x | x |Now, we can write the expression for the equilibrium constant, Kc:Kc = [Cu NH ] / [Cu][NH]^4 Given that Kc = 1.6 10 at 25C, we can substitute the equilibrium concentrations from the ICE table into the Kc expression:1.6 10 = x / 0.10-x 0.05-4x ^4 Unfortunately, we don't have enough information to determine the effect of the temperature change on the equilibrium constant. However, we can solve for x assuming the Kc value remains constant:1.6 10 = x / 0.10-x 0.05-4x ^4 This equation is a bit complex to solve algebraically, so we can use numerical methods or make an assumption that x is small compared to 0.10 and 0.05, which simplifies the equation:1.6 10 x / 0.10 0.05 ^4 Now, we can solve for x:x 1.6 10 0.10 0.05 ^4x 1.25 10 MSo, the new equilibrium concentration of Cu NH at 35C, assuming the Kc value remains constant, is approximately 1.25 10 M. Keep in mind that this value is an approximation, and the actual equilibrium concentration may be different if the Kc value changes significantly with temperature.