Why does buffer capacity increase as a solution becomes very acidic (pH 1) or very basic (pH 13)?
Equilibrium Calculations • ex. CO(g) + H2O(g)⁶CO2(g) + H2(g) Kc=0.64 You start with 1.0 mol CO and 1.0 mol CO2 in a 1 L ﬂask. You then add 2.0 mol H2O. What is the concentration of H2 at equilibrium Check for equilibrium ﬁrst: Q does not equal 0—>system not in equilibrium Make ICE table: CO(g) + H2O(g) ⁶ CO2(g) + H2(g) Initial 1.0 M 2.0 M 1.0 M 0 M Change -x -x +x +x Equilibrium (1.0-x) (2.0-x) (1.0+x) x Kc = 0.64 = [1.0+x][x] [1.0-x][2.0-x] 0.64 = x + x^2 2 - 3x + x^2 0.64(2 - 3x + x^2) = x + x^2 -0.36x^2 - 2.92x + 1.28 = 0 *sta