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Westminster H.S. AP Chemistry Name ___________________________________ Period ___ Date ___/___/___ Acid-Base Equilibria BUFFER CALCULATIONS The weak acid, acetic acid, has the formula, HC2H3O2. Ka acetic acid = 1.8x10-5 (a) A buffer solution is prepared by adding 0.10 Liter of 2.0 molar acetic acid solution to 0.10 Liter of a 1.0 molar sodium hydroxide solution. Compute the hydrogen ion concentration of the buffer solution. PROBLEM BREAKDOWN: (i) Calculate moles of HC2H3O2. (ii) Calculate moles of OH-. (iii)What is the total volume (in Liters)? (iv) Fill in this NEUTRALIZATION chart using Molarities HC2H3O2 + OH- H2O(l) + C2H3O2- H3O+ + C2H3O2- (v) Fill in this EQUILIBRIUM chart: HC2H3O2 + H2O(l) (vi) Write the equilibrium expression for HC2H3O2. Substitute the equilibrium values into the expression and compute the hydrogen ion concentration. Ka acetic acid = 1.8x10-5 (b) Suppose that 0.010 Liter of 0.50 M hydrochloric acid is added to 0.20 Liter of the buffer prepared in (a). Compute the hydrogen ion concentration of the resulting solution. PROBLEM BREAKDOWN: (i) Calculate moles of HC2H3O2 and C2H3O2-. (ii) Calculate moles of H+. (iii)What is the total volume (in Liters)? (iv) Fill in this chart using Molarities C2H3O2- + H+ HC2H3O2 (v) Fill in this chart: HC2H3O2 + H2O(l) H3O+ + C2H3O2- (vi) Write the equilibrium expression for HC2H3O2. Substitute the equilibrium values into the expression and compute the hydrogen ion concentration.