- Task Detine The Term Buffer Solution Marks 5 Calculate The Ph Of A Buffer Solution Prepared Using 500 Ml 0 100 Mol L 1 (174.66 KiB) Viewed 39 times
Task + Detine the term buffer solution! Marks 5 Calculate the pH of a buffer solution prepared using 500 ml 0.100 mol/l ethanoic acid CH3COOH and 200 ml 0.100 mol/l sodium hydroxide NaOH. pK, for acid is 4.74. 3 Task 5 The following reaction H + HCO3 H2CO3 -> H20+CO, is important in maintaining the pH of blood at a nearly constant value of about 7.4 What happens to the position of equilibrium (H+ + HCO; - H2CO3) and the pH when blood absorbs acid or base? A person suffering from anxiety begins breathing rapidly and as a result suffers alkalosis, an increase in blood pH. One cure for this problem is breathing in a paper bag. Why does this procedure lower blood pH? 8 Task 6 A 25.0 ml solution of a weak monobasic base BOH(aq) is titrated with 0.10 mol/l hydrochloric acid HClag), and the following graph is obtained. tuffer region 12 11 10 petat E SONO halt heutralization 6 point = pk6= 9.2 equivalence point 4 3 2. 1 0 0 5 Сл 10 15 20 25 30 35 40 V, ml (3) a) Determine and show on the graph the equivalence point, half- neutralization point (mid-point) and buffer region. (2) b) Determine the pH at the equivalence point and explain why the point is not at the 7. (2) c) Determine volume of HCI used for neutralization of weak base at equivalence point and calculate the concentration of weak base. (1) d) Determine the pKp of weak base and show on the graph.