Question

Instructions: Complete all the problems in this assignment Show all your work and submit a PDF with your answers through Husky CT for your lab section. Please e-mail me if you have an issues with the submission. Activity #1 Calculate the pH for the following acidic solutions 1. Calculate the pH and pOH for the following solutions: a. 0.200 M HNO3 b. 0.200 M H2SO4 2. Calculate the equilibrium concentration for [H], [A-], and [HA], the pH and pOH for a 0.200 M propionic acid solution. Ka = 1.3 x 10-5 3. Calculate the equilibrium concentrations for [H], [A], and [HA], the pH and pOH for a 0.200 M carbonic acid solution. Ka = 4.2 x 10-7 4. Calculate the equilibrium concentrations for [H], [A-], and [HA], the pH and pOH for a 0.200 M lactic acid solution. Ka = 8.3 x 10-4 Use your calculation results to complete the following table pH POH Acid HNO3 H2SO4 Propionic Acid (CH3CH2CO2H) Carbonic Acid (H2CO3) Lactic Acid (C3H603) What is relationship between the K, and the pH of the solution? Rank the following acids in terms of their strength from weak to stronger.

Answer 1

1) a) HNO HNOO [H] +0.200M 1 pH = -log (HP) = -log(0.200) 0.699 : b) H₂SO4 → 24th of son2 Che] = 2x0,200 A 0.4oom pH = -log(0.400) > 0.398 2) HA+ HO HO HO 1. tx tx change |(443)=[AⓇ] = 1.6x1024 (0.2-x) x x equilibrium [ua] =0.2-0.0016 ka = [Hot] [40] [HA? 0.2 o initial -0.1984 M 13x105x ( 0.20%) →X = 0.0016 M pH = -log(0.0016) — 2.19, poh= in - 11.2) HA + H2O = H the 0.2 []=[AⓇ] = 0.00029 M X initial change equilibricem (012->) x x [HA] = 0.2-0.00029 50.19971 m 4.2x107- 10.20%) = 0.000 29 M pH = -log(0.00029) 73.54 , POH = 14-3.54 F 10.46 HO +A® A) HA+ HO 0.2 initial o CAL J =[AⓇ] = 0.0125 M o 4x x tx x change equilibrium (0.2-2) CHA] = 0.2-0.0125 = 0.1875 M 81371543 - X 50,0 125 M (012-x) PH = -log(0.0125) ► 119, pOH = 14-109 - 12.1