A 200. mL solution of 0.25 M ammonia is titrated with 1.0 M HCl. Calculate the pH after 60 mL of HCl have been added.
A 200. mL solution of 0.25 M ammonia is titrated with 1.0 M HCl. Calculate the...
50. ml of a 1.0 M solution of hydrochloric acid, HCl, is titrated with a 1.0 M solution of sodium hydroxide. What is the pH after 51 mL of NaOH has been added? Assume that the volumes are additive.
5.00 mL of 0.250 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia is 1.75 x 10-5 What is the pH of the ammonia solution prior to the addition of any HCl? What is the pH of the solution after 5.00 mL of HCl has been added?
A 91.0 mL sample of 0.0300 M HCl is titrated with 0.0600 M ROOH solution. Calculate the pH after the following volumes of base have been added. (a) 16.8 ml (b) 43.2 mL (C) 45.5 mL pH = pH = pH = (d) 46.0 mL () 82.8 ml pH = pH =
A 96.0 mL sample of 0.0300 M HCl is titrated with 0.0600 M KOH solution. Calculate the pH after the following volumes of base have been added. (a) 18.7 mL pH = (b) 45.6 mL pH = (c) 48.0 mL pH = (d) 48.5 mL pH = (e) 85.0 mL pH =
Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.
A 20.0-mL sample of 1.50 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 12.00 mL of acid have been added to ammonia? Kb for NH3 = 1.8 × 10–5
Calculate the pH for 100. mL of a 0.500 M solution of ammonia, (NH3 Kb=1.8x10-5) being titrated with 0.500 M HCl at the following positions in the titration. i) The initial pH (before any HCl has been added). A. 9.44 B. 10.81 C. 11.48 D. 12.00 E. 11.75
A 20.0-mL sample of 1.50 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 12.00 mL of acid have been added to ammonia? Kb for NH3 = 1.8 × 10–5 5.93 9.30 8.06 9.07 10.45
5.00 mL of 0.250 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia is 1.75 x 10-5. What is the pH of the solution after the addition of 25.00 mL of HCl?
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01× 10-14.) (a) What was the original pH of the ammonia solution? 匹の10.85 (b) What is the pH at the equivalence point? の5.50 (c) Draw a titration curve for this titration. ( r curve should be quantitative; calculate the pH at different points to construct...