5. A 50.00 mL 0.1000 M HNO2 (Ka = 7.2 x 10+) is being titrated with 0.1000 M NaOH. a. Calculate the pH of the solution before any amount of titrant is added. (Hint: Construct an ICE table) b. Calculate the volume of NaQH required to reach the equivalence point. c. Calculate the pH after the addition of 25.00 mL of NaQH. d. Calculate the pH at equivalence point. (Hint: Determine first the concentration of the conjugate base that was produced. You will construct an ICE table for the conjugate base.) e. Calculate the pH after adding 75.00 mL of NaOH. f. Using your answers from a to f, roughly generate a titration curve.

You have 100 mL of an acetic acid/acetate buffer. The solution is comprised of 0.33 M acetic acid and 0.01 M acetate. What is the new pH when 5.0 mL of 0.10 M HCl is added to this solution? The pKa of this pair is 4.76. (Note: You must use the I.C.E method for this one).

A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide.  a. What is the pH of the solution before adding any nitric acid? b. What is the pH at the half-equivalence point? c. What is the pH after the addition of 65.00 mL of nitric acid?

a 20.70mL sample of 0.64 M HCL is titeares with 0.64M NaOH. Calculate the pH after the addition of 19.38 mL NaOH

A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO.a. What is the initial pH of this solution?b. What is the pH after addition of 150.0 mg of HBr?c. What is the pH after addition of 85.0 mg of NaOH?

Consider the titration of 25.0mL of 0.375MHBr with 0.250MKOH .a.Calculate the volume (in mL) to reach the equivalence point. b.Calculate the initial pH (before the addition of KOH). c.Calculate the pH after the addition of 30.0mL of KOH.

A) A buffer solution contains 0.413 M KHSO3 and 0.242 M Na2SO3. Determine the pH change when 0.121 mol KOH is added to 1.00 L of the buffer.pH after addition − pH before addition = pH change B )A 24.0 mL sample of 0.256 M methylamine, CH3NH2, is titrated with 0.335 M hydrobromic acid.After adding 7.50 mL of hydrobromic acid, the pH is . C) A 29.4 mL sample of 0.202 M ethylamine, C2H5NH2, is titrated with 0.295 M nitric acid.At the equivalence point, the pH is . D) A 23.2 mL sample of 0.365 M triethylamine, (C2H5)3N, is titrated with 0.214 M hydroiodic acid.After adding 57.4 mL of hydroiodic acid, the pH is

Consider the titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCI. Calculate the pH after 65.0 mL of HCI added. (K for CH3NH2=4.4 × 10-4) A. 10.96 B. 9.75 C. 7.00 D. 3.68 E. 2.54

Consider the titration curve describing the titration of a strong acid by addition of a strong base. Which of the following statements is incorrect? a. The equivalence point is at pH = 7.0. b. The pH is lower at the end of the titration than at the beginning. c. The pH increases rapidly around the equivalence point. d. At the equivalence point, the only species present are water and a neutral salt. e. The pH does not increase very rapidly at the beginning of the titration.

= 0.01 x 0.100 = 0.001 001 50.0 X0-250 = 0.0125 0.0123 025 0.06 0.300 x0.01 0.100. X 0.01 B. 9.25 0.06 6A 10.0 mL solution of 0.300 M NH3 is titrated with 0.100 M HCI. Calculate the pH after the addition of 10.0 mL of acid. A. 9.55 0.001 -0.003 0.300 x 0.0 0.001 C. 8.95 0.02 PH = PKG +10g [0.0156 2.67=4.744+ [19165 TI-84 Plus TEXAS INSTRUMENTS D. 9.73 = Pl= 3.68 - 267 28.3. 0:3 0002 0.002 M Plt = -log = .05 U.2 E. 8.77 Pit=Pkg tog 20.015 = 1.01 [A] [HA]