10-6. Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. What is the equivalence volume? Find the pH at the following volumes of HBr and make a graph of pH versus Va: Va = 0, 1.00, 5.00, 9.00, 9.90, 10.00, 10.10, and 12.00 mL.

Consider the titration of 35ml of 0.150mol/L benzoic acid (Ka=6.3*10^-5) with 0.110 mol/L NaOH. Calculate the initial pH of the benzoic acid Calculate the pH after the addition of 30.0 mL of NaOH Calculate the pH of the equivalence point Calculate the pH after the addition of 60mL of NaOH Provide a rough sketch of the titration curve.

A titration of 200.0 mL of 2.55 MH 2A was done with 1.00 M NaOH. For the diprotic acid H 2A, Ka1 =2.5 x 10-5, Ka2=3.1 x 109. Calculate the pH before any 1.00 M NaOH has been added. Oa. 11.83 Ob.8.68 O c. 9.66 Od.2.17 Oe. 4.20

Data for the titration of 100.00 mL of a weak acid by NaOH are given in the table. Find the end point by preparing a Gran plot, using the last 10% of the volume prior to Ve. mL NaOH 0.00 1.31 2.34 3.91 5.93 7.90 11.35 13.46 15.50 16.92 18.00 18.35 18.95 19.43 19.93 20.48 V₂ = pH 4.14 4.30 4.44 4.61 4.79 4.95 5.19 5.35 5.50 5.63 5.71 5.77 5.82 5.89 5.95 6.04 mL NaOH 20.75 21.01 21.10 21.13 21.20 21.30 21.41 21.51 21.61 21.77 21.93 22.10 22.27 22.37 22.48 22.57 pH 6.09 6.14 6.15 6.16 6.17 6.19 6.22 6.25 6.27 6.32 6.37 6.42 6.48 6.53 6.58 6.63 mL NaOH 22.70 22.76 22.80 22.85 22.91 22.97 23.01 23.11 23.17 23.21 23.30 23.32 23.40 23.46 23.55 pH 6.70 6.74 6.78 6.82 6.86 6.92 6.98 7.11 7.20 7.30 7.49 7.74 8.30 9.21 9.86 mL

Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid (HPr), and we slowly add 0.1000 M NaOH. What is the pH at 40.00 mL and 50.00 mL?

Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300 M NaOH. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Use a BCA table to detrmine the moles of reactant and product after the reaction of the acid and base. Ignore the amount of liquid water. Then, set up an ICE table to identify the unknown. Then figure the pH.

Be sure to answer all parts. Find the pH and the volume (mL) of 0.487 M HNO3 needed to reach the equivalence point in the titration of 2.65 L of 0.0750 M pyridine (C5H5N, Kb = 1.7 × 10−9). Volume =  mL HNO3 pH =

Set up a BCA table and then ICE table to determine the pH at the equivalence point.