Consider the titration of 50.0 mL of 0.170 M HA (K₁ = 4.2 x 105, pKa = 4.38) with 0.150 M NaOH. Determine the pH at the equivalence point 4.38 ○ 7.00 ○ 8.64 ○ 9.56 8.73

For a titration of 50.0 mL of 0.100 M acetic acid with 0.100 M NaOH, calculate pH: 1. at 0.00 mL NaOH addition (pH=2.87) 2. at 10.00 mL NaOH addition (pH=4.14) 3. at 25.00 mL NaOH addition (pH=4.74) 4. at 50.00 mL NaOH addition (pH=8.72) 5. at 51.00 mL NaOH addition (pH=11.00)

Calculate the pH at each point in the titration of 20.0 mL of 0.125 M weak acid, HA, with a Ka value = 5.20x10-4with 0.100 M NaOH after the following increments of base: 0 mL, 20.0 mL, 25.0 mL and 30.0 mL.

Which of the following indicators is best suited to determine the equivalence point of a titration of 0.25 M ammonium chloride (NH4CI) with a 0.25 M solution of a strong base? The titration curve is shown below. Data: pka (NH4CI) = 9.26 14 12 10 6 4 10 20 30 40 Volume of strong base (mL) Indicator pK HIn Phenolphthalein 9.3 Alizarin Yellow R11.2 Bromothymol blue 7.1 Bromocresol green 4.7 Hd