A 44.20 mL sample of phenol (Ka=1.60x10-10) analyte with a concentration of 0.113 mol L-1 is titrated with a 0.113 mol L-1 solution of NaOH titrant. Determine the pH of the solution when the titration reaches the equivalence point.

A buffer at pH 5.1 is prepared from a total concentration of 0.278 M sodium acetate and acetic acid. What are the concentrations of acetic acid and acetate in this solution? The Ka for acetic acid is 1.76 x 10-5 and the pKa is 4.75.

In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb=4.4 x 10-4), with 0.50 M HCl, calculate the pH under the following conditions: after 50.0 mL of 0.50 M HCl has been added at the equivalence point

65 mL of 0.65 M benzoic acid (Ka = 6.4×10-5) is titrated by 0.05 M NaOH. 1)Calculate the pH of the acid solution before any titrant is added. 2)Calculate the pH after 795.9 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 3)Calculate the pH after 845 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 4)Calculate the pH after 1.58 x 10^3 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid.

The following is a titration curve for a monoprotic weak acid. 0.200 grams of the acid was dissolved in 50.00 mls of water and titrated with a 0.150 M solution of NaOH. 14.00 13.00 12.00 11.00 10.00 9.00 8.00 pH 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 Vol. Base (mL) What is the pKa of the acid? How many moles of acid were present? What is the molecular weight of the acid? What pH range should the indicator change color to determine the endpoint of titration? Over what pH range is [HA]> [A]? 00 08 25.00 00'0 00 0 00 9 00 0

Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.05 M NaOH? alizarin, pH range: 5.7-7.2       bromocresol green, pH range: 3.8-5.4       phenol red, pH range: 6.4-8.0       methyl yellow, pH range: 2.7-4.0       naphtholphthalein, pH range: 7.3-8.7

In a lab, you titrate 27.0 mL of 0.100 M acetic acid (CH3COOH, a weak acid, pKa 5.756, Ka 2.75 x 10-5), with 0.100 M NaOH. At the equivalence point, the concentration of the primary species in solution is approximately What is the pH of the solution at the equivalence point? At the equivalence point, what percentage of the analyte has been titrated?

How many mL of 1.0 M NaOH must be added to 100. mL of 0.050 M HC2H3O2 to make a buffer with a pH = 5.00? Ka = 1.8 x 10-5 for acetic acid.

30 mL of 0.1 M HCI is titrated with 0.1 M CH3NH₂ (Ka = 2.0 x 10-¹1) solution. Calculate the pH after adding 15 mL of CH3NH₂ to initial acid 12.01 5.81 1.48 3.49 9.57

Which acid, along with it's corresponding salt, would be best to make a buffer of pH 7? hydrofluoric acid, Kg = 6.8 x 104 O hypochlorous acid, K, = 3.5 x 10o-8 O hydrocyanic acid, K, = 4.9 x 10-10 O acetic acid, K, = 1.8 x 105