Hypochlorous acid has a pKa of 7530. If a 66.0 mL solution of o.180 M is titrated with o.150 M NaOH. Calculate the pH of the solution at each of the following points on the titration curve. Consult Textbook Numerical Answer a) Before the addition of any NaOH pH- b) After adding 11.40 mL of NaOH pH- c) At the equivalence point pH- d) After adding 82.2 mL of NaOH pH-
A 50.00 mL sample of a 0.150 M aqueous solution of a weak acid HA is titrated with a 0.300 M aqueous solution of NaOH. At which point in the titration will the pH of the solution equal pKa of the acid? a) After addition of 50.00 mL of the NaOH solution b) After addition of 25.00 mL of the NaOH solution c) After addition of 12.50 mL of the NaOH solution d) After addition of 6.25 mL of the...
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
5 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 2.1 . This solution is titrated with a 0.210 M NaOH solution. 60.2 mL of this NaOH solution is needed to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the value of pKa for HA (aq)? (c) What is the pH at the equivalence point? (d) What...
2.77 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 1.33. This solution is titrated with a 0.250 M NaOH solution. 40.6 mL of this NaOH solution is needed to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the value of pKa for HA (aq)? (c) What is the pH at the equivalence point? (d) What is...
A 20 mL sample of 0.01 M propionic acid (CH3CH2COOH; Pka = 4.87) is titrated with 0.05 M NaOH. A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the location of the equivalence point on...
Suppose 500 mL of 0.200 M nitrous acid , which has a pKa of 3.347, solution is titrated with 75.0 mL of a 1.00 M NaOH. What is the final pH? The error interval is +/- 0.2 pH units.
A weak acid, HA, is partially titrated using NaOH. You start with 50.0mL of a 0.100 M HA and add 30.0 mL of a 0.100 M NaOH, and measure the pH of the solution at 7.00. What is the pKA of Ha? What would be the pH of the titration at the equivalence point (when 50.0 mL of NaOH is added)? I got the correct answer for the pKa (6.82), but don't know how to approach the second part. The...
2.77 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 1.33. This solution is titrated with a 0.250 M NaOH solution. 44.2 mL of this NaOH solution is needed to reach the equivalence point. (a) (2 marks) What is the molar mass of HA? (b) (2 marks) What is the value of pKa for HA (aq)? (c) (2 marks) What is the pH at...
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CH3CH2COOH; Pka = 4.87) is titrated with 0.05 M NaOH. A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the location of the...