4. (20 pts) 25 mL of 0.12M solution of HClO2 (pKa=1.92) is titrated with a 0.087M...
25 mL of 0.12M solution of HClO2 (pKa=1.92) is titrated with a 0.087M solution of KOH. Find the pH - Initially before adding any KOH - After 8.5 mL of KOH is added - At the equivalence point of the titration - After 39 mL (total) of KOH is added
4. (20 pts) 25 ml of 0.12M solution of HCIO2 (pkae1.92) is titrated with a 0.087M solution of KOH Find the pH • Initially before adding any KOH After 8.5 mL of KOH is added At the equivalence point of the titration • After 39 mL (total) of KOH is added
3) A weak monoprotic acid has a pKa 6.15. 50.00 mL of an 0.1250M aqueous solution of this weak acid is titrated with 0.1000M NaOH. a) What is the equivalence point volume and 2 equivalence point volume for this titration? Find the pH b) before the titration begins; c) after 20.00 mL of the NAOH has been added, d) after 62.50 mL of the NaOH has been added; and e) after 85.00 mL of the NAOH has been added. 4)...
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 40.0 mL solution of 30.0 M of succinic acid (aq) is titrated with 0.300 M of KOH. Find the pH of the solution. (pKa=4.2). A) initially B) 1/2 way to the equivalence point C) at the equivalence point D) 1.00 mL past the equivalence post 2) sketch the titration curve that results from above titration. Label A) only a weak base present. B) Buffer. C) Only a weak acid present. D) Strong base in excess. E) pH = pKa
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...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
can u help? im not sure about my answers Question 6 2 pts A 50.0 mL sample of 0.20 M HCl(aq) is titrated with 0.10 M NaOH(aq) (adding NaOH to HCI). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. Assume that the volumes of the solutions are additive. NaOH HCI Parta) [Select ] after 1) After adding 20 mL of the NaOH solution, the...
Question 1 5 pts If 27.2 mL of 0.102 M acid with a pKg of 5.44 is titrated with 0.1 M NaOH solution, what is the pH of the titration mixture after 11.3 mL of base solution is added? 5 pts Question 2 If 20.7 mL of 0. 102 M acid with a pKa 4.33 is titrated with 0.107 M NAOH solution, what is the pH of the acid solution before any base solution is added? Question 3 5 pts...
1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...