A 50 mL sample of 0.20 M propionic acid buffer (pKa 4.87 according to Google) has an initial pH of 4.77. After an unknown amount of 0.25 M HCl is added to the buffer, its pH has been lowered to 4.47. Using the Henderson-Hasselbalch equation, determine what volume of HCl was added to the buffer to cause the pH change, as well as the mass of Pr- necessary to return the buffer to its original pH.
A 50 mL sample of 0.20 M propionic acid buffer (pKa 4.87 according to Google) has...
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 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...
You perform a titration using 25.0 mL of a 0.20 M propionic acid (HC3H5O2) as your analyte and 0.25 M NaOH as your titrant. Assume a new 25.0 mL of analyte is used for each step, determine the pH when the following volumes of titrant are used. (Propionic acid Ka= 1.32 x 10^-5) a. 15.0 mL titrant added. b. 25.0 mL titrant added.
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...
You must prepare 100.00 mL of a 0.25 M a buffer at pH = 5.00. The following imaginary buffers are available to you: HA (pKa = 2.61; MW = 99.32 g/mol) HY (pKa = 7.55; MW = 76.31 g/mol) HW (pKa = 4.51; MW = 100.52 g/mol) b. What is the ratio of base species to acid species (141) a. Which weak acid should be used to make the buffer? (2 pts) needed for the buffer according to the Henderson-Hasselbalch...
A buffer made with 150.00 mL of 0.20 M formic acid (Ka=1.8x10-4) and 250.00 mL of 0.10 M formate has a final volume of 1.0 L. What is the pH after 6.00 mL of 1.0 M HCL is added to the buffer?
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CHsCH2COOH; Pk 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 Jocation of the equivalence...
In a preparation of a buffer, 1.0 L of weak acid solution of phenol HOC6H5 with [M] = 0.85 M was mixed with its phenolic salt NaOC6H5 of [M] = 0.80 M. (Ka for HOC6H5 = 1.6 X 10-10) (i)Write equilibrium chemical equation for ionization of HOC6H5 ? (ii)Write equilibrium chemical equation for hydrolysis of the anion OC6H5 ? (iii)Calculate the pH of this solution using the Henderson-Hasselbalch equation? (iv)(a)Calculate the pH after 50 mL of 1.5 M HCl has...
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...
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small amount of nitric acid is added the pH only slightly drops. Write the chemical equation that shows the added nitric acid being neutralized by this buffer. 2. What is the pH of a buffer that is 0.120 M formic acid (HCHO2) and 0.080 M in potassium formate (KCHO2)? The Ka of formic acid is 1.8 x 10^ -4 . 3. The curve shows the...