Based on your structures above, provide explanations on why some of the observed retention factors change with pH of the mobile phase.

In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two  methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…

The pKa of acetic acid is 4.76. What volume of 2 M HCl can be added to 100 mL of 0.1M acetate buffer at pH 4.76 before it is 90% titrated (i.e., is at the end of its buffering capacity)?

Prepare 500ml of 2M of Tris-HCI buffer with pH 8.9. Tris base molecular weight is 121.14 g/mol. Explain the preparation procedure for Tris buffer.

Need hand written solution only

What must be the minimum concentration of hydrocyanic acid in 1.00L buffer solution of a pH 9.8 hydrocyanic acid/sodium cyanide buffer if the pH changes by 0.20 units when 0.032 moles HCI are added? Click here for the table of lonization Constants of Weak Acids. Provide the answer with 3 decimal places. DO NOT use the scientific notation.

It is desired to prepare a buffer solution with a pH equal to 10 with the ethylamine-ethylammonium chloride pair:   How many grams of ethylammonium chloride (C2H5NH3^+Cl^- ) should be added to 750 mL of ethylamine (C2H5NH2) 0.05 M to obtain this solution? Assume that the volume of the solution remains constant.

What is the pH of the solution of 20mL IM H,PO, (pKa values = 2.16, 7.21, and 12.32) at the given points in the titration with a 1 M NaOH solution. (a) Initially (b) After 10 mL of NaOH. (c) After 20 mL of NaOH (d) After 35 mL of NaOH (e) After 50 mL of NaOH (f) After 70 mL of NaOH

6. What is the change in pH that occurs when 0.50 mmol strong acid is added to the 100 mL solution of 0.0200 M in lactic acid and 0.0800 M in sodium lactate 2 (Kalactic acid)= 1.38 x 10- ) (round to 3 digits after the point).

Determine the pH during the titration of 33.6 mL of 0.231 M triethylamine ((C2H5)3N, Kb = 5.2\times 10-4) by 0.231 M HNO3 at the following points. (a) Before the addition of any HNO3 (b) After the addition of 12.5 mL of HNO3 (c) At the titration. midpoint (d) At the equivalence point (e) After adding 49.4 mL of HNO3