A. How would you prepare 1.5L of a buffer of pH = 4.00 using 0.25M formic acid and solid sodium salt of the acid? (ignore volume changes) In your answer, indicate the volume of solution you would use and the mass of the salt you would use. Show all calculations. In order to make the buffer,

1. What would be the pH of buffer containing 137ml of 3.50M boric acid and 228ml of 1.90M lithium borate. The pKa of buffer system is 13.80.  solved answer pH= 13.76 2. What would be the pH of the buffer from question 1, after adding 84.5ml of 0.71 M KOH (strong base) to buffer? ??

Which statement is incorrect? Select one: a. The endpoint is when the indicator changes color. b. The volume of solution in the buret should be recorded when the endpoint is reached. O c. When the indicator changes color and remains, 2 more drops of the solution in the buret should be added. d. Phenolphthalein will go from a colorless solution to a pink solution for the addition of NaOH to an acid solution. e. It is good practice to place the flask over a white background to better observe the color change of the solution. ge Next page Experiment #10 - Molecular étv

It was assumed: a) Before any acetic acid was added, essentially all the indicator was in the In- form.  b) After the HCl was added, essentially all the indicator was in the HIn form.  Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine: 1) The fraction fo the indicator in the HIn form in solution B before any of solution A was added 2) The fraction of the indicator in the In- form after the HCl was added.

Give detailed Solution..no need handwritten answer (don't use Ai for answering this)

Calculate the pH of the buffers prepared in the following ways: a. by mixing 50.00 mL of 0.200 M ammonium nitrate, NH,NO,, with 25.00 mL 0.200 M NaOH b. by neutralizing half of the acid in 100.00 mL of 0.200 M ammonium nitrate solution with 1.0 M NaOH c. by mixing 60.00 mL of 0.400 M sodium formate (NaCHOO) with 40.00 mL 0.360 M HCI d. by mixing 80.00 mL of 1.00 M NH, with 40.00 mL of 1.00 M HCI e. by mixing equal volumes of 1.00 M NH, and 0.50 M HCI

How many mol of HCI would have to be added to 0.692 L of a 4.813 M B: in order to obtain a buffer with a pH of 8.79? (The Kb for B: is 6.05 10-2). Assume there is no volume change. mol HCI

A 10.0 ml. solution of 0.300 M NH, is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCI solution: 0.00 ml., 10.0 ml., 30.0 ml., and 40.0 ml.. Round your answer to 3 decimal places. Note: Reference the K, of acids at 25 °C and K, of bases at 25 °C tables for additional information. Part 1 of 4 0.00 ml. Added, pH= Part 2 of 4 10.0 mL Added, pH = 0.. 0.8