Please show all work for full credit. .4ac quadratic formula:bvb-4ac You are titrating 60.00 mL of...
You are titrating 100.00 mL of 0.4200 M propanoic acid ( CH3CH2CO2H) with 1.000 M KOH Find the pH at the following points during the titration. The Ka for propanoic acid is 1.34 x 105 15. (32 pts) a) 0.00 mL of 1.000 M KOH b) 10.00 mL of 1.000 M KOH c) 21.00 mL of 1.000 M KOH d) 42.00 mL of 1.000 M KOH e) 60.00 mL of 1.000 M KOH f) Circle the best indicator for this...
Write legibly. Show your work for full credit. All calculations should be performed for an aqueous solution at a temperature of 25 °C. 1. Calculate the pH after the addition of 0.00, 10.00, 25.00, 40.00, 45.00 ,50.00, 51.00, 55.00, 60.00, and 70.00 mL of 0.1000 M of HCl in the titration of 50.00 mL of 0.1000 M NaOH.. 2. Make a graph of pH versus the volume of HCl added. (Use Excel Spread Sheet)
Please show all work. Be sure to answer all parts. Find the pH of the two equivalence points and the volume (mL) of 0.0496 M KOH needed to reach them in the titration of 17.3 mL of 0.130 M H2CO3. Second equivalent point First equivalent point mL KOH mL KOH pH= pH =
1) Calculate the pH for the titration of 60.00 mL of a 0.1500 M methylamine with 45.00 mL of 0.1000 M HCl. Kb = 4.42 × 10−4 2) One liter of a pH 5.00 propionic acid buffer with a total concentration of 60 mM must be prepared. Calculate the mmols propionic acid and sodium propionate needed to prepare the buffer. Ka = 1.34 x 10-5 for propionic acid please show your work and clear net answer
Please workout solution, thank you! L__ of 15 points) A student pipettes 25.00 mL of 0.150 M methylamine (CH3NH2) solution into a flask, titrating the solution with 0.150 M HCI. a) What is the pH when 0.00 mL of the titrant has been added? b) What is the pH when 25.00 mL of the titrant has been added? c)Indicate which of the following indicators should be used for the titration? Indicator pKa Indicator pka Cresol red 1.5 Erythrosin B 2.9...
II vino Show all work for full credit. 1. A titration curve was drawn for 25 mL of HCl being titrated with NaOH using the following information: a. The starting pH is 1.5. b. The y equivalence point is at 17.3 mL of base. c. The concentration of the base is 0.005 M. d. What is the concentration of the HCl used?
3. A 30.0 mL sample of 0.165 M propanoic acid (HC3H5O2) is titrated with 0.300 M potassium hydroxide. Calculate the pH under the following conditions. Please write your final answers in the box. Show your work below and/or on scratch paper. (5 points) K CaH02 7.7 x 100 K, HCsHsO2 1.3 x 10 Answer Question What is the initial pH of propanoic acid before titrating with KOH? b a. 2.834 What is the pH after the addition of 10.0 mL...
Please record your answers directly onto these pages. Show all work for full credit. 1. A buffer solution is prepared by adding 60.00 mLs of 0.345 M NaH3EDTA and 65.00 ml.s of 0.350 M Na2H2EDTA. (The fully protonated acid is HAEDTA, a tetraprotic acid) a. Give the NIE associated with each K. Kal = 1.02 x 10-2 Kay= 2.14 x 10-3 Ka3 -6.92 x 10-7 K4 = 5.50 x 10-11 b. Calculate the pH of this buffer solution. c. Calculate...
Please show all work. Thank you. 3. 25.0 mL of 1.25 M HNO3is titrated with 0.95 M KOH. Calculate the pH of the solution (a) after the add'n of 20.0 mL of KOH, (b) at the stoichiometric pt., (c) after the add'n of 40.0 mL of KOH
Please show all work, handwritten please. Thank you. Acid-Base Equilibria; Buffers, and Titrations Be sure to show ALL YOUR WORK! 1. Consider the titration of a 35.0 mL sample of 0.105 M HBr with 0.200 M KOH. Determine each of the following quantities. a. the initial pH b. the volume of KOH solution required to reach the equivalence point c. the pH at the equivalence point 2. Use the table of indicators below to choose the best indicator for the...