1) Create a buffer solution of pH= 4.75 from 1M acetic acid (HA)and 1M sodium acetate (NaA) solution (total volume 100 mL): Use PKa = 4.75 Use H-H equation to find the molar ratio of HA and NaA; mix both solutions so that total volume 100 mL or near 100. mL 2) Calculate to find new pH value if 1.00 mL of 10 M HCI is added to the buffer created above. solution

1) Create a buffer solution of pH= 4.75 from 1M acetic acid (HA)and 1M sodium acetate (NaA) solution (total volume 100 mL): Use PKa = 4.75 Use H-H equation to find the molar ratio of HA and NaA; mix both solutions so that total volume 100 mL or near 100. mL 2) Calculate to find new pH value if 1.00 mL of 10 M HCI is added to the buffer created above. solution

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

genow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator%3Dassignment-take [References) How moles of hydrofluorie acid, HF, must be added to 250 mL of 0.34 M sodium fluoride to give a buffer of pH 3.51? Ignore the volume change due to the amany addition of hydrofluorie acid. (K, for HF is 6.8 x 10 4) mol
2. In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186
A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10. ( PREV 1 3 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp 3.8 x 10-10 %3D %3D 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5) [1.6 x 10-10] [3.8 х 1011 [x + 4.20] [x - 4.20] [x + 6.3 x 10-51 [x - 6.3 х 10-5] [x + 1.6 x 101°] [x - 1.6 x 10-10] [x + 3.8 x 10-101 [x - 3.8 x 101°]
Please help out and show full solutions
ave to.) The K of acetic acid is 1.8 | 10. (Note: solid sodium acetate comes as a hydrate NaC2H3O2 3H2O), and thus has a molar mass of 135.08 g/mol.) Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic acid/acetate buffer at pH 4.10, given that you will use 5.00 mL of 1.0 M acetic acid.
Consider a 1.0 L buffer containing 0.095 mol L-1 HCOOH and 0.1 mol L-1 HCOO-. What is the pH of the solution after adding 1.6 x 10-3 mol of NaOH? Express your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15. They are also posted on eClass.
How do I complete problem 1 in a step by step?
Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH
All boxes please
Given: A certain weak acid,HA with a Ka value of 5.61 •10-6 is tutorage's with NaOH. part A: a solution is made by titration 7.00mmol of HA and 3.00 mmol of the strong base. What is the resulting pH? Part B: more strong base is added until the equivalence point is reached. What is the pH of this addition at the equivalence point if the total volume is 34mL?
A buffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate. What will the solution pH be if 0.126 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places) Type your answer...
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).