Styles2. Use a 100-mL beaker to make a 50 ml of the sodium acetate (NaA)/acetate (HA) buffersolution, as shown in the table. Measure and record the pH. Pipette 25 ml of this buffersolution and place it in a new 50-ml beaker. Add 1 ml of 1 M HCI or 1 M NAOH to eachseparate beaker and mix well. Measure and record pH.Table 2:Buffered solution (acetate)Calculated pHMeasuredpH25 mL 1.0 M NaAc + 25 ml 1.0M HA4.234.1225 ml above mix buffer +1 ml 1.0 M HCI4.2225 ml above mix buffer + 1 ml 1.0 M NAOHD, Focus* The pka of acetic acid is 4.75.

pH of the buffer can be calculated using Hasselbach-Henderson equation pH =pKa +log [NaA][HA]

Answered: Styles 2. Use a 100-mL beaker to make a…

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...

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Part A Use the Henderson-Hasselbalch equation to calculate the pH of each of the following solutions. a solution that is 0.175 M in HC2H3O2 and 0.100 M in KC2H3O2 Express your answer using two decimal places. ? pH = Submit Request Answer Part B a solution that is 0.200 M in CH3NH2 and 0.110 M in CH3 NH3B. Express your answer using two decimal places. ? pH = Submit Request Answer
In the acid-base titration lab (Lab X), we used NaOH to neutralize a diluted H5SO4solution. i) Write a balanced chemical reaction for this neutralization reaction: ii) Identify the acid and the base in this reaction. iii) We used an indicator (Phenolphthalein) in this titration. Can we do this titration without an indicator? Briefly explain your answer. iv) When we started adding NaOH to the acid solution, it turned pink and quickly the color disappeared. What is the reason for this observation? v) Using the above balanced reaction, find the volume of 1.6 M NAOH needed to neutralize 25.0 mL of 2.0 M H2S04 solution (give the answer in mL)? For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac)
Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...
A 1.0 L buffer solution has 0.15 mol L1 HCN and 0.60 mol L-1 KCN. The K, of HCN is 4.9 x 10-10. Which action will destroy the buffer? A. Add 0.50 mol HCN to the buffer. B. Add 0.50 mol KCN to the buffer. C. Add 0.50 mol HCl to the buffer. D. Add 0.50 mol KOH to the buffer. E. More than one of the above will destroy the buffer.
250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following questions. A. B. A pH buffer solution contains 1.747 mole CH3COOH and 1.630 mole CH3COONa. The volume of the pH buffer solution is C. What is the pH of the solution? pH = Please provider your answer below. 0² 0₂ $ If you add 5.000 mL, 1.998 M of HC1 to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. Please provider your answer below. → П $ П If you add 5.000 mL, 1.998 M of Ba(OH)₂ to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. Please provider your answer below. $
Write out a chemical equation. (The chemical equation, for example, is NaOH + HCl ® HOH + NaCl.) Explain what the equivalence point is, what the pH is at the equivalence point in this reaction and why the pH is what it is.
Can you help me with this?
A) how many miles of NaOH were required to reach the equivalence point ? B) how many moles of NaOH were required to reach the equivalence point ? C) How many moles of CH3COOH were present in the initial sample of acid ? D) what was the exact concentration of the initial acetic solution ?
1. Suppose you have a solution of 25.0 ml pure water. You add add three drops of 1.0 M HCI to the pure water solution. Find the pH change of solution after addition of HCI. 2. Find the pH change of 25.0 ml pH buffer (0.20 M HAC + 0.20 M NaAc) after adding three drops of 1.O MM HCI. Use the editor to format your answer
Please answer the 3 boxes for ph
The following are steps that you might need to perform in order to prepare a buffer. Choose the answer that puts the steps in the correct order. A. Add enough water to reach the final volume needed. B. Mass out the solid buffer salt. C. Take the pH of the buffer. D. Add -60% of the total volume of water. E. Add acid or base to reach the desired pH. Select one: O B, D, C, E, A O B, A, C, E ⒸB, D, C, E, Cx B, D, A, C, E
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

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