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 isC.What is the pH of the solution? pH =Please provider your answer below.0² 0₂$If you add 5.000 mL, 1.998 M of HC1 to 250.0 mL above solution you prepared, what will be the final pH? Assume that thevolume is additive.Please provider your answer below.→П$ ПIf 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 thevolume is additive.Please provider your answer below.$

A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

4. 250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following questions. A. B. C. A pH buffer solution contains 1.747 mole CH3COOH and 1.630 mole CH3COONa. The volume of the pH buffer solution is What is the pH of the solution? pH = Please provider your answer below. Please provider your answer below. 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. 0² 0₂ 00 Please provider your answer below. S 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. A 0² 0₂

4. 250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following questions. A. B. C. A pH buffer solution contains 1.747 mole CH3COOH and 1.630 mole CH3COONa. The volume of the pH buffer solution is What is the pH of the solution? pH = Please provider your answer below. Please provider your answer below. 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. 0² 0₂ 00 Please provider your answer below. S 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. A 0² 0₂

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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please help on my buffers worksheet for chem
Can you confidently determine if the molarities are accurate? Explain why or why not.
Which of the following constitute a buffer? A. NH3 and KNO3 B. HCN & NaCN C. HF & NaCl D. NaOH & NaCl Group of answer choices C A & C B A, B and C
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
A buffer solution is formed by adding 0.320 moles of solid sodium lactate, NaC₃H₅O₃, to 500.0 ml of 0.800 M lactic acid, HC₃H₅O₃ solution. You may assume that the change in volume is negligible upon addition of the solid.A.) Calculate the pH of the buffer solution.pH = ____B.) Calculate the pH of the buffer solution after the addition of 10.00 ml of 2.00 M HBr.pH = _____
If a buffer solution is made from 450.0 mL of 3.8 M aniline salt mixed with 400.0 mL of 4.1 M aniline, calculate the following:a. The initial pH of the buffer solution.b. The pH of the solution if 20.0 mL of 0.500 M HBr is added to the buffered solution.c. The pH of the solution if 20.0 mL of 0.500 M KOH is added to the buffered solution.
2. A solution of pH 12 will contain a large concentration of (fill in) a. Cl- b. Na+ С. ОН- d. H+ ions. Buffers are substances that keep the pH of a solution stable. In blood, the main buffer system is carbonic acid-bicarbonate in which bicarbonate acts as the a. H+ suppressor b. H+ асceptor c. H+ donor d. H+ processor H,CO3 HCO,- + Looking at the above equation we can deduct that if an acidic solution is injected in the blood of a person, the above equilibrium will move to the a. right b. left The action of buffers in the blood is important to keep the pH stable around а. 7.4 b.7.0 с. 7.8 d. 6.8 In the human stomach, digestive enzymes require a high concentration of a. hydroxide ions b. protons c. cholesterol d.inositol for optimal function.
a. Calculate the number of moles of HCI(g) that must be added to 1.0 L of 1.1 M NaC,H3O2 to produce a solution buffered at pH = pK,. K. (HC,H3O2) = 1.8 x 10-6 Number of moles = mol b. Calculate the number of moles of HCI(g) that must be added to 1.0 Lof 1.1 M NaC,H3 O, to produce a solution buffered at pH = 4.20. KA(HC,H;O2) = 1.8 x 10-5 Number of moles = mol c. Calculate the number of moles of HCI(g) that must be added to 1.0 L of 1.1 M NaC,H3O2 to produce a solution buffered at pH = 5.00. K. (HC, H, O2) = 1.8 x 10-5 Number of moles = 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
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 Titration of 25 mL of .1 M CH3CO2H With .1 M NaOH. Calculate The pH After Adding The Following Volumes of NaOH: a. 0 mL b. 12.5 mL. c. 20 mL d. 25 mL. e. 37.5 mL. I do know the answers, I just don't know the way to get to these answers. a. pH = 2.87 b. pH = 4.74 c. pH = 5.34 d. pH = 8.72 e. pOH = -log(.0192 M) = 1.72 pOH 14-1.72 = 12.28 pH (I just know the last steps to the answer for part e, but don't know all the other steps to get to answer).
A 125.0 mg sample of an unknown, monoprotic acid was dissolved in 100.0 mL of distilled water and titrated with a 0.050 M solution of NaOH. The pH of the solution was monitored throughout the titration, and the data were collected in the table below. Determine the Ka of the acid and use the data table to identify the unknown acid. volume of OH- added (mL) pH 0 3.09 5 3.65 10 4.10 15 4.50 17 4.55 18 4.71 19 4.94 20 5.11 21 5.37 22 5.93 22.2 6.24 22.6 9.91 22.8 10.2 23 10.4 24 10.8 25 11.0 30 11.5 40 11.8 Determine the Ka. Use the data table below to identify the name of the unknown acid. Ka pKa acetic 1 $$CH3COOH(aq)+H2O(l)H3O+(aq)+CH3COO−(aq) 1.76x10-5 4.75 benzoic 1 $$C6H5COOH(aq)+H2O(l)H3O+(aq)+C6H5COO−(aq) 6.25x10-5 4.20 formic 1 $$HCOOH(aq)+H2O(l)H3O+(aq)+HCOO−(aq) 1.77x10-4 3.75 oxalic 1 $$HOOCCOOH(aq)+H2O(l)H3O+(aq)+HOOCCOO−(aq) 5.9x10-2 1.23 2…