I need help with part b for number 6 RevA buffer contains 0.14 mol of propionic acid (C2H,COOH) and 0.15 mol of sodium propionate (C2H5COONA) in 1.20 L.Part AYou may want to reference (Page) Section 17.2while completing this problem.What is the pH of this buffer?Express the pH to two decimal places.pH = 4.92Previous AnswersCorrectThis buffer is composed of 0.14 mol of propionic acid and 0.15 mol of its conjugate base, proppropionic acid is 4.9. The Henderson-Hasselbalch equation is used to determine the pH of thisacid and base forms are dissolved in the same volume, you can calculate the pH directly usingmoles as follows:0.15molpH = pKa +log0.14molPart BWhat is the pH of the buffer after the addition of 0.02 mol of NaOH?Express the pH to two decimal places.pH =SubmitPrevious Answers Request AnswerP Type here to searchCo

Given: 0.14 mol of propinoic acid 0.15 mol of sodium propionate Volume is 1.20 L 0.02 mol of NaOH

A buffer contains 0.14 mol of propionic acid ( C2H;COOH) and 0.15 mol of sodium propionate ( C2H;COONA) in 1.20 L. Part A You may want to reference (Page) Section 17.2 while completing this problem. What is the pH of this buffer? Express the pH to two decimal places. pH = 4.92 Previous Answers v Correct This buffer is composed of 0.14 mol of propionic acid and 0.15 mol of its conjugate base, pr propionic acid is 4.9. The Henderson-Hasselbalch equation is used to determine the pH of th acid and base forms are dissolved in the same volume, you can calculate the pH directly using moles as follows: 0.15mol pH = pKa + log o.14mol Part B What is the pH of the buffer after the addition of 0.02 mol of NaOH? Express the pH to two decimal places. pH =

A buffer contains 0.14 mol of propionic acid ( C2H;COOH) and 0.15 mol of sodium propionate ( C2H;COONA) in 1.20 L. Part A You may want to reference (Page) Section 17.2 while completing this problem. What is the pH of this buffer? Express the pH to two decimal places. pH = 4.92 Previous Answers v Correct This buffer is composed of 0.14 mol of propionic acid and 0.15 mol of its conjugate base, pr propionic acid is 4.9. The Henderson-Hasselbalch equation is used to determine the pH of th acid and base forms are dissolved in the same volume, you can calculate the pH directly using moles as follows: 0.15mol pH = pKa + log o.14mol Part B What is the pH of the buffer after the addition of 0.02 mol of NaOH? Express the pH to two decimal places. pH =

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.78QE

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.) a. Calculate the pH of this solution. b. Calculate the pH after 0.10 mole of HCl has been added to the original solution. Assume no volume change on addition of HCl. c. Calculate the pH after 0.20 mole of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
a Draw a pH titration curve that represents the titration of 50.0 mL of 0.10 M NH3 by the addition of 0.10 M HCl from a buret. Label the axes and put a scale on each axis. Show where the equivalence point and the buffer region are on the titration curve. You should do calculations for the 0%, 30%, 50%, and 100% titration points. b Is the solution neutral, acidic, or basic at the equivalence point? Why?
A buffer solution is prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M and pH is 4.20. a. Calculate the concentration of C6H5NH3+ in this buffer solution. b. Calculate the pH after 4.0 g NaOH(s) is added to 1.0 L of this solution. (Neglect any volume change.)
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
A buffer is made up of 239 mL of 0.187 M potassium hydrogen tartrate (KHC4H4O6) and 137 mL of 0.288 M potassium tartrate (K2C4H4O6). Ka for is (H2C4H4O6)4.55105. Assuming volumes are additive, calculate (a) the pH of the buffer. (b) the pH of the buffer after adding 0.0250 mol of HCI to 0.376 L of the buffer. (c) the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer.