3 Calculate the pH after 0.16 mole of solid NaOH is added to 1.00 L of each of the following solutions:a. 0.056 M propanoic acid (HC3 H; O2, K, = 1.3 x 10-) and 0.081IM sodium propanoate%3DpH%3Db. 0.56 M propanoic acid and 0.81 M sodium propanoatepH =c. Is the solution in part a still a buffer solution after the NaOH has been added?OyesOno

Here we have to calculate the pH of the respective solution after addition of 0.16 moles of solid…

mole of solid NaOH is added to 1.00 L of each of the following solutions: a. 0.056 M propanoic acid (HC, H502, K, = 1.3 x 10-) and 0.081M sodium propanoate pH = b. 0.56 M propanoic acid and 0.81 M sodium propanoate pH = c. Is the solution in part a still a buffer solution after the NaOH has been added? Oyes Ono

mole of solid NaOH is added to 1.00 L of each of the following solutions: a. 0.056 M propanoic acid (HC, H502, K, = 1.3 x 10-) and 0.081M sodium propanoate pH = b. 0.56 M propanoic acid and 0.81 M sodium propanoate pH = c. Is the solution in part a still a buffer solution after the NaOH has been added? Oyes Ono

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 30QRT

See similar textbooks

Similar questions

In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the major species in solution at equilibrium (besides water), and what are their concentrations?
Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Calculate the pH after 0.032 mole of NaOH is added to 1.00 L of each of the following solutions. a. 0.145 M HONH, (K = 1.1 × 10-) pH = b. 0.145 M HONH, Cl pH = c. pure H₂O pH = d. a mixture containing 0.145 M HONH₂ and 0.145 M HỌNH3 C1 pH =
We mal sourced a How many moles of NH4Cl must be added to 1.0 L of a 0.050-M solution of NH3 to give a buffer solution with a pH of 9.17? The K₂ of NH4* is 5.56*10-10. Assume a negligible change in volume as the solid is added. Enter your answer in non-scientific notation to 3 decimal places. Enter only the number, not the units. tyr
If you add 200 mL of 0. 100 M HCI to 1.00 L solution containing 0,150 M HEN and 0.300 M NaCN, what will the pH of this solution be? K, of HEN - 6.8 x 10-10.