Tutorial Problem for Weak Base and Strong AcidYou are given an Erlenmeyer flask containing 100.00 mL of 0.100 M B¯ and a buret containing 0.100M HCI. B¯ is a weak acid with a K of 5.9 x 10 º. Calculate the pH of the solution (to 2 decimalplaces) after titrating the following volumes of HCl:What is the pH after 0.0 mL HCI is added? 4.0At this point no strong acid has been added, so you need to solve a weak base pH problem.What volume of HCI is added at the equivalence point (to 0.1 mL)? 49mLWhat is the pH at the equivalence point? 49.At this point no strong acid or weak base remains, so you need to solve a weak acid pH problem for the weak base's conjugate acid.What is the pH after 50.0 mL HCl is added? 49You are in the buffer region here. You need to find the relative ratio of [B-]/[HB]. Make sure to convert K, into K, before using the Henderson-Hasselbalch equation.aWhat is the pH after 150.0 mL HCI is added? 4.0/You are in a region where both the weak conjugate acid and strong acid are present, so you need to solve a strong acid pH problem.

We have to find pH of solution.

utorial Problem for Weak Base and Strong Acid ou are given an Erlenmeyer flask containing 100.00 mL of 0.100 M B and a buret containing 0.100 M HCI. B" is a weak acid with a K, of 5.9 x 10-6. Calculate the pH of the solution (to 2 decimal laces) after titrating the following volumes of HCI: Vhat is the pH after 0.0 mL HCI is added? 40M t this point no strong acid has been added, so you need to solve a weak base pH problem. Vhat volume of HCI is added at the equivalence point (to 0.1 mL)? 49 Vhat is the pH at the equivalence point? 40D t this point no strong acid or weak base remains, so you need to solve a weak acid pH problem for the weak base's conjugate acid. mL Vhat is the pH after 50.0 ml HCI is added? 40 ou are in the buffer region here. You need to find the relative ratio of [B-1/[HB]. Make sure to convert K, into K, before using the Henderson-Hasselbalch equation. Vhat is the pH after 150.0 mL HCI is added? 49 ou are in a region where both the weak conjugate acid and strong acid are present, so you need to solve a strong acid pH problem.

utorial Problem for Weak Base and Strong Acid ou are given an Erlenmeyer flask containing 100.00 mL of 0.100 M B and a buret containing 0.100 M HCI. B" is a weak acid with a K, of 5.9 x 10-6. Calculate the pH of the solution (to 2 decimal laces) after titrating the following volumes of HCI: Vhat is the pH after 0.0 mL HCI is added? 40M t this point no strong acid has been added, so you need to solve a weak base pH problem. Vhat volume of HCI is added at the equivalence point (to 0.1 mL)? 49 Vhat is the pH at the equivalence point? 40D t this point no strong acid or weak base remains, so you need to solve a weak acid pH problem for the weak base's conjugate acid. mL Vhat is the pH after 50.0 ml HCI is added? 40 ou are in the buffer region here. You need to find the relative ratio of [B-1/[HB]. Make sure to convert K, into K, before using the Henderson-Hasselbalch equation. Vhat is the pH after 150.0 mL HCI is added? 49 ou are in a region where both the weak conjugate acid and strong acid are present, so you need to solve a strong acid pH problem.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 57P

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Similar questions

What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Choose a weak-acid/weak-base conjugate pair from which you could prepare a buffer solution with pH = 7.5. Explain how you chose the conjugate pair. Calculate the ratio [weak base]/[weak acid) required to give pH = 7.5.
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
Consider a solution prepared by mixing a weak acid HA and HCl. What are the major species? Explain what is occurring in solution. How would you calculate the pH? What if you added NaA to this solution? Then added NaOH?
8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
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?
a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
(clear handwritten answer please) 29.0 mL sample of a 0.441 M aqueous hypochlorous acid solution is titrated with a 0.429 M aqueous barium hydroxide solution. What is the pH at the start of the titration, before any barium hydroxide has been added?
a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
Directions: Read and analyze the following questions and compute for is unknown in the given problem. 1. Calculate the pH of a buffer made up of 0.544M CH3NH2 and 0.678M CH:NH3°CI- Ka of CH:NH2 is 1.8 x 105. The buffer is made up of CH3NH2 (weak base) and CH3NH3 CI (salt or conjugate acid) 2. Calculate the pH of buffer made of 0.500M NH3 and 0.456M NH.CI, pKo NH3 = 4.74. 3. Calculate the pH of a buffer solution consisting of 0.96OM NH3 and 0.608M NH4". The Ko for NH3 = 1.8 x 105. The reaction is: NH3 + H2O = NH + OH" item 2 and 3
which of the following weak acids would be the best to use to make buffer solution of pH=7.2?