This question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. didadid H3C HO, H3C° O`Na* H3C O Na* H,C OH a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added, b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they?

This question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. didadid H3C HO, H3C° O`Na* H3C O Na* H,C OH a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added, b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they?

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...

See similar textbooks

Similar questions

A solution contains 0.48 mol of HF (pKa = 3.75). 0.24 mol of NaOH are added, and the solution is brought to a final volume of 2 L. Without using a calculator, what is the pH of the solution? A) pH is 3.75 B) pH is less than 3.75 C) pH is greater than 3.75 D) pH is less than 10.25 E) pH is 7.0
predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: name acetic acid acid hydrocyanic acid solution 0.1 M NaCN 0.1 M NH C 0.1 MHONH,Br Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a 2 next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ K₁ formula HCH,CO₂ 1.8x10 HCN 4.9 × 10 10 pH choose one X Ű choose one choose one choose one base 3 Ċ K₂ name formula ammonia NH₂ 1.8×10 hydroxylamine HONH₂ 1.1×108
pH calculation after first equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 48.6 mL of 0.500 M NAOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka, of oxalic acid = 5.60 x 10 and Ka, of oxalic acid = 5.42 x 10
pH: 3 [H*]: 10-3 M [OH]: 10-11 M 14 1 1 7 · 10-7 10-7 10-14 10-14 Dip litmus paper into the solution or add a drop of universal indicator. Use the sliders to change the pH of the solution and observe the effect on the indicators. Click Reset to start over. Help Reset The solution turns orange when the univeral indicator is added to it. Is the solution basic, acidic, or neutral?
explain why the ph doesnt change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the base NH3 and a salt of its conjugate acid NH4CL
||| = O ACIDS AND BASES Determining the strength of acids from a sketch Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Note: Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. = H₂O Solution 1 (Choose one) Explanation Solution 3 (Choose one) Check ▼ ▬▬▬▬▬ Solution 2 (Choose one) ▼ Solution 4 (Choose one) 0/5 X spv7Aqws 3 Allie © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi
a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3? The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.
A solution is made by dissolving 5.315 g of hydrocyanic acid (HCN, 27.062 g/mol, K- 6.17 x 10-10) and 7397 g of potassium cyanide %3D (KCN, 65.116 g/mol) in enough water to make 750.0 mL of solution. Calculate the pH of this solution after 19.74 mL of a 1L814 M NAOH solution has been added to it.
How many milliliters of 0.0416 M KOH are needed to completely neutralize the HCI in 260 mL of a hydrochloric acid solution that has a pH of 2.80? mL 0.0416 M KOH
A solution is prepared that is initially 0.39M in methylamine (CH3NH₂), a weak base, and 0.41 M in methylammonium chloride (CH₂NH3C1). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH]. You can leave out the M symbol for molarity. initial change final [CHÍNH,] [CHÍNH, 0 0 0 0 0 [OH-] 0 X Ś
This question has two parts. Part-I (a) Calculate the pH of a 0.20 M HF solution. The Ka of HF is 6.8*10-4. Show the ICE table and all calculations. Part-II (b) Calculate the pH of a solution containing both 0.20 M HF and 0.10 M HCl? The Ka of HF is 6.8*10-4. Show the ICE table and all calculations.
Consider two solutions; one of a weak acid and one of a strong acid. How is it possible that a solution of weak acid can have a lower pH than a solution of strong acid? Select one: The concentration of the strong acid is higher than the concentration of the weak acid. The concentration of the weak acid is greater than the concentration of the strong acid. The weak acid only partially dissociates in solution. The strong acid completely dissociates in solution.