a. A0.100 M solution of NaOH has a higher pH than a 0.100 M solution of Ba(OH)2. TRUE / FALSE b. What is the pH of a solution made by dissolving Fe(NOs)2 in water? ACIDIC / NEUTRAL / BASIC c. If you have a buffer solution made from 1 parts ammonia and 2 parts ammonium ions, what is the pH of that solution? 8.95 / 9.55

a. A0.100 M solution of NaOH has a higher pH than a 0.100 M solution of Ba(OH)2. TRUE / FALSE b. What is the pH of a solution made by dissolving Fe(NOs)2 in water? ACIDIC / NEUTRAL / BASIC c. If you have a buffer solution made from 1 parts ammonia and 2 parts ammonium ions, what is the pH of that solution? 8.95 / 9.55

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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8.When a small amount of 12 M HNO3(aq) is added to a buffer solution made by mixing CH3NH2(aq) and CH3NH3Cl(aq), the pH of the buffer solution changes from 10.64 to 10.62. Which of the following equations represents the reaction that accounts for the fact that the pH does not change significantly when the HNO3(aq) is added? a) CH3NH2(aq) + H+(aq) → CH3NH3+(aq) b)CH3NH3+(aq) + H+(aq) → CH3NH42+(aq) c) NO3- (aq) + H+(aq) → HNO3(aq) d) OH- (aq) + H+(aq) → H2O(l)
7. a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the solution if the Kb for CH3NH2 is 4.4x10^-4?
You are given a diprotic acid H₂A. 10.00 mL of this acid solution of 0.0200 M is titrated with NaOH solution of 0.0213 M (the concentration is NaOH is standardized by sulfamic acid). pka, = 4.53, pka₂ = 8.59 All the following questions are based on the above information. Calculate Vel O a. 9.39 mL O b. 18.9 ml O c. 10.00 ml. O d. 9.35 mL Calculate V.2- O a. 15.43 ml. Ob. 20.00 ml. O c. 18.78 ml O d. 24.85 mL.
2. What is the pH of a 0.01 M HNO3 solution? What is the ratio of acid to conjugate base for this system? (Ka= 2.4 x 10^1)
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2. You are given three solutions: HCI (Solution A); NaOH (Solution B); pH = 8.76 solution (Solution S). You are asked to prepare the following solutions, starting with Solution S, and adding small amounts of Solution A or Solution B %3D to it. a. A solution of pH = 7.00 To Solution S, carefully add small amounts of Solution A/ Solution B (Circle one) till the required pH is reached. b. A solution of pH = 6.54 To Solution S, carefully add small amounts of Solution A / Solution B (Circle one) till the required pH is %3D reached. A solution of pH = 9.87 To Solution S, carefully add small amounts of Solution A / Solution B (Circle one) till the required pH is С. %3D reached.
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A buffer solution is made that is 0.409 M H2S and 0.409 M in NaHS. If Ka1 for H2S is 1.00x10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.087 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
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Now that we are getting closer to the winter holidays, I like lighting candles around my house. I particularly like the smell of cinnamon this time of year. The smell of cinnamon comes from a compound related to cinnamic acid (Ka = 3.63 x 10-5). What is the pH of a 0.350 M solution of cinnamic acid? b. What is the pOH of 0.350 M HNO3?
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