eqreqPreq2req#3Which of the following aqueous solutions are good buffer systems?(Select all that apply.)0.21 M hypochlorous acid + 0.11 M potassium hypochlorite0.25 M nitric acid + 0.20 M sodium nitrate0.25 M ammonium bromide + 0.35 M ammonia0.19 M sodium hydroxide + 0.25 M sodium bromide0.33 M hydrofluoric acid + 0.30 M sodium fluoride20EDSubmit AnswerC000000 F4$4RFShow Hint%5V[Review Topics][References)Use the References to access important values if needed for this question.Retry Entire Group 9 more group attempts remainingCengage Learning Cengage Technical SupportTGMacBook AirA6SBYH&7F7UN00 *8J11FB-M-9KF9OVHdb)0LF10APFILЛ.+ 11alt:13;GNext>command optionSave and ExitF12X FENTY...deleteenre

We are provided with some mixture of compound and we need to find whether it's a good buffer or not.…

Review Topics] References) Use the References to access important values if needed for this question. Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.21 M hypochlorous acid + 0.11 M potassium hypochlorite 0.25 M nitric acid + 0.20 M sodium nitrate 0.25 M ammonium bromide + 0.35 M ammonia 0.19 M sodium hydroxide + 0.25 M sodium bromide 0.33 M hydrofluoric acid + 0.30 M sodium fluoride

Review Topics] References) Use the References to access important values if needed for this question. Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.21 M hypochlorous acid + 0.11 M potassium hypochlorite 0.25 M nitric acid + 0.20 M sodium nitrate 0.25 M ammonium bromide + 0.35 M ammonia 0.19 M sodium hydroxide + 0.25 M sodium bromide 0.33 M hydrofluoric acid + 0.30 M sodium fluoride

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

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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.
A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?
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 solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.
8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.
A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate. Some of the sodium acetate is converted to acetic acid, resulting in a final volume of 650 mL of solution. The pH of the final solution is 4.56. a What is the molar concentration of the acetic acid? b How many milliliters of hydrochloric acid were added to the original solution? c What was the original concentration of the sodium acetate?
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
Blood contains several acid base systems that tend to keep its pH constant at about 7.4. One of the most important buffer systems involves carbonic acid and hydrogen carbonate ion. What must be the ratio of [HCO3] to [H2CO3] in the blood if the pH is 7.40?
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
You have 0.10-mol samples of three acids identified simply as HX, HY, and HZ. For each acid, you make up 0.10 M solutions by adding sufficient water to each of the acid samples. When you measure the pH of these samples, you find that the pH of HX is greater than the pH of HY, which in turn is greater than the pH of HZ. a Which of the acids is the least ionized in its solution? b Which acid has the largest Kd?
Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0

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