Calculating the composition of a buffer of a given pHA chemistry graduate student is given 500. mL of a 0.80M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid withK=4.9 × 10a- 10. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH =9.05?You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol,and round it to 2 significant digits.☐ x10☑00.18ArABNew Chrome available:

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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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-10 What A chemistry graduate student is given 125. mL of a 1.70 M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.01? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
4 F M -5 A chemistry graduate student is given 300. mL of a 1.10M benzoic acid (HCH,CO₂) solution. Benzoic acid is a weak acid with K-6.3 x 10. What mass of NaC6H₂CO₂ should the student dissolve in the HC H,CO₂ solution to turn it into a buffer with pH = 4.65? You may assume that the volume of the solution doesn't change when the NaC6H5CO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 Explanation 85°F Mostly sunny 4- 3 Check X $ 4 0 X с F5 % 5 5 E ▬▬ F6 6 Q Search F7 & 7 L F8 A * 8 9 F9 F10 ( 9 *- F11 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Z ) 0 O *+ W F12 | 1 PrtSc + Insert = h Delete Backspace כ' נס 00- ►/11 Ar 1: 3/27 Lock
Which of the following is the best choice for a buffer system? 1.equal volumes of 0.1 M ammonia (NH₃ ) and 0.1 M ammonium chloride (NH₄Cl) 2.equal volumes of 2 M weak acid (HA) and 1 M sodium hydroxide (NaOH) 3.equal concentrations of sodium hydroxide (NaOH) and hydrobromic acid (HBr)) 4.equal concentrations of sodium hydroxide (NaOH) and nitric acid (HNO₃) 5.equal volumes of 2 M weak acid (HA) and 0.5 M conjugate base (A⁻ ))
3. A 0.270 M solution of sodium formate, used in several fabric dyeing and printing processes, is prepared by dissolving it in water. A 75.0-mL sample of this sodium solution is titrated with 0.270 M hydroboric acid (HBr, strong acid) at 25°C. What is the pH of the solution after 15 mL of HBr has been added beyond the equivalence point of the titration. Sodium formate is a basic salt, with the formula HCOONA, and the acid- ionization constant of its conjugate, formic acid (HCOOH), is 1.7 x10-4 at 25°C.
solution. Methylamine is a weak base with K = 4.4 x 104. What mass of A chemistry graduate student is given 125. mL of a 1.80M methylamine (CH₂NH₂): CH3NH₂Cl should the student dissolve in the CH₂NH₂ solution to turn it into a buffer with pH = 10.95? You may assume that the volume of the solution doesn't change when the CH3NH₂Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. M
928 O Acids and Bases Calculating the composition of a buffer of a given pH A chemistry graduate student given 250. mL of a 1.70M nitrous acid (HNO₂) solution. Nitrous acid is a weak acid with K-4.5 x 10 What mass of NaNO, should the student dissolve in the HNO, solution to turn it into a buffer with pH = 3.10? You may assume that the volume of the solution doesn't change when the NaNO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. Explanation Check X 15 Reading schedule S tv Lara V 9 da Ad 19.6 Reduction Po zoom Aa
Which of the following aqueous solutions are good buffer systems? 0.10 M nitrous acid + 0.13 M sodium nitrite 0.31 M ammonium bromide + 0.31 M ammonia 0.29 M hydroiodic acid + 0.23 M potassium iodide 0.16 M potassium fluoride + 0.21 M hydrofluoric acid O 0.39 M acetic acid + 0.25 M potassium acetate
Suppose you have an alkaline buffer consisting of 0.20 M aqueous ammonia (NHs) and 0.10 M ammonium chloride (NH4CI). What is the pH of the solution? 5 Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0 x 10-10. How do the concentration/volumes of the buffer affect the buffer capacity? E.g., 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid solution with 25.0 mL of 0.10 M sodium acetate solution).
Which of the following aqueous solutions are good buffer systems? 0.28 M perchloric acid + 0.19 M sodium perchlorate 0.38 M sodium perchlorate + 0.29 M barium perchlorate 0.16 M potassium hydroxide + 0.20 M potassium chloride 0.30 M ammonia + 0.35 M sodium hydroxide 0.15 M acetic acid + 0.12 M sodium acetate
Which of the following aqueous solutions are good buffer systems? 0.13 M acetic acid + 0.20 M sodium acetate 0.20 M nitric acid + 0.25 M sodium nitrate 0.28 M ammonium nitrate + 0.36 M ammonia 0.13 M potassium hydroxide + 0.22 M potassium chloride 0.32 M nitrous acid + 0.30 M sodium nitrite
In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a) Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b) Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c) Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.
A chemistry graduate student is given 250, ml, of a 1.30 M pyridine (C5H5N) solution, Pyridine is a weak base with Kg = 1.7 x10^-9. What mass of C5H5NHBr should the student dissolve in the C5H5N solution to turn it into a buffer with pH = 5.227 You may assume that the volume of the solution doesn't change when the C5H5NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

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