A buffer contains 0.040 mol of lactic acid (pK₁ = 3.86) and 0.065 mol of sodium lactate per liter. H₂C. OH Lactic acid OH Calculate the pH of the buffer. H₂C OH Sodium lactate Calculate the change in pH after adding 7.0 mL of 0.30 M HCl to 1.0 L of the buffer. O Na+ Calculate the change in pH after adding 7.0 mL of 0.30 M HCl to 1.0 L of pure water. buffer pH: 4.07 buffer pH change: water pH change: 0.4 Incorrect 3.15 Incorrect units units

A buffer contains 0.040 mol of lactic acid (pK₁ = 3.86) and 0.065 mol of sodium lactate per liter. H₂C. OH Lactic acid OH Calculate the pH of the buffer. H₂C OH Sodium lactate Calculate the change in pH after adding 7.0 mL of 0.30 M HCl to 1.0 L of the buffer. O Na+ Calculate the change in pH after adding 7.0 mL of 0.30 M HCl to 1.0 L of pure water. buffer pH: 4.07 buffer pH change: water pH change: 0.4 Incorrect 3.15 Incorrect units units

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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If you wanted to create a buffer with a pH = 3.2, what substances would you choose to make the buffer? Weak Acid K, pK, HCIO, 7.2 x 10-3 1.94 HNO, CH,COOH H,CO, 4.0 x 10-4 3.39 1.8 x 10-5 4.75 6.3 x 10-8 6,35 HBRO 2.8 x 10-9 8.55 HCO, 4.0 x 10-13 10.33 HNO, and NO, CH;COOH only HNO, only HCO; and CO,2 HBГО and BrO HCIO, and CIO, CH3COOH and CH;COO
Use an acid-base titration to calculate the molar mass of an acıd. A 0.6758-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized barium hydroxide. The equivalence point in the titration is reached after the addition of 30.31 mL of 9.152x10 ² M barium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid. g/mol
-4 A chemistry graduate student is given 500. mL of a 1.60M nitrous acid (HNO₂) solution. Nitrous acid is a weak acid with K =4.5 × 10 NaNO₂ should the student dissolve in the HNO₂ solution to turn it into a buffer with pH. = 3.19? What mass of You may assume that the volume of the solution doesn't change when the NaNO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A buffer is formed by adding 1.0 mol of dimethylamine, (CH3)2NH, and 1.0 mol of dimethylammonium, (CH3)2NH2+, in a 1.0 L container. If a 10.0 mL sample of this buffer is diluted to 1000 mL with water, what is the pH of the diluted buffer?For dimethylamine, Kb = 5.4 × 10-4Insert your answer in decimal notation rounded to 2 decimal digits.
We have to make a borate buffer with pH = 8.8 where the boric acid pKa = 9.00. If we start with a 1 liter of 0.1 M boric acid solution, what mass of hydroxide ions should be added to get the desired pH? Boric acid has the molecular formula B (OH) 3 and the borate ion B (OH)
What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of a buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (The Ka for acetic acid is 1.80 ×10-5.)
A buffer solution contains 1.250 mol of phenol, C6H5OH, and 0.950 mol of sodium phenoxide, C6H5ONa, in 1.00 L of solution. Ka = 1.30 x 10-10. a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.525 mol of NaOH? (assume no volume change upon the addition of the NaOH) c. To the buffer produced in part a, what is the pH of the buffer after the addition of 0.225 mol of HCI? (assume no volume change up the addition of the HCI)
6. A buffer solution contains 0.120 moles of propionic acid, HC3H502, and 0.100 moles of sodium propionate, NaC3H5O2, in 1.00 L of solution. Ka = 1.32 x 10-5 a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.010 mol of NaOH? c. Beginning with the initial buffer from part a, what is the pH of the buffer after the addition of 0.010 mol of HBr?
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
5
Consider a buffer made by dissolving 0.140 mol cyanic acid, HCNO, and 0.11 mol potassium cyanate, KCNO, in enough water to make a 1-L solution. Assuming that the volume does not change, what is the pH of the buffer before any acid or base is added? Ka = 3.5 x 10-4 O 3.46 O 3.25 3.36 O None of the above
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