Chemistry: An Atoms-Focused Approach (Second Edition)
2nd Edition
ISBN: 9780393614053
Author: Thomas R. Gilbert, Rein V. Kirss, Stacey Lowery Bretz, Natalie Foster
Publisher: W. W. Norton & Company
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Chapter 16 Solutions
Chemistry: An Atoms-Focused Approach (Second Edition)
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- Lactic acid, C3H6O3, occurs in sour milk as a result of the metabolism of certain bacteria. Calculate the pH of a solution of 56. mg lactic acid in 250. mL water. Ka for D-lactic acid is 1.5 × 10−4.arrow_forwardA chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.60. What was the concentration of the solution? The Kd of lactic acid is 1.4 104.arrow_forwardWhat is the pH of a solution that consists of 0.20 M ammonia, NH3, and 0.20 M ammonium chloride, NH4Cl?arrow_forward
- The base ethylamine (CH3CH2NH2) has a Kb of. A closely related base, ethanolamine(HOCH2CH2NH2), has a Kb of 3.2105. (a) Which of the two bases is stronger? (b) Calculate the pH of a 0.10M solution of the strong base?arrow_forwardLactic acid, HC3H5O3, is a weak acid; write an equation for its ionization in aqueous solution. If 0.15 M solution of lactic acid has pH = 2.34, calculate the molar concentration of H3O+in the solution. What are the Ka of lactic acid and the degree of ionization of the acid?arrow_forwardWhat is the pH of a 0.0338 M nitric acid, HNO3, solution?arrow_forward
- Consider the titration of 100 mL of 0.25 M formic acid (HCOOH) with 1.0 M NaOH. The Ka of formic acid is 1.77 × 10−4. HCOOH (aq) + NaOH (aq) → NaHCOO (aq) + H2O (l) What is the pH of the formic acid solution before any titrant (NaOH) is added?arrow_forwardWhat is the concentration of hydroxide ion in a 0.45 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 ✕ 10−14.) M What is the pH?arrow_forwardAcetic acid (CH3COOH) is a product of many microbial metabolisms. It forms acetate ion and a hydrogen ion according to the folllowing reaction: CH3COOH(aq) ↔ CH3COO(aq) - + H + K = 2.0 x 10^-5 I'm a total granola type who makes his own vinegar at home. (Vinegar is acetic acid.) I measured the pH of the vinegar I made to be 2.7. (Recall, pH = -log10[H+]). What is the molar concentration of acetic acid in my vinegar, to two decimal placesarrow_forward
- Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.arrow_forwardWhat is the pH of 0.322 M KC6H5Oarrow_forward6a. Draw the Lewis Dot structure for the following diprotic acid: HOOC-CH,-COOH. 38.5 mL of a 1.15 M solution of this acid is titrated to the equivalence point with 0.69 M KOH. Write the balanced equation for this reaction and determine the volume of base needed to completely neutralize the acid.arrow_forward
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