In industrial environments, benzoic acid, C6H5COOH, is widely used to produce a range of products such as perfumes, dyes, topical drugs, and insect repellents. C6H5COOH + H2O = C6H5COO + H3O+ If this solution above has an initial concentration of C6H5COOH was 0.13 M, what is the pH of the solution? Ka for benzoic acis is 6.5 x 10-5.

In industrial environments, benzoic acid, C6H5COOH, is widely used to produce a range of products such as perfumes, dyes, topical drugs, and insect repellents. C6H5COOH + H2O = C6H5COO + H3O+ If this solution above has an initial concentration of C6H5COOH was 0.13 M, what is the pH of the solution? Ka for benzoic acis is 6.5 x 10-5.

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...

See similar textbooks

Similar questions

2. Dr. Dahm has a 0.4 M solution of nitrous acid. If he takes 3 mL of this solution and dilutes it to 100 mL calculate the pH of the new solution. (assume that no dissociation takes place until the new solution is made.) Ka = 4.6 ´ 10-4 HNO₂(aq) + H₂O(1) NO₂ (aq) H,O*(aq) +
What is the pH of a solution prepared by adding 18.0 mL of 1.51 M nitric acid to 180.0 mL of 0.150 M dimethylamine solution (CH3)2NH? Round your answer to 2 decimal places.
(a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?
Calculate the pH of the weak acid, lactic acid (HC3H5O3), if the concentration is 0.10 mol/L and the Ka value is 1.4 x 10-4
A chemist dissolves 866. mg of pure perchloric acid in enough water to make up 50. mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits. x10 ?
Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a)The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b)The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.
7. Carbonic acid (H2CO3) is a diprotic acid with Ka1 = 4.30 × 10–7 and Ka2 = 5.60 × 10–11 What is the pH in a 1.834 M solution of carbonic acid? 8. The ionization constant, Kb, for weak base, B, is 7.56 × 10–5. What is the pH of a 0.6545 M solution of this base? The equation for the ionization of weak base B as follows. B (aq) + H2O(l) ⇌ BH+(aq) + OH⁻(aq)
The neutralization of an acid with a base yields a salt and usually water in aqueous solution. Calculate the pH when 53.0 mL of 0.217 M hydrochloric acid is mixed with 53.0 mL of 0.217 M sodium hydroxide solution at 25 °C. pH = Calculate the pH when 53.0 mL of 0.217 M of a monoprotic weak acid, HA, is mixed with 53.0 mL of 0.217 M sodium hydroxide solution at 25 °C. The Ka for HA is 4.5 x 10-3. pH =
A chemist dissolves 172. mg of pure barium hydroxide in enough water to make up 120. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits. x10 ?
A chemist dissolves 371. mg of pure potassium hydroxide in enough water to make up 180. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits. 0 x10
What is the pH of a 0.680 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
What is the pH of a 0.430 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?