Benzoic acid, HC7H502, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 X 1 0 -5 . A solution of sodium benzoate, NaC7H502, in water has a concentration of 0.015 mol.dm-3 . a) What is the equilibrium concentration of benzoic acid in the sodium benzoate solution? b) What is the pH of this solution?

Benzoic acid, HC7H502, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 X 1 0 -5 . A solution of sodium benzoate, NaC7H502, in water has a concentration of 0.015 mol.dm-3 . a) What is the equilibrium concentration of benzoic acid in the sodium benzoate solution? b) What is the pH of this solution?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.72PAE

See similar textbooks

Similar questions

Benzoic acid (C₂H5CO₂H), a weak acid, has a dissociation constant of K=6.3x10^-5. 1. Write the equilibrium equation of the solution. 2. Write the Ka expression of the equilibrium involved. 3. What is the equilibrium concentration of all species if the initial concentration is a.) 0.0315M, b) 0.315M² 4. What is the resulting pH and pOH for a) and b)? 5. What is the %ionization of benzoic acid in a) and b) solution?
Nitrous acid (HNO2) is an essentially nonvolatile acid that ionizes in water with an equilibrium constant of 4 x 10-4 mol/liter. Assume that 10 mmol of nitrous acid are added to a liter of water that is open to the atmosphere.a. List all chemical species that you expect to occur in the water. For which of these do you know the concentration a priori? (you may assume the water has reached equilibrium with the air, and therefore H2CO3* concentration is approximately 12 mM, per Henry’s law)b. Write every equation that constrains the composition of the system at equilibrium identifying each as a mass conservation, mass action, or electroneutrality constraint.
Consider the following dissociation reaction of the weak acid, HA: HA + H2O ⇔ H3O+ + A- What is the name given to the equilibrium constant of this type of reaction? A. The rate constant. B. The acidity constant. C. The acid ionisation constant. D. The buffer constant
The acid - dissociation constant (Ka) of chlorous acid (HCIO2) is 1.1 x 10-2 Calculate the concentrations of H+. CIO 2-, and HCIO2 at equilibrium if the initial concentration of HCIO2 is 0.0125 M
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 0.060 M . Express your answer using two significant figures. part B Calculate the equilibrium concentration of C6H5COO−C6H5COO− in the solution if the initial concentration of C6H5COOHC6H5COOH is 0.060 MM . Express your answer using two significant figures.
There is a buffer solution containing 0.50 M acetic acid (CH3COOH, Ka= 1.8 X 10-5) and 0.50 M sodium acetate (CH3COONa). Calculate the pH of this solution. CH3COOH(aq) ↔ H+(aq) ↔ CH3COO-(aq) early 0.50 ~ 0 0.50 change - x + x + x equilibrium 0.50 - x x 0.50 + x
Calculate the acid ionization constant (pKa) for the acid with a 0.775 M solution of a weak acid (HA) that has a pH of 3.38.
Benzoic acid is a weak acid that has antimicrobial properties. Its sodium salt, sodium benzoate, is a preservative found in foods, medications, and personal hygiene products. Benzoic acid ionizes in water: C6H5COOH(aq) ⇌ C6H5COO−(aq) + H+(aq) The pKa of this reaction is 4.2. In a 0.66 M solution of benzoic acid, what percentage of the molecules are ionized?
A student determine the k a of an acid to be 5.8722 x 10 -4. What is the pK a? 4.0532 1.0014 3.2312 4.9060 4.4782
The ionization constant of a very weak acid, HA, is 1.6×10-9. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] = _______ mol/L [A-] = __________ mol/L [HA] = _________ mol/L pH = ___________
How do you find the equilibrium constants value for Na2CO3,NH4Cl,ZnCl2 and KAl(SO4)2. And would they Ka or Kb?
The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of the acid if the pKa of the acid 5.74? A. 0.657 M B. 0.387 M C. 0.315 M D. 0.0576 M E. 0.274 M