Concept explainers
Interpretation:
The pH of the solution with a dissolved salt is to be predicted.
Concept Introduction:
Salt is a strong electrolyte that dissociates completely when added to water.
When a salt contains a cation that comes from a weak base, the cation recombines with water to produce a weak base and hydronium ions and forms an acidic solution.
When a salt contains an anion that comes from a weak acid, the anion recombines with water to produce a weak acid and hydroxide ions and forms a basic solution.
If the anion comes from a strong acid, it does not recombine and is present in the solution as a free ion, without having any effect on the pH of the solution.
The cations that are highly charged and are of a small size form acidic solutions.
The cations from group 1A and selective cations of group 2A, along with the ones from strong bases, will form neutral solutions.
When the cation as well as the anion of the salt hydrolysis, the ionization constant of the species decides the pH of the solution.
For
For
For
Here,
The relationship between
Want to see the full answer?
Check out a sample textbook solutionChapter 16 Solutions
CHEMISTRY(HARDCOVER W/CODE) CUSTOM
- Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3 with deonised water.arrow_forwardGiven that log Kso for Zr(OH)4(s) is 10-54.1, at what pH would the maximum concentration of Zr4+(aq) be 10-3 M?arrow_forwardWhat is the equilibrium hydronium ion concentration of an initially 4.9 M solution of hypobromous acid, HOBr(weak acid) at 25°C (Ka = 2.36 x 10-9)?arrow_forward
- What is the equilibrium pH of an initially 5.1 M solution of hypochlorous acid, HOCl, at 25°C (Ka = 3.5 x 10-8 ; Kw = 1.01 × 10-14)?arrow_forwardCalculate ph of a 0.94 M solution of a weak base with KB= 1.97 x 10^-9arrow_forwardAt 25 °C, the methylammonium ion, CH3NH3*, has a Ka of 2.0 x 10-¹¹. What is the pH of a 0.45 mol.L-¹ solution of methylamine, CH3NH₂?arrow_forward
- Calculate the [H+], [OH], pH, pOH of the unbuffered solution: A) 0. 01M CH3COOH; Ka = 1.8 x 10 -5arrow_forwardDetermine the pH for a 0.267 M NaC3H5O3 solution at 25 C, the Ka for HC3H5O3 is 1.3 x 10^-5arrow_forwardCalculate the pH of a 0.0500M solution of phenylacetic acid, C6H5CH2COOH and 0.0200M with its salt, C6H5CH2COONa. Ka= 4.9 x 10^-5arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning