Question

Calculate the pH of a 0.22 M solution of aluminum chloride, which dissolves completely to give the hydrated aluminum ion Al(H2O)6 3+ in solution. Al(H2O)6 3+(aq) + H2O(l) ? H3O+(aq) + Al(H2O)5(OH)2+(aq) Ka = 1.4 × 10-5 Report your answer to the hundredths place. Provide your answer below:

          Calculate the pH of a 0.22 M solution of aluminum chloride, which dissolves completely to give the hydrated aluminum ion Al(H2O)6 3+ in solution.
Al(H2O)6 3+(aq) + H2O(l) ? H3O+(aq) + Al(H2O)5(OH)2+(aq) Ka = 1.4 × 10-5
Report your answer to the hundredths place.
Provide your answer below:

Calculate the pH of a 0.22 M solution of aluminum chloride, which dissolves completely to give the hydrated aluminum ion Al(H2O)6 3+ in solution.
Al(H2O)6 3+(aq) + H2O(l) ? H3O+(aq) + Al(H2O)5(OH)2+(aq) Ka = 1.4 × 10-5
Report your answer to the hundredths place.
Provide your answer below:

Added by Kevin R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

12/05/2022

Step 1

22 M. Second, we know that the reaction is a 1:1 ratio, so the concentration of H3O+ will also be 0.22 M. The pH is calculated by the negative logarithm of the H3O+ concentration. So, pH = -log[H3O+] = -log(0.22) = 0.66. Show more…

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Calculate the pH of a 0.22 M solution of aluminum chloride, which dissolves completely to give the hydrated aluminum ion Al(H2O)6 3+ in solution. Al(H2O)6 3+(aq) + H2O(l) ⇌ H3O+(aq) + Al(H2O)5(OH)2+(aq) Ka = 1.4 × 10-5 Report your answer to the hundredths place. Provide your answer below: