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Calculate the pH of a 0.15 M aqueous sol...

Calculate the `pH `of a `0.15` M aqueous solutions of `AlCl_(3)`
Given :`[Al(H_(2)O)_(6)]^(3+)(aq)+H_(2)O(l)hArr[(AlH_(2)O)_(5)OH]^(2+)(aq),K_(a)=1.5xx10^(-5)`

A

`2.82`

B

`5`

C

`9`

D

`11.18`

Text Solution

AI Generated Solution

To calculate the pH of a 0.15 M aqueous solution of AlCl₃, we can follow these steps: ### Step 1: Identify the nature of the salt AlCl₃ is a salt formed from a weak base (Al(OH)₃) and a strong acid (HCl). In solution, Al³⁺ ions will hydrolyze, leading to the formation of H⁺ ions. ### Step 2: Write the hydrolysis reaction The hydrolysis of Al³⁺ can be represented by the following equilibrium reaction: \[ ...
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