The acid dissociation constant Kof trimethylacetic acid (HC( (HC (CH₂)₂CO₂) is 9.33 × 10¯ Calculate the pH of a 1.1M solution of trimethylacetic acid. Round your answer to 1 decimal place. pH = X
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![The acid dissociation constant, \( K_a \), of trimethylacetic acid \((\text{HC(CH}_3\text{)}_3\text{CO}_2)\) is \( 9.33 \times 10^{-6} \).
Calculate the pH of a 1.1 M solution of trimethylacetic acid. Round your answer to 1 decimal place.
\[ \text{pH} = \text{[input box]} \]
There is an input box for entering the pH value, along with an "X" button, presumably to clear the entry, and a refresh button to reset the question or input.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F812a333f-5569-4734-822a-5aed0505f779%2F63fb70d0-8e2f-4696-b84a-9443d2f81bf1%2F9wsjh_processed.png&w=3840&q=75)
Ka of trimethylacetic acid (HC(CH3)3CO2) = 9.33 × 10-6
Concentration of trimethylacetic acid (C) = 1.1 M
pH of the solution = ?
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