The image shows a chemical equation related to acid-base chemistry. The formula is expressed as: \[ C_T = [H^+] \left( 1 + \frac{[H^+]}{K_a} \right) \] Below the equation, two values are provided: - \( C_T = 9.5 \times 10^{-5} \) - \( K_a = 10^{-7.6} \) The unknown in the equation is: \[ [H^+] = ? \] This equation is used to find the concentration of hydrogen ions \([H^+]\) in a solution. It relates the total concentration of the acid \(C_T\), the hydrogen ion concentration \([H^+]\), and the acid dissociation constant \(K_a\).
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What are the algebraic steps to isolate [H+] so I can solve for it with given variables?
![The image shows a chemical equation related to acid-base chemistry. The formula is expressed as:
\[ C_T = [H^+] \left( 1 + \frac{[H^+]}{K_a} \right) \]
Below the equation, two values are provided:
- \( C_T = 9.5 \times 10^{-5} \)
- \( K_a = 10^{-7.6} \)
The unknown in the equation is:
\[ [H^+] = ? \]
This equation is used to find the concentration of hydrogen ions \([H^+]\) in a solution. It relates the total concentration of the acid \(C_T\), the hydrogen ion concentration \([H^+]\), and the acid dissociation constant \(K_a\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F91195c14-8c67-42a0-b9d0-a3e8c2a59df0%2F43f728b5-382a-4609-b877-18e93ee60e7a%2Fy2wqvhn_processed.png&w=3840&q=75)
Given that, and
To find the value of , substitute the given values in .
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