Phenylacetic acid (C6H₂CH₂CO₂H) is a weak monoprotic acid with K₂ = 4.90 x 10-5. What is the pH of a 9.21 x 10-¹ M solution of potassium phenylacetate (CH₂CH₂CO₂K* )?
Phenylacetic acid (C6H₂CH₂CO₂H) is a weak monoprotic acid with K₂ = 4.90 x 10-5. What is the pH of a 9.21 x 10-¹ M solution of potassium phenylacetate (CH₂CH₂CO₂K* )?
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![**Topic: Calculating the pH of a Weak Acid Solution**
Phenylacetic acid (\(C_6H_5CH_2CO_2H\)) is a weak monoprotic acid with an acid dissociation constant (\(K_a\)) of \(4.90 \times 10^{-5}\). The task is to determine the pH of a \(9.21 \times 10^{-1} \, M\) solution of potassium phenylacetate (\(C_6H_5CH_2CO_2^− K^+\)).
**Context:**
When salts like potassium phenylacetate are dissolved in water, they dissociate into ions. In this case, the phenylacetate ion (\(C_6H_5CH_2CO_2^−\)) acts as a conjugate base and can accept a proton (\(H^+\)) from water, forming phenylacetic acid and a hydroxide ion (\(OH^−\)). This results in a basic solution.
The pH of such a solution can be calculated by considering the hydrolysis reaction and using the relationship between \(K_a\) and \(K_b\) (the base dissociation constant), given by:
\[ K_w = K_a \times K_b \]
where \(K_w\) is the ion-product constant of water (\(1.0 \times 10^{-14}\)). By calculating \(K_b\), we can determine the \(OH^−\) concentration and subsequently the pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3425cae7-78b6-4102-b4ec-611d4b67bd59%2Fed9b7cf6-f667-4078-95f7-6692d79862d1%2F25poc33_processed.png&w=3840&q=75)
Transcribed Image Text:**Topic: Calculating the pH of a Weak Acid Solution**
Phenylacetic acid (\(C_6H_5CH_2CO_2H\)) is a weak monoprotic acid with an acid dissociation constant (\(K_a\)) of \(4.90 \times 10^{-5}\). The task is to determine the pH of a \(9.21 \times 10^{-1} \, M\) solution of potassium phenylacetate (\(C_6H_5CH_2CO_2^− K^+\)).
**Context:**
When salts like potassium phenylacetate are dissolved in water, they dissociate into ions. In this case, the phenylacetate ion (\(C_6H_5CH_2CO_2^−\)) acts as a conjugate base and can accept a proton (\(H^+\)) from water, forming phenylacetic acid and a hydroxide ion (\(OH^−\)). This results in a basic solution.
The pH of such a solution can be calculated by considering the hydrolysis reaction and using the relationship between \(K_a\) and \(K_b\) (the base dissociation constant), given by:
\[ K_w = K_a \times K_b \]
where \(K_w\) is the ion-product constant of water (\(1.0 \times 10^{-14}\)). By calculating \(K_b\), we can determine the \(OH^−\) concentration and subsequently the pH.
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