Which one of the following Weak Base Kb C5H5N 1.7 x 10-9 HONH2 1.1 x 10-8 C6HSNH2 4.3 x 10-10 H2NNH2 1.3 x 10-6

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**Question:**
Which one of the following 1.0 M solutions would have the lowest pH?

**Table of Weak Bases and their \(K_b\) Values:**

| Weak Base | \(K_b\)     |
|-----------|-------------|
| \( \text{C}_5\text{H}_5\text{N} \) | \( 1.7 \times 10^{-9} \) |
| \( \text{HONH}_2 \)      | \( 1.1 \times 10^{-8} \) |
| \( \text{C}_6\text{H}_5\text{NH}_2 \) | \( 4.3 \times 10^{-10} \) |
| \( \text{H}_2\text{NNH}_2 \)  | \( 1.3 \times 10^{-6} \) |

**Options:**
A) \( \text{C}_5\text{H}_5\text{N} \)

B) \( \text{HONH}_2 \)

C) \( \text{C}_6\text{H}_5\text{NH}_2 \)

D) \( \text{H}_2\text{NNH}_2 \)

**Explanation:**

To determine which solution would have the lowest pH, analyze the \(K_b\) values. A lower \(K_b\) indicates a weaker base, leading to a stronger conjugate acid and a lower pH. Among the given bases:

- \( \text{C}_6\text{H}_5\text{NH}_2 \) with \( 4.3 \times 10^{-10} \) has the weakest \(K_b\), suggesting the lowest pH for its solution.
Transcribed Image Text:**Question:** Which one of the following 1.0 M solutions would have the lowest pH? **Table of Weak Bases and their \(K_b\) Values:** | Weak Base | \(K_b\) | |-----------|-------------| | \( \text{C}_5\text{H}_5\text{N} \) | \( 1.7 \times 10^{-9} \) | | \( \text{HONH}_2 \) | \( 1.1 \times 10^{-8} \) | | \( \text{C}_6\text{H}_5\text{NH}_2 \) | \( 4.3 \times 10^{-10} \) | | \( \text{H}_2\text{NNH}_2 \) | \( 1.3 \times 10^{-6} \) | **Options:** A) \( \text{C}_5\text{H}_5\text{N} \) B) \( \text{HONH}_2 \) C) \( \text{C}_6\text{H}_5\text{NH}_2 \) D) \( \text{H}_2\text{NNH}_2 \) **Explanation:** To determine which solution would have the lowest pH, analyze the \(K_b\) values. A lower \(K_b\) indicates a weaker base, leading to a stronger conjugate acid and a lower pH. Among the given bases: - \( \text{C}_6\text{H}_5\text{NH}_2 \) with \( 4.3 \times 10^{-10} \) has the weakest \(K_b\), suggesting the lowest pH for its solution.
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