Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its Ka value.

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Chapter1: Chemical Foundations
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**Question:**

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its \( K_a \) value.

**Options:**

- ○ HCHO₂, \( 1.8 \times 10^{-4} \)
- ○ HF, \( 3.5 \times 10^{-4} \)
- ○ HCN, \( 4.9 \times 10^{-10} \)
- ○ HClO₂, \( 1.1 \times 10^{-2} \)
- ○ HNO₂, \( 4.6 \times 10^{-4} \) 

**Explanation:**
The solution with the highest pH will be the weakest acid, which has the smallest \( K_a \) value, indicating the least dissociation in water.
Transcribed Image Text:**Question:** Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its \( K_a \) value. **Options:** - ○ HCHO₂, \( 1.8 \times 10^{-4} \) - ○ HF, \( 3.5 \times 10^{-4} \) - ○ HCN, \( 4.9 \times 10^{-10} \) - ○ HClO₂, \( 1.1 \times 10^{-2} \) - ○ HNO₂, \( 4.6 \times 10^{-4} \) **Explanation:** The solution with the highest pH will be the weakest acid, which has the smallest \( K_a \) value, indicating the least dissociation in water.
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