Choose from the given list of aqueous solutions

Choose from the given list of aqueous solutions (A-D): Which solution is the most basic? Which solution has the lowest pH? Which solution is the least basic? Which solution is the least acidic? pH ~log[H3O+] [H2O+]x[OH-] = 10^-14 Solution A has [H2O+] = 4.410^-10 M Solution B has [H3O+] = 9.310^-10 M Solution C has [OH-] = 2.310^-6 M Solution D has [OH-] = 4.910^-6 M

The Correct Answer and Explanation is:

To determine which solution is the most basic, the least acidic, the least basic, and the lowest in pH, let’s go step by step and analyze each solution. Given that the concentration of either [H3O+][H_3O^+][H3​O+] (hydronium ions) or [OH−][OH^-][OH−] (hydroxide ions) is provided for each solution, we can use the relationship between pH, pOH, and the ion product of water: [H3O+][OH−]=10−14 (at 25°C)[H_3O^+][OH^-] = 10^{-14} \, \text{(at 25°C)}[H3​O+][OH−]=10−14(at 25°C)

1. Solution A:
   • [H3O+]=4.4×10−10 M[H_3O^+] = 4.4 \times 10^{-10} \, \text{M}[H3​O+]=4.4×10−10M
   • Using [H3O+][H_3O^+][H3​O+], we can find the pH: pH=−log⁡(4.4×10−10)≈9.36\text{pH} = -\log(4.4 \times 10^{-10}) \approx 9.36pH=−log(4.4×10−10)≈9.36 This indicates a basic solution.
2. Solution B:
   • [H3O+]=9.3×10−10 M[H_3O^+] = 9.3 \times 10^{-10} \, \text{M}[H3​O+]=9.3×10−10M
   • Similarly, for pH: pH=−log⁡(9.3×10−10)≈9.03\text{pH} = -\log(9.3 \times 10^{-10}) \approx 9.03pH=−log(9.3×10−10)≈9.03 This is also a basic solution, but slightly more acidic than Solution A due to the higher [H3O+][H_3O^+][H3​O+].
3. Solution C:
   • [OH−]=2.3×10−6 M[OH^-] = 2.3 \times 10^{-6} \, \text{M}[OH−]=2.3×10−6M
   • We can use the relationship [H3O+]=10−14[OH−][H_3O^+] = \frac{10^{-14}}{[OH^-]}[H3​O+]=[OH−]10−14​ to find the hydronium concentration: [H3O+]=10−142.3×10−6≈4.35×10−9 M[H_3O^+] = \frac{10^{-14}}{2.3 \times 10^{-6}} \approx 4.35 \times 10^{-9} \, \text{M}[H3​O+]=2.3×10−610−14​≈4.35×10−9M Now calculate the pH: pH=−log⁡(4.35×10−9)≈8.36\text{pH} = -\log(4.35 \times 10^{-9}) \approx 8.36pH=−log(4.35×10−9)≈8.36 This is also a basic solution, but more basic than A and B.
4. Solution D:
   • [OH−]=4.9×10−6 M[OH^-] = 4.9 \times 10^{-6} \, \text{M}[OH−]=4.9×10−6M
   • Using the same relationship as above: [H3O+]=10−144.9×10−6≈2.04×10−9 M[H_3O^+] = \frac{10^{-14}}{4.9 \times 10^{-6}} \approx 2.04 \times 10^{-9} \, \text{M}[H3​O+]=4.9×10−610−14​≈2.04×10−9M And the pH: pH=−log⁡(2.04×10−9)≈8.69\text{pH} = -\log(2.04 \times 10^{-9}) \approx 8.69pH=−log(2.04×10−9)≈8.69 This is the most basic solution among all of them.

Answers:

• Most Basic Solution: Solution D (pH ≈ 8.69)
• Lowest pH: Solution B (pH ≈ 9.03)
• Least Basic Solution: Solution B (pH ≈ 9.03)
• Least Acidic Solution: Solution A (pH ≈ 9.36)

Explanation:

• The lower the pH, the more acidic the solution, and the higher the pH, the more basic it is.
• Solutions A and B have the lowest pH values and are therefore the most acidic.
• Solutions C and D are basic, with Solution D being the most basic due to the highest concentration of hydroxide ions.