A solution has a hydronium ion concentration, [tex][H_3O^+][/tex], of [tex]4.9 \times 10^{-2} \, \text{M}[/tex]. What is the [tex]\text{pH}[/tex] of the solution?

A) 1.69
B) 1.69 x [tex]10^2[/tex]
C) 1.51
D) 1.51 x [tex]10^2[/tex]

The pH is calculated by applying the negative logarithm to the hydronium ion concentration, in this case, resulting in a pH of 1.31 which is not one of the provided options.

Explanation:

The subject question revolves around determining pH from the hydronium ion concentration, [H3O+]. The relationship between pH and [H3O+] is defined by the pH scale equation: pH = -log [H3O+] Using the given hydronium ion concentration of 4.9×10−2M, we conduct the operation: pH = -log (4.9 × 10−2). When we execute this calculation, we get a pH of 1.31. However, this option is not available in the provided answers. Ensure there is not a mistake in the question or computation.

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A solution has a hydronium ion concentration, [tex][H_3O^+][/tex], of [tex]4.9 \times 10^{-2} \, \text{M}[/tex]. What is the [tex]\text{pH}[/tex] of the solution?A) 1.69 B) 1.69 x [tex]10^2[/tex] C) 1.51 D) 1.51 x [tex]10^2[/tex]

Answer :

Final answer:

Explanation:

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Other Questions

A solution has a hydronium ion concentration, [tex][H_3O^+][/tex], of [tex]4.9 \times 10^{-2} \, \text{M}[/tex]. What is the [tex]\text{pH}[/tex] of the solution?

A) 1.69
B) 1.69 x [tex]10^2[/tex]
C) 1.51
D) 1.51 x [tex]10^2[/tex]