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A chemist makes a solution of [tex][tex]$NaOH$[/tex][/tex] for use in an experiment. She dissolves [tex][tex]$0.00500 \, \text{mol NaOH}$[/tex][/tex] in 1.00 [tex][tex]$L H_2O$[/tex][/tex]. The [tex][tex]$NaOH$[/tex][/tex] completely dissociates to form a solution with [tex]\left[ OH^{-} \right] = 0.00500 \, M[/tex].

What is the [tex]pOH[/tex] of this solution?

A. 0.00500
B. 5.00
C. 2.30
D. [tex]-2.30[/tex]

Sagot :

GinnyAnswer
To determine the pOH of the solution given that the concentration of hydroxide ions, [tex]\([OH^-]\)[/tex], is 0.00500 M, we can follow these steps:

1. Identify the formula for pOH:
[tex]\[ \text{pOH} = -\log_{10}[\text{OH}^-] \][/tex]

2. Insert the concentration of [tex]\([\text{OH}^-]\)[/tex]:
[tex]\[ [\text{OH}^-] = 0.00500\text{ M} \][/tex]

3. Calculate the pOH:
[tex]\[ \text{pOH} = -\log_{10}(0.00500) \][/tex]

Performing the logarithmic calculation:

[tex]\[ \text{pOH} = -\log_{10}(0.00500) \approx 2.30 \][/tex]

Thus, the pOH of the solution is approximately 2.30.

Therefore, the correct answer is:

[tex]\[ \boxed{2.30} \][/tex]
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