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What is the pH of a solution with a concentration of 2.4 × 10-5 molar H3O+? Show, or explain, the work used to solve this problem.

Sagot :

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[tex]pH=-log|H_{3}O^{+}|\\\\ pH=-log2.4*10^{-5}=-(log2.4+log10^{-5})=-(0,38-5)=-(-4.62)\\\\ pH=4.62[/tex]

Answer:

The pH of the solution is 4.61.

Explanation:

The pH of the solution is defined as negative logarithm of [tex]H_3O^+[/tex] ion concentration.

[tex]pH=-\log[H_3O^+][/tex]

The concentration of [tex]H_3O^+=2.4\times 10^{-5} molar[/tex]

[tex]pH=-\log[2.4\times 10^{-5} M]=4.61[/tex]

The pH of the solution is 4.61.

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