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Zigmanuir [339]
3 years ago
15

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 proble

m.
Chemistry
2 answers:
MrRissso [65]3 years ago
7 0
pH=-log|H_{3}O^{+}|\\\\
pH=-log2.4*10^{-5}=-(log2.4+log10^{-5})=-(0,38-5)=-(-4.62)\\\\
pH=4.62
Rina8888 [55]3 years ago
4 0

Answer:

The pH of the solution is 4.61.

Explanation:

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

pH=-\log[H_3O^+]

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

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

The pH of the solution is 4.61.

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A solid mixture consists of 47.6g of KNO3 (potassium nitrate) and 8.4g of K2SO4 (potassium sulfate). The mixture is added to 130
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<u>Answer:</u> No crystals of potassium sulfate will be seen at 0°C for the given amount.

<u>Explanation:</u>

We are given:

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This means that, all of potassium sulfate will be dissolved.

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