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3 years ago

Show that the pH of a solution is -0.301 when its hydronium ion concentration equals 2 moles/L. Is the solution acidic or basic?

Chemistry

1 answer:

vaieri [72.5K]3 years ago

8 0

Answer:

The answer to your question is below

Explanation:

Data

Demonstrate pH = -0.301

concentration = 2 moles/L

Formula

pH = -log [H⁺]

Process

1.- Calculate the [H⁺] concentration

[H⁺] = 2 moles/L = 2 M2.- Substitute in the formula

pH = -log[2]

simplification

pH = -0.301

2.- Conclusion

It is an acidic solution

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This is an incomplete question, here is a complete question.

Determine whether each of the following electron configurations is an inert gas, a halogen, an alkali metal, an alkaline earth metal, or a transition metal. Justify your choices.

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(b) $1s^22s^22p^63s^23p^63d^74s^2$ → Transition metal

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Halogen : These are the elements which lie in group 17.

Their general electronic configuration is: $ns^2np^5$ where n is the outermost shell.

An alkali metal : These are the elements which lie in group 1.

Their general electronic configuration is: $ns^1$ where n is the outermost shell.

An alkaline earth metal : These are the elements which lie in group 2.

Their general electronic configuration is: $ns^2$ where n is the outermost shell.

Transition elements : They are the elements which lie between 's' and 'p' block elements. These are the elements which lie in group 3 to 12. The valence electrons of these elements enter d-orbital.

Their general electronic configuration is: $(n-1)d^{1-10}ns^{0-2}$ where n is the outermost shell.

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The element having this electronic configuration belongs to the transition family.

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The element having this electronic configuration belongs to the transition family.

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