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AnnyKZ [126]
3 years ago
6

Calculate the hydrogen-ion concentration (H+] for the aqueous solution in which [OH-1 is 1 x 10-12 mol/L.

Chemistry
2 answers:
Artemon [7]3 years ago
7 0

Answer:If we have [H+][OH-]= Kw = 1.0 x 10^-14

Then [H+]= Kw/ [OH-]= 1.0x 10^-14/ 1 x 10^-11 =1 x 10^-3 mol/L

And here is the solution - as you can see it is an acidic one :

pH = - log [H+]= - log 1 x 10^-3 = 3 < 7

Explanation:

Vlad1618 [11]3 years ago
5 0

Answer:

[H+] = 0.01mol/L

Explanation:

p[OH] = -log[OH-]

[OH-] = 1*10^-12

pOH = -Log[1*10^-12]

pOH = 12.

But pH + pOH = 14

pH = 14 - pOH

pH = 14 - 12

pH = 2

pH = -Log[H+]

2 = -Log[H+]

Take the anti log of both sides

10⁻² = [H+]

[H+] = 0.01

The hydrogen ion concentration is 0.01mol/L

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

Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide:

2MnCO_3(s)+O_2(g)\rightarrow 2MnO_2(s)+2CO_2(g)

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Explanation :

The given two chemical reactions are:

(1) 2MnCO_3(s)+O_2(g)\rightarrow 2MnO_2(s)+2CO_2(g)

(2) 3MnO_2(s)+4Al(s)\rightarrow 3Mn(s)+2Al_2O_3(s)

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(1)

(2) 6MnO_2(s)+8Al(s)\rightarrow 6Mn(s)+4Al_2O_3(s)

Now we are adding both the reactions, we get the overall chemical reaction.

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The  MnO_2 is common on both side, by cancelling it, we get:

The net chemical equation for the production of manganese is:

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