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How would you Calculate the H3O ion concentration in a solution with pH3 and a solution with pH8?

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In a solution, hydrogen ions normally bond with molecules of water, forming H3O+ (hydronium) ions. Thus, the concentration of the hydronium ions will be the same as the concentration of hydrogen ions, which is related to the pH of a solution according to the following equation:

pH = -log[H+] = -log[H3O+]

This equation can be solved for the concentration of hydronium ions:

[H3O+] = 10-pH

Thus, for a solution with a pH of 3, the concentration of hydronium ions will be 10-3 = 0.001 moles/liter, and for a solution with a pH of 8, the concentration of hydronium ions will be 10-8 = 0.00000001 moles/liter.
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What is the pH of an aqueous solution with the hydronium ion concentration H3O 2 x 10-14 M?

To find the pH use this: -log(2 X 10^-14 M) = 13. 7 pH ( you could call it 14 )
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What would its new pH be if the concentration of H3O plus ions in the solution were increased by 100 times and why?

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How much more solution is pH10 than pH8?

At pH = 10 there is 1*10-4 mol/L OH- At pH = 8 there is 1*10-6 mol/L OH- So at pH10 it is 100 times more OH- in this alkaline solution (and 100 times less H+)
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