The concentration of hydroxide ions in the antacid, milk of magnesia, is 5.2x10^-4 M. Calculate the concentration of hydronium ions at 25 degrees celcius.
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To calculate the concentration of hydronium ions (H3O+) in a solution, you can use the formula for the ion product of water (Kw) at 25 degrees Celsius:
Kw = [H3O+][OH-]
The Kw value at 25 degrees Celsius is 1.0 x 10^-14. Since the solution in question is basic (due to the presence of hydroxide ions), we can assume that [H3O+] is low and [OH-] is roughly equal to the concentration of hydroxide ions.
Given that the concentration of hydroxide ions ([OH-]) is 5.2 x 10^-4 M, we can substitute this value into the Kw equation:
1.0 x 10^-14 = [H3O+] x 5.2 x 10^-4
Rearranging the equation to solve for [H3O+], we get:
[H3O+] = (1.0 x 10^-14) / (5.2 x 10^-4)
[H3O+] = 1.92 x 10^-11 M
Therefore, the concentration of hydronium ions ([H3O+]) in the solution, milk of magnesia, at 25 degrees Celsius is approximately 1.92 x 10^-11 M.
To calculate the concentration of hydronium ions (H3O+) in a solution, we need to use the concept of pH and pOH.
In water, the product of the concentration of hydronium ions (H3O+) and hydroxide ions (OH-) is always equal to 1 x 10^-14 at 25 degrees Celsius. This can be represented as:
[H3O+][OH-] = 1 x 10^-14
We can rearrange this equation to solve for hydronium ion concentration:
[H3O+] = (1 x 10^-14) / [OH-]
Given that the concentration of hydroxide ions ([OH-]) in milk of magnesia is 5.2 x 10^-4 M, we can substitute this value into the equation:
[H3O+] = (1 x 10^-14) / (5.2 x 10^-4)
Calculating this expression:
[H3O+] = 1.92 x 10^-11 M
Therefore, the concentration of hydronium ions in milk of magnesia at 25 degrees Celsius is approximately 1.92 x 10^-11 M.