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The ph of an aqueous solution of 1.00 x 10-2 m HOCN is 2.77 at 25 0c. Calculate ka for HOCN.
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Sure, here is the calculation of Ka for HOCN:
The pH of an aqueous solution of 1.00 x 10-2 M HOCN is 2.77 at 25 0C. Calculate Ka for HOCN.
The pH of a solution is given by the following equation:
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in moles per liter.
We can use the pH to calculate the concentration of hydrogen ions:
[H+] = 10^-pH
[H+] = 10^-2.77 = 1.74 x 10^-3 M
The Ka for HOCN can be calculated using the following equation:
Ka = [H+][OCN-]/[HOCN]
We know that [H+] = 1.74 x 10^-3 M and that [HOCN] = 1.00 x 10^-2 M. We can solve for [OCN-] using the following equation:
[OCN-] = Ka[HOCN]/[H+]
[OCN-] = (1.74 x 10^-3 M)(1.00 x 10^-2 M)/(1.74 x 10^-3 M) = 1.00 x 10^-2 M
Now we can calculate Ka:
Ka = [H+][OCN-]/[HOCN]
Ka = (1.74 x 10^-3 M)(1.00 x 10^-2 M)/(1.00 x 10^-2 M) = 1.74 x 10^-3
Therefore, the Ka for HOCN is 1.74 x 10^-3.
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