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zarasht:
The pH value of a particular weak acid is 6.79; calculate the hydrogen ion concentration for this acid.
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justjm:
The information is that the pH=6.79. I suggest you memorize the formulas below unless you have a reference sheet: \(-log[H_3O^+]=pH\) \(10^{-pH}=[H_3O^+]\) \(-log[OH^-]=pOH\) \(10^{-pOH}=[OH^-]\) \(K_w=[OH^-][H_3O^+]=1×10^{-14}\)...at 25°C \(pOH+pH=14\) at 25°C There are a few more equilibrium formulas and the H-H equation. Most of the formulas I listed above are derivable. If you remember formulas 1, 3, and 5, you can derive the rest if you know logarithm rules. Anways we can use this formula: \(10^{-pH}=[H_3O^+]\) pH=6.79 \(10^{-6.79}\) You can plug that into your calculator and figure it out
justjm:
btw H3O+ is the same as H+
zarasht:
thank you
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