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Power of hydrogen
pH=−log10[H+]\text{pH} = -\log_{10}[\text{H}^+]pH=−log10[H+]
pOH=−log10[OH−]\text{pOH} = -\log_{10}[\text{OH}^-]pOH=−log10[OH−]
pH+pOH=14\text{pH} + \text{pOH} = 14pH+pOH=14
Completely dissociate (break apart)
Molarity × number of H+\text{H}^+H+ ions released
2 H+\text{H}^+H+ ions per molecule
Calculate pOH first, then use pH=14−pOH\text{pH} = 14 - \text{pOH}pH=14−pOH
Increases by 1 unit
Only partially dissociate
How much the acid dissociates
[H+]=Ka×Macid[\text{H}^+] = \sqrt{K_a \times M_{\text{acid}}}[H+]=Ka×Macid
Weak acids have higher pH values
Strong acids: high; weak acids: lower
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