cava chem 303 s2d30 3.04 Measuring Acids and Bases
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| show | In an aqueous solution, the product of the concentration of hydrogen ions and the concentration of hydroxide ions is always equal to 1.0 × 10^(-14) M.
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| the concentrations of H+ ions and OH- ions are each is 1 × 10^([...]) M in a neutral solution. | show 🗑
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| If the concentration of H+ is then [...] than 1 × 10^(-7) M, the solution is acidic. | show 🗑
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| If the concentration of H+ is then [...] than 1 × 10^(-7) M, the solution is basic. | show 🗑
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| another word for 'basic' (as opposed to acidic) is '[...]'. | show 🗑
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| The pH of a solution is based on a measurement of the concentration of [...] ions. | show 🗑
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| show | pH is the negative log of the concentration of hydrogen ions, [H+].
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| show | Square brackets around something in chemistry mean 'the concentration of whatever is in the square brackets'.
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| [H+] is the way we write the *[...]* of hydrogen ions H+. | show 🗑
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| show | pH = –log[H+]
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| Neutral solutions have a pH of [...]. | show 🗑
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| show | In "PEE-EYTCH", the letter P is lower-case and the H is upper-case.
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| show | Acidic solutions have a pH lower than 7
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| Basic solutions have a pH [...] than 7 | show 🗑
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