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moles of H+ = 42.0 x 0.120 millimoles = 5.04 millimoles final volume = 1.55 L
[H+] = (5.04 x 10^-3)/1.55 = 3.25 x 10^-3M pH = -log[H+] = 2.49
Solution
moles of H+ = 42.0 x 0.120 millimoles = 5.04 millimoles final volume = 1.55 L
[H+] = (5.04 x 10^-3)/1.55 = 3.25 x 10^-3M pH = -log[H+] = 2.49

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moles of H+ = 42.0 x 0.120 millimoles = 5.04 mill.pdf

  • 1. moles of H+ = 42.0 x 0.120 millimoles = 5.04 millimoles final volume = 1.55 L [H+] = (5.04 x 10^-3)/1.55 = 3.25 x 10^-3M pH = -log[H+] = 2.49 Solution moles of H+ = 42.0 x 0.120 millimoles = 5.04 millimoles final volume = 1.55 L [H+] = (5.04 x 10^-3)/1.55 = 3.25 x 10^-3M pH = -log[H+] = 2.49