LiOH is a strong base so we assume it dissociates.pdf
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The document discusses the complete dissociation of lithium hydroxide (LiOH) as a strong base, leading to an OH- concentration of 8.82 x 10^-3 M. It calculates the pOH as 2.05 and subsequently the pH as 11.95. Overall, the pH indicates the basic nature of the solution.
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![LiOH is a strong base so we assume it dissociates completely. So there will be 8.82
x 10^-3 M of OH- pOH = -log[OH-] = -log(8.82 x 10^-3) = 2.05 pH = 14 - pOH = 14 - 2.05 =
11.95
Solution
LiOH is a strong base so we assume it dissociates completely. So there will be 8.82
x 10^-3 M of OH- pOH = -log[OH-] = -log(8.82 x 10^-3) = 2.05 pH = 14 - pOH = 14 - 2.05 =
11.95](https://image.slidesharecdn.com/liohisastrongbasesoweassumeitdissociates-230408182257-0b58fce8/85/LiOH-is-a-strong-base-so-we-assume-it-dissociates-pdf-1-320.jpg)
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LiOH is a strong base so we assume it dissociates.pdf
- 1. LiOH is a strong base so we assume it dissociates completely. So there will be 8.82 x 10^-3 M of OH- pOH = -log[OH-] = -log(8.82 x 10^-3) = 2.05 pH = 14 - pOH = 14 - 2.05 = 11.95 Solution LiOH is a strong base so we assume it dissociates completely. So there will be 8.82 x 10^-3 M of OH- pOH = -log[OH-] = -log(8.82 x 10^-3) = 2.05 pH = 14 - pOH = 14 - 2.05 = 11.95