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June 6, 2021 - Answer (1 of 3): 1. Given that pH = 3.17 2. Know that pH = -log{H+} = 3.17 3. {H+} = 10^-3.17 = 6.76x10^-4M 4. And pOH = 14 - pH = 14–3.17 = 10.83 5. Then pOH = -log{OH-} = 10.83 6. {OH-} = 10^-10.83 = 1.47x10^-11 M 7. To check: {H+} x {OH-} = 10^-14 8. 6.76x10^-4M x 1.47x10^-11M = 1.0x10^-14 ...

The pH of a solution is equal to: · Water can be considered an acid because of its ability to ionize to a proton and a negatively charged hydroxide ion: H-O-H H + + OH -

September 10, 2019 - Distinguishing between the different forms of Hydrogen can be confusing to those of us who flunked high school chemistry. This article is an attempt to clarify the differences between H, H2, H+, H- and OH-.

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Data from this table are plotted in the figure below over a narrow range of concentrations between 1 x 10-7 M and 1 x 10-6 M. The point at which the concentrations of the H3O+ and OH- ions are equal is called the neutral point. Solutions in which the concentration of the H3O+ ion is larger ...

December 3, 2021 - Register Alias and Password (Only available to students enrolled in Dr. Lavelle’s classes.) ... Hi, how do I calculate the OH- concentration given the H+ concentration as in question 5 in the Achieve homework?

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Balance any equation or reaction using this chemical equation balancer! Find out what type of reaction occured.