What is the pH of a 6.50 x 10-3 M OH solution?Formulas(OH]=1x10[H*] = 10-PHH*OH[OH-] = 10-POH(H]=1x 104JOH]pH = – log,[H*]pOH = - log,[OH-]के10pOH 14- pHpH + pOH = 14pHРОН%3DpH 14-pOHO 2.1911.819.794.21LHOR- HodLHBo-- Hd

The concentration of OH− ion, [OH−] = 6.50×10−3 M

What is the pH of a 6.50 x 10-3 M OH solution? Formulas (OH)=1x10 [H*] = 10-PH [OH-] = 10-POH H* %3D OH (H]=1x 104 [OH] pH = - log,o[H*] pOH = – log,[OH-] POH 14-pH pH + pОН %3D 14 pH РОН pH 14-pOH O 2.19 O 11.81 9.79 O 4.21 LHO - HOd LHSo- - Hd

What is the pH of a 6.50 x 10-3 M OH solution? Formulas (OH)=1x10 [H] = 10-PH [OH-] = 10-POH H %3D OH (H]=1x 104 [OH] pH = - log,o[H*] pOH = – log,[OH-] POH 14-pH pH + pОН %3D 14 pH РОН pH 14-pOH O 2.19 O 11.81 9.79 O 4.21 LHO - HOd LHSo- - Hd

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

What is the pH of a 6.50 x 10-3 M OH solution?
Formulas
(OH]=1x10
[H*] = 10-PH
H*
OH
[OH-] = 10-POH
(H]=1x 104
JOH]
pH = – log,[H*]
pOH = - log,[OH-]
के
10
pOH 14- pH
pH + pOH = 14
pH
РОН
%3D
pH 14-pOH
O 2.19
11.81
9.79
4.21
LHOR- Hod
LHBo-- Hd

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