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A solution of naoh has a concentration of 5.51 x 10-3 m. what is the ph of this solution? ph = 2.26 ph = 5.51 ph = 11.74 ph = 3.00

Respuesta :

pH = 11.74. Because NaOH dissociates completely in water, [OH-] = [NaOH].
pOH = -log[OH-] = -log(5.51x10-3) = 2.26
pH = 14 - pOH = 14 - 2.26 = 11.74
Baraq

Answer:

ph = 11.74

Explanation:

Given the dissociation of NaOH in water is NaOH Imported Asset Na+ + OH-.

Hence, if the concentration of NaOH is 5.51 x 10-3 M,

the concentration of OH- must also be 5.51 x 10-3 M,

Given that a mole to mole ratio of 1:1.

To find the pH of the solution, one will then use pOH = -log[OH-] and subtracting from 14, which is = pH+pOH = 14 for water at 298K

Hence, pOH = −log105.51×10−3

=2.26

Therefore, pH = 14−2.26 = 11.74