Calculate the pH of a 0.0350M
2 answers:
Answer:
pH = 12.544
Explanation:
0.0350M 0.0350M 0.0350M.........equilibrium
∴ pOH = - log [OH-]
∴ pH + pOH = 14
⇒ [OH-] = 0.0350 M
⇒ pOH = - Log (0.0350)
⇒ pOH = 1.456
⇒ pH = 14 - 1.456
⇒ pH = 12.544
Answer:
12.54
Explanation:
The dissociation equation of NaOH is given below:
NaOH <==> Na+ + OH-
Molarity of NaOH = 0.0350M
From the equation,
Since 1M of NaOH produced 1M of OH-, then, 0.035M of NaOH will also produce 0.035M of OH-..
From the above,
[OH-] = 0.035M
Now, we can solve the pH by doing the following:
pOH = — log [OH-]
pOH = — log 0.035
pOH = 1.46
Recall
pH + pOH = 14
pH = 14 — pOH
pH = 14 — 1.46
pH = 12.54
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