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Allisa [31]
4 years ago
12

At 100°C, the Kw of water is 5.6x10−13. What is the pOH of a solution that has a pH of 6.25 at 100°C? A) 6.00 B) 6.25 C) 7.00 D)

7.75 E) 8.00
Chemistry
2 answers:
Alex_Xolod [135]4 years ago
8 0

Answer:

The pOH of a solution that has a pH of 6.25 at 100°C is 7.75 (option D)

Explanation:

pOH + pH = 14

pOH = 14 - 6.25

pOH = 7.75

Therefore, at 100°C, the Kw of water is 5.6x10⁻¹³ and the pOH of a solution that has a pH of 6.25 at 100°C is 7.75.

Thus, option D, is the correct answer.

taurus [48]4 years ago
6 0

Answer:

D. 7.75.

Explanation:

Equation for the dissociation of water:

H2O(aq) --> H+(aq) + OH-(aq)

[H+][OH-] = Kw

The constant, Kw, is the ionic product of water. The product of concentrations of H+ and OH- ions in water at a particular temperature is known as ionic product of water.

Kw = 5.6x10−13

Since,

pH + pOH = 14

pH = 6.25

6.25 + pOH = 14

Therefore,

pOH = 14 - 6.25

= 7.75.

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