Answer:
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Answer:
Are basic:
[OH⁻] = 3.13x10⁻⁷M and [H₃O⁺] = 9.55x10⁻⁹M
Explanation:
A solution is basic when pH = - log [H₃O⁺] is higher than 7.
It is possible to convert [OH⁻] to [H₃O⁺] using:
[H₃O⁺] = 1x10⁻¹⁴ / [OH⁻]
a. [OH⁻] = 3.13x10⁻⁷M
[H₃O⁺] = 1x10⁻¹⁴ / [3.13x10⁻⁷M]
[H₃O⁺] = 3.19x10⁻⁸M
pH = - log [H₃O⁺] = 7.50
[OH⁻] = 3.13x10⁻⁷M is basic
b. pH = -log [H₃O⁺] = - log 0.000747M = 3.13.
This solution is not basic
c. [H₃O⁺] = 9.55x10⁻⁹M
pH = 8.02
This solution is also basic.
First by getting moles of salicylic acid:
moles of salicylic acid = molarity * volume
= 0.02 * 0.05 L
= 0.001 mol
then moles of base KOH = molarity * volume
= 0.02 * 0.055L
= 0.0011
when total volume = 0.05 + 0.055 = 0.105 L
[salisalic acid] = moles / total volume
= 0.001 / 0.105
= 0.0095
[KOH] = moles / total volume
= 0.0011 / 0.105
= 0.01
by using H-H equation, we can get the PH:
PH = Pka + ㏒[salt/acid]
by substitution:
PH = 2.97 + ㏒[0.01 / 0.0095]
= 2.99
The answer is c hopefully I helped you