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a 0.00959 M solution of a weak base has a pH of 9.33. What is the Ka for its conjugate acid?

Question

a 0.00959 M solution of a weak base has a pH of 9.33. What is the Ka for its conjugate acid?

check_circleAnswer
Step 1

Concentration of OH- is calculated as follows,

PH + pОН %3D 14
РОН %3 14-рH %3D14-9.33 %34.67
pOH logOH
4.67
2.14x10
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PH + pОН %3D 14 РОН %3 14-рH %3D14-9.33 %34.67 pOH logOH 4.67 2.14x10

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Step 2

Value of Kb can be determined by plotting ICE table. The base is t...

В -
ВH"
Н.О
-НО
Initial
0.225
0.00959
0
+2.14x10
- 2.14 x10
+2.14x10
Change
9.57 х10-3
2.14x10
2.14x10
Equilibrium
[вн |он ]
Кь
(214x10°)(214х10°)
4.78x10
[в]
9.57 x 10
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В - ВH" Н.О -НО Initial 0.225 0.00959 0 +2.14x10 - 2.14 x10 +2.14x10 Change 9.57 х10-3 2.14x10 2.14x10 Equilibrium [вн |он ] Кь (214x10°)(214х10°) 4.78x10 [в] 9.57 x 10

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