a solution that is 0.170 M in HC2H3O2 and 0.110 M in KC2H3O2
what is the pH?
a solution that is 0.250 M in CH3NH2 and 0.135 M in CH3NH3Br
what is the pH?
1)
Ka of HC2H3O2= 1.8*10^-5
pKa = - log (Ka)
= - log(1.8*10^-5)
= 4.745
use:
pH = pKa + log {[conjugate base]/[acid]}
= 4.745+ log {0.11/0.17}
= 4.556
Answer: 4.56
2)
Kb of CH3NH2 = 4.47*10^-4
Kb = 4.47*10^-4
pKb = - log (Kb)
= - log(4.47*10^-4)
= 3.35
use:
pOH = pKb + log {[conjugate acid]/[base]}
= 3.35+ log {0.135/0.25}
= 3.082
use:
PH = 14 - pOH
= 14 - 3.0821
= 10.9179
Answer: 10.92
a solution that is 0.170 M in HC2H3O2 and 0.110 M in KC2H3O2 what is the...
Solve for pH using henderson hasselbach equation a. a solution that is 0.195 M in HC2H3O2 and 0.110 M in KC2H3O2 b. a solution that is 0.255 M in CH3NH2 and 0.130 M in CH3NH3Br express using two decimal places
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Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that is 0.195 M in HC2H3O2 and 0.115 M in KC2H3O2 Express your answer using two decimal places. a solution that is 0.220 M in CH3NH2 and 0.110 M in CH3NH3Br Express your answer using two decimal places.
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