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Which has minimam pkb
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A 1.0 M solution of an unknown weak base has a pH of 12.3 at 25 oC.
What is the identity of the base? a. Ammonia, pKb = 4.8 b.
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i think its c
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the pKb for methylamine is 3.36, what is the Kb for methylamine?
pKa+pKb= 14.00 Kb= 10^-pKb = 4.4x10^-4 is the answer but HOW??
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pKb = 3.36 pKb = -log Kb 3.36 = -logKb -3.36 = log Kb Punch in 3.36 and hit the change sign button
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To explain why aniline (pKb 9.37) is a weaker base than cyclohexanamine (pKb 3.34) using resonance
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a. a 0.1 M solution of an acid with
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To determine the solution with the lowest pH (more acidic), we need to compare the acid dissociation
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The pKb of pyridine is 8.75. What is the pH of a 0.480M solution of pyridine?
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B) What is the pH of a 0.243mol
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A. ...........HCN ==> H^+ + CN^- I.......0.0098.....0......0 C.........-x........x.....x
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Determine the pH (to two decimal places) of a solution prepared by adding 15.9 mL of 0.0551 M sodium hydrogen oxalate
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mmoles acid = 15.9 x 0.0551 = ? mmoles base = 0.488/molar mass Na2C2O4) pH = pKa2 + log(base)/(acid)
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The pKb of ammonia, NH3, is 4.74 at 25°C. Which of the following is the Ka of the ammonium ion, NH4+?
not sure what to do,
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The easy way. pKa + pKb = pKw = 14 You have pKa of 9.26 which is right but you took the -log of 4.26
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A weak base has pKb = 9.25..
A. Calculate the % ionization at pH = 8.25 B. Calculate the % ionization at pH = 10.25 C. What is
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To calculate the ionization of a weak base, you can use the equilibrium constant expression for the
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Determine the pkb of methylamine if the kb is 4.4*10^-4.
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To find the pKb of methylamine, we first need to calculate the Kb (equilibrium constant for the base
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