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Acids and Bases: Base equations

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Wize University Chemistry Textbook > Acids and Bases

Base Equations (Kb, pKb)

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CH3NH3 is a weak base. When mixed with water, we see the following reaction:

CH3NH3 + H2O <----> CH3NH4+ + OH-

Once the reaction reaches equilibrium, Kb was found to be 1.07 x 10-3. If the reaction at equilibrium contains 2.5 M CH3NH3 and 0.37 M CH3NH4+, how much OH- is in solution?


More Base Equations (Kb, pKb) Questions:
Consider the following reaction in water:
NaOH <----> Na+ + OH-
This reaction has a Kb of 1 x 10-10 and a pOH of 3. If there is 1 M of NaOH at equilibrium, what is the concentration of Na+ in solution?
An aqueous solution only contains a 0.050 M in a weak base. Which of the following statements would be true about the solution?
Consider the weak bases below and their Kb values:
C6H7OKb=1.3×10−10C_6H_7O \hspace{48pt}K_b=1.3 \times 10^{-10}
C2H5NH2Kb=5.6×10−4C_2H_5NH_2 \hspace{30pt}K_b=5.6 \times 10^{-4}
Ammonia(NH3) is a weak base, Kb = 1.8 x 10-5 and benzoic acid (C6H5CH2O-) is a weak acid, Ka = 6.3 x 10-5. A solution of ammonium benzoate (NH4)(C6H5CH2O-) is:
To 150 mL of water was added 0.18 moles of ammonia (NH3 Kb= 2.3 x 10-5) calculate the pH.
Triemethylamine (N(CH3)3) is a base (pKb=4.19) used in a variety of organic reactions. It can also be used as an effective Lewis base due to it's small steric profile.
if a solution of [N(CH3)3H]2[SO4]is dissolved in neutral water the pH will be,
Strength of Acids and Bases
What is the strongest acid below? What is the weakest acid?
Strongest acid:
Cl3CCOOH
Weakest acid:
HCN
Acids and Bases: Base Equations
Consider the weak bases below and their Kb values:
C6H7OKb=1.3×10−10C2H5NH2Kb=5.6×10−4C5H5NKb=1.7×10−9\begin{alignedat}{} &C_6H_7O &&K_b = 1.3\times10^{-10}\\ &C_2H_5NH_2 &&K_b = 5.6\times10^{-4}\\ &C_5H_5N &&K_b = 1.7\times10^{-9} \end{alignedat}
Arrange the conjugate acids of these weak bases in order of increasing acid strength.