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Strength of Acids and Bases

Related Topics

Wize University Chemistry Textbook > Acids and Bases

Base Equations (Kb, pKb)

1 Activity

Wize University Chemistry Textbook > Acids and Bases

Acid Equations (Ka, pKa)

3 Activities

What is the strongest acid below? What is the weakest acid?

Strongest acid:
Weakest acid:

Standard Ka values

What is the strongest base below? What is the weakest base?

Strongest base:
Weakest base:

Standard Kb values



More Base Equations (Kb, pKb) Questions:
Acids and Bases: Base equations
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?
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,
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.
More Acid Equations (Ka, pKa) Questions:
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What are the Ka and Kb of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
Methyl diethanolamine CH3N(C2H4OH)2 is a weak base which we will abbreviate as mdea. The conjugate acid, mdeaH+, has a pKa = 8.52.
Nitrous acid has a Ka of 7.1 x 10-5. What are [H3O+], [NO2- ] andin 0.50 M HNO2?
Acids and Bases: Weak Acid Practice
Nitrous acid has a Ka of 7.1 x 10-5. What are [H3O+] and [NO2- ] in 0.50 M HNO2?
Nitrous acid has a Ka of 7.1 x 10-5. What are [H3O+], [NO2- ] andin 0.50 M HNO2?
Acids and Bases: Ka
The following occurs when HCl is placed in water:
HCl <----> H+ + Cl-
The Ka for this reaction is known to be Ka = 5.64 once it reaches equilibrium. At equilibrium, 1.35 x 10-7 M of HCl and 1.2 M of Cl- can be found. What is the pH of the solution at equilibrium?
The following reaction occurs in water:
CH3OH <----> CH3O- + H+
Once the reaction was allowed to reach equilibrium, 0.5 M of CH3OH, 0.3 M of CH3O+, and 0.3 M of H+ were found in solution. What is the Ka of this solution?
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10-15. What is the concentration of H3O+ ions in pure water at this temperature?
What is the pH of a 1.1M solution of nitrous acid (HNO2). The Ka of nitrous acid is 7.2 x 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 4.00 L of water was added 100 mg of HF (6.6 x 10-4). What is the pH?
CH3COOH is a weak acid with a Ka of 1.8 x 10-5. In what pH range would you most likely an aqueous solution of Na(CH3COO).
Acids and Bases: Henderson Hasselbalch
To a solution of acetic acid (Ka=1.8×10−5\rm K_a = 1.8 \times 10^{-5}) was added 0.1 mol of NaOH\rm NaOH. After the addition of NaOH\rm NaOH the volume was 1.4L and the pH\rm pH was 5.2.
a) This solution a buffer? (True/False)
b) Calculate the number of moles of acetic acid that were originally in solution. Report your answer in moles to three significant figures. Do not include units in the answer field
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
A solution of [CH3NH3][CH3COO] is made in an undergraduate laboratory. Use the information below to predict the acidity of the solution.
CH3COOH: Ka = 1.8 x 10-5
CH3NH3+: Ka = 2.3 x 10-11
Acids and Bases: Conjugate
Using the data in the table, which of the conjugate bases below is the strongest base?
AcidKaHOAc1.8×10−5HCHO21.8×10−4HClO3.0×10−8HF6.8×10−4\def\arraystretch{1.5} \begin{array}{c} \hline \rm Acid &&&K_a\\ \hline HOAc&&&1.8 \times 10^{-5}\\ HCHO_2&&&1.8 \times 10^{-4}\\ HClO &&& 3.0 \times 10^{-8}\\ HF &&& 6.8 \times 10^{-4}\\ \hline \end{array}
Acids and Bases: Acidity
Nitrous acid has a Ka of 7.1 x 10-5. What are [H3O+] and [NO2- ] in 0.50 M HNO2?
Which of the solutions below would have the HIGHEST pH value?
Methyl diethanolamine CH3N(C2H4OH)2 is a weak base which we will abbreviate as mdea. The conjugate acid, mdeaH+, has a pKa = 8.52.
Practice: Relating [H3O+], [OH-], pH and pOH
Compare two acids and their 1M solution:
Acid 1:Ka=1.0×10−3Acid 2:Ka=1.0×10−6\rm Acid\ 1:K_a=1.0\times10^{-3}\qquad Acid\ 2:K_a=1.0\times10^{-6}