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Consider the weak bases below and their Kb values: C6H7O Kb = 1.3 …

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Wize University Chemistry Textbook > Acids and Bases

Applications of Acid and Base Equations

3 Activities

Wize University Chemistry Textbook > Acids and Bases

Conjugate Acid-Base Pairs

2 Activities

Consider the weak bases below and their Kb values:
C6H7O Kb = 1.3 x 10-10
C2H5NH2 Kb = 5.6 x 10-4
C5H5N Kb = 1.7 x 10-9
Arrange the conjugate acids of these weak bases in order of increasing acid strength.
More Applications of Acid and Base Equations Questions:
Weak Acids and Bases
Calculate the pH of the following solution.
A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Note: Acetic Acid Ka = 1.8 x 10-5
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a) A 6.30 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.500 g of sodium hydrogen phosphate (Na2HPO4, MW = 141.9579 g/mol) in 150.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a) A 6.30 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Weak Acids and Bases
Will HCO3- act as an acid or as a base?
Weak Acids and Bases
Calculate the pH and pOH of the following solutions, knowing that Ka = 1.8x10^-5.
a) A 5.33 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 1.15 x 10-3 g of CH3COONa in 100.0 mL of water.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.150 g of sodium hydrogen phosphate (Na2HPO4, MW = 141.9579 g/mol) in 125.0 mL of water.
Ka (HPO42−) = 4.2 x 10−13;  Kb (HPO42−) = 1.6 x 10−7. K_a\ \left(HPO_4^{2-}\right)\ =\ 4.2\ x\ 10^{-13};\ \ K_b\ \left(HPO_4^{2-}\right)\ =\ 1.6\ x\ 10^{-7}.\
Weak Acids and Bases
Calculate the percent dissociation for the following solutions.
a) A 0.444 M aqueous solution of HCN (Ka = 6.2 x 10-10).
b) A 3.50 x 10-2 M aqueous solution of NaCN.
Weak Acids and Bases
Sulfurous acid (H2SO3) is a diprotic weak acid (pKa1 = 1.85, pKa2 = 7.20). Bisulfite (HSO3-) is the conjugate base of sulfurous acid and is an amphoteric species (can act as an acid or a base). Will HSO3- act as an acid or as a base?
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 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
Find the pH during titration of 20.00 mL of 0.100 M butanoic acid with 0.100 M NaOH solution after the following additions of base: 0 mL, 10.00 mL, 20.00 mL, 25.00 mL (Ka = 1.54 x 10-5)
Acids and Bases: pH
What is the pH of a 0.10 M solution of NaF? (Ka for HF = 6.8×10-4)?
More Conjugate Acid-Base Pairs Questions:
In a reaction, which of the following could be conjugate acid-base pairs?
Weak Acids and Bases
Will HCO3- act as an acid or as a base?
Weak Acids and Bases
Sulfurous acid (H2SO3) is a diprotic weak acid (pKa1 = 1.85, pKa2 = 7.20). Bisulfite (HSO3-) is the conjugate base of sulfurous acid and is an amphoteric species (can act as an acid or a base). Will HSO3- act as an acid or as a base?
In the reaction HSO4−(aq) + OH−(aq) ⇌ SO42−(aq) + H2O (l)HSO_4^-\left(aq\right)\ +\ OH^-\left(aq\right)\ ⇌\ SO_4^{2-}\left(aq\right)\ +\ H_2O\ \left(l\right) the conjugate acid-base pairs are
Select which of the following WOULD NOT be a conjugate acid/base pair.
Consider the following reaction:
NH4++OH−⇌H2O+NH3NH^{4+}+OH^-\rightleftharpoons H_2O+NH_3
Choose the INCORRECT statement
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
HCl+H2O⇌\rm HCl\quad+\quad H_2O\quad \xrightleftharpoons{\hspace{1.5cm}}
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
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}
In the reaction HSO4(aq)−+OH(aq)−⇌SO4(aq)2−+H2O(l)HSO^-_{4(aq)}+OH^-_{(aq)} \rightleftharpoons SO^{2-}_{4(aq)}+H_2O_{(l)}the conjugate acid-base pairs are
To 2L of pure water is added Mg(ClO4)2. What would the effect on pH be?
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,
A series of solutions are formed with strontium salts of the form SrX2 where X=F, Cl, Br, I.
Which of the solutions will have the highest pH?
Pure water has a pH of 7.00. 1.1g of MgBr2 is added to 15L of pure water. The solubility of MgBr2 in water is approximatly 101.5g/L. What is the pH of the resulting solution?
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
HCl+NH3⇌\rm HCl\quad+\quad {NH_3}\quad \xrightleftharpoons{\hspace{1.5cm}}
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
+CH3COOH⇌H2O+Na+CH3COO−\rm \quad+\quad {CH_3COOH}\quad \xrightleftharpoons{\hspace{1.5cm}}\quad H_2O\quad+\quad Na^+CH_3COO^-
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
Acids and Bases: Conjugate
In each equation, label the acids, bases and conjugate acid-base pairs
NH3+H3PO4↔NH4++H2PO4−NH_3+H_3PO_4 \leftrightarrow NH^+_4+H_2PO^-_4
CH3O−+NH3↔CH3OH+NH2−CH_3O^-+NH_3 \leftrightarrow CH_3OH+NH^-_2
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
HCl+H2O⇌\rm HCl\quad+\quad H_2O\quad \xrightleftharpoons{\hspace{1.5cm}}
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
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: Conjugate identification
In the reaction HSO4-(aq) + OH-(aq) ⇌ SO42-(aq) + H20(l), the conjugate acid-base pairs are:
B is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HB+?
Acids and Bases: Conjugate Acid-base Pairs
Indicate how many of these combinations are conjugate acid-base pairs. Select all that apply.