High School
SAT
ACT
University
MCAT
LSAT
DAT

Acids and Bases

Related Topics

Wize University Chemistry Textbook > Acids and Bases

Applications of Acid and Base Equations

3 Activities

checklist
Mark Yourself Question
  1. Grab a piece of paper and try this problem yourself.
  2. When you're done, check the "I have answered this question" box below.
  3. View the solution and report whether you got it right or wrong.
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)
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}
Consider the weak bases below and their Kb values:
C6H7O Kb = 1.3 x 10-10
C2H5NH2 Kb = 5.6 x 10-4
Acids and Bases: pH
What is the pH of a 0.10 M solution of NaF? (Ka for HF = 6.8×10-4)?