Podcast
Questions and Answers
A weak acid is one for which the equilibrium lies far to the right.
A weak acid is one for which the equilibrium lies far to the right.
False
Phosphoric acid (H3PO4) is an example of a strong acid.
Phosphoric acid (H3PO4) is an example of a strong acid.
False
A strong conjugate base is formed from a weak acid.
A strong conjugate base is formed from a weak acid.
True
PH = -log [OH-] for a strong acid.
PH = -log [OH-] for a strong acid.
Signup and view all the answers
The pH of a 0.10M solution of HCl is 2.
The pH of a 0.10M solution of HCl is 2.
Signup and view all the answers
The pH of a 0.10M solution of H2SO4 is -log[0.2].
The pH of a 0.10M solution of H2SO4 is -log[0.2].
Signup and view all the answers
The concentration of H+ in an aqueous solution with an OH- concentration of 1.2 x 10-6 M is 8.3 x 10-7.
The concentration of H+ in an aqueous solution with an OH- concentration of 1.2 x 10-6 M is 8.3 x 10-7.
Signup and view all the answers
The pH of an aqueous solution with an OH- concentration of 1.2 x 10-6 M is 7.1.
The pH of an aqueous solution with an OH- concentration of 1.2 x 10-6 M is 7.1.
Signup and view all the answers
A weak acid dissociates completely into ions.
A weak acid dissociates completely into ions.
Signup and view all the answers
The conjugate base of a weak acid is always weak.
The conjugate base of a weak acid is always weak.
Signup and view all the answers
Study Notes
Volumetric Analysis
- Volumetric analysis is a type of analytical chemistry that deals with the measurement of the volume of a solution required to react completely with a known volume of another solution.
- Problems in volumetric analysis include calculating the mole fraction of a substance in a solution, determining the normality of a solution, and expressing the concentration of a solution in different units.
Mole Fraction and Molarity
- The mole fraction of a substance in a solution is the ratio of the number of moles of the substance to the total number of moles of all substances in the solution.
- The molarity of a solution is the number of moles of solute per liter of solution.
Normality and Molarity
- The normality of a solution is the number of equivalents of solute per liter of solution.
- Normality is related to molarity by the formula: Normality = Molarity x Number of equivalents per mole.
Concentration Units
- Concentration units include g/L, ppm, and ppb.
- ppm (parts per million) is a unit of concentration that represents the number of parts of a substance per million parts of a solution.
- ppb (parts per billion) is a unit of concentration that represents the number of parts of a substance per billion parts of a solution.
Acids and Bases
- Acids are substances that donate a proton (H+), while bases are substances that accept a proton.
- The Arrhenius theory of acids and bases defines acids as substances that increase the concentration of H+ in a solution, and bases as substances that increase the concentration of OH- in a solution.
Bronsted-Lowry Theory
- The Bronsted-Lowry theory of acids and bases defines an acid as a substance that donates a proton, and a base as a substance that accepts a proton.
- This theory is an improvement over the Arrhenius theory because it can explain the behavior of acids and bases in non-aqueous solutions.
Lewis Theory
- The Lewis theory of acids and bases defines an acid as a substance that accepts an electron pair, and a base as a substance that donates an electron pair.
- This theory is more general than the Bronsted-Lowry theory because it can explain the behavior of acids and bases in a wide range of solutions.
Leveling Effect
- The leveling effect is the phenomenon where the strength of an acid is determined by the solvent in which it is dissolved.
- In a solvent such as water, the leveling effect causes strong acids to be completely dissociated, while weak acids are only partially dissociated.
Acid Strength
- The strength of an acid is defined by the equilibrium position of its dissociation reaction.
- A strong acid is one that is completely dissociated in a solvent, while a weak acid is one that is only partially dissociated.
pH Calculation
- The pH of a solution is calculated using the formula: pH = -log[H+].
- The pH of a strong acid solution can be calculated using the formula: pH = -log[Concentration of acid].
- The pH of a weak acid solution can be calculated using the formula: pH = -log[Concentration of acid] + pKa.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
This quiz covers volumetric analysis in analytical chemistry, with questions on weak acids and mole fractions. Prepared by Dr. Ahmed Bahgat.
