The pH of 2.65 M CH3NH2 is 12.54, revealing the fascinating characteristics of this organic compound. This value not only provides insights into its chemical properties but also highlights its potential applications in various scientific disciplines.
To delve deeper into the significance of this pH value, we will explore the concept of pH, the pKa of CH3NH2, and the equilibrium established during its hydrolysis. Additionally, we will uncover the practical applications of CH3NH2, shedding light on its versatility and importance in modern chemistry.
Definition of pH
pH is a measure of the acidity or alkalinity of a solution. It is defined as the negative logarithm (base 10) of the molar concentration of hydrogen ions ([H+]) in a solution:
pH =
log[H+]
Understanding the pKa of CH3NH2
pKa is a measure of the strength of an acid or base. It is defined as the negative logarithm (base 10) of the acid dissociation constant (Ka) of the acid or base. For a base, pKa is related to its basicity:
pKa =
log(Kb)
The pKa of CH3NH2 is 10.63. This indicates that CH3NH2 is a weak base.
Calculation of [OH-] and [H+]
Given the pH of 12.54, we can calculate the concentration of hydroxide ions ([OH-]) in the solution using the following equation:
pH = 14
- pOH = 14
- (-log[OH-])
Therefore, [OH-] = 10^-1.46 = 3.5 x 10^-2 M.
The concentration of hydrogen ions ([H+]) can be calculated using the following equation:
[H+] = Kw/[OH-] = 10^-14/[OH-]
Therefore, [H+] = 10^-14/3.5 x 10^-2 M = 2.9 x 10^-13 M.
Equilibrium Constant (Kb) of CH3NH2
The equilibrium constant (Kb) for a base is a measure of its strength. It is defined as the ratio of the concentration of the base and its conjugate acid at equilibrium:
Kb = [CH3NH2]/[CH3NH3+][OH-]
Using the calculated [OH-] concentration, we can calculate the Kb value for CH3NH2:
Kb = [CH3NH2]/[CH3NH3+][OH-] = 1/[CH3NH3+][OH-]
Therefore, Kb = 1/(2.9 x 10^-13 M) = 3.45 x 10^12.
Hydrolysis of CH3NH2
Hydrolysis is a reaction in which a compound reacts with water to form a new compound. In the case of CH3NH2, hydrolysis occurs as follows:
CH3NH2 + H2O → CH3NH3+ + OH-
The equilibrium constant for this reaction is known as the hydrolysis constant (Kh).
Applications of CH3NH2: The Ph Of 2.65 M Ch3nh2 Is 12.54
CH3NH2 is used in a variety of applications, including:
- As a solvent in organic chemistry
- As a catalyst in the production of pharmaceuticals
- As a reagent in environmental analysis
Essential Questionnaire
What is the significance of pH in chemistry?
pH is a crucial parameter in chemistry as it indicates the acidity or alkalinity of a solution, providing insights into the chemical reactions and properties of substances.
How does the pKa of CH3NH2 influence its basicity?
The pKa of CH3NH2 determines its strength as a base. A lower pKa value indicates a stronger base, meaning CH3NH2 readily accepts protons and forms hydroxide ions.
What is the practical importance of CH3NH2?
CH3NH2 finds applications in various fields, including organic synthesis, pharmaceutical manufacturing, and environmental remediation. Its unique properties make it a valuable reagent and intermediate in chemical processes.
