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The equilibrium constant ( K_b ) for the reaction of methylamine (CH₃NH₂) with water to form its conjugate acid (CH₃NH₃⁺) and hydroxide ions (OH⁻) can be expressed as:
[ K_b = \frac{[CH_3NH_3^+][OH^-]}{[CH_3NH_2]} ]
This reaction represents the base dissociation of methylamine in aqueous solution, where it acts as a weak base. The value of ( K_b ) can be determined experimentally or calculated using the relationship between ( K_w ), ( K_a ), and ( K_b ) if the ( K_a ) for its conjugate acid is known.
What else can I help you with?
What is the equation for potassium bromide and water?
KBr + H2O = Kaq+ Braq- Haq+ OHaq-
Is ammonium hydroxide soluble in ethanol?
There is no such thing as an ammonium hyroxide salt because when an ammonium ion comes into contact with a hydroxide, it spontaneously forms NH3 gas and water. But fundamentally it would be soluble because all ammonium ions are soluble. Hope this helps
