Respuesta :
The pH of a 0.0100 m solution of aniline (c6h5nh2) , a weak base. kb = [tex]4.0 * 10^{-10}[/tex] (ice problem) is 8.30. pH, historically referring to "potential of hydrogen", is a scale that is used to measure the acidity or basicity of an aqueous solution. The more the solution is acidic the less is the pH and more the solution is basic higher is the pH.
In order to calculate the pH of an aqueous solution we must be aware of the value of the concentration of the hydronium ion in moles per liter that is called molarity. The pH is calculated using the expression:
pH = - log [H3O+],
Kb is the base dissociation constant. It is a measure to know how completely a base has dissociated into its component ions in water.
Let us now see a example:
What is the pH of a 0.15 M solution of weak acid ammonium bromide? The Kb value for ammonia is 1.8 × 10^–5?
⇒ x =[tex]\sqrt{1.8*{10^{-5} }(0.15)}[/tex]
⇒ x = [tex]5.1 *10^{-3}[/tex]
⇒ log([tex]5.1*10^{-3}[/tex])
⇒ pH = 2.79
⇒ pH = 14-2.79
⇒ pH = 11.71
Hence, the pH of a 0.15 M solution o weak acid ammonium bromide is 11.71.
To learn more about pH, head here
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