Chapter 20 - Acids, bases and pH Flashcards
What is a Brønsted-Lowry acid?
A proton donor.
What is a Brønsted-Lowry base?
A proton acceptor.
What is a conjugate acid-base pair?
Two species that can be interconverted by transfer of a proton.
The formula of the acid and base in a conjugate acid-base pair differs by H+.
What is a monobasic acid?
An acid in which each molecule can release one proton.
What is a dibasic acid?
An acid in which each molecule can release two protons.
What is a tribasic acid?
An acid in which each molecule can release three protons.
What is the acid dissociation constant, Ka?
The equilibrium constant that measures the extent of acid dissociation.
The larger the value of Ka, the _______ the pKa value and the ________ the acid.
The larger the value of Ka, the smaller the pKa value and the stronger the acid.
Water can acts as an ____ or a ____.
Water can acts as an acid or a base.
The larger the value of [H+], the _______ the pH value and the more _____ the solution is.
The larger the value of [H+], the smaller the pH value and the more acidic the solution is.
What is an important rule to remember about strong monobasic acids?
[H+] = [HA]
A strong acid completely dissociates.
What is the ionic product of water?
Kw = [H+] [OH-]
In all aqueous solutions, H+(aq) and OH-(aq) are both present.
When [H+] = [OH-]…
When [H+] > [OH-]…
When [H+] < [OH-]…
…a solution is neutral.
…a solution is acidic.
…a solution is alkaline.
For a strong monobasic base…
[OH-] = [Base]
If you are given [Base] and temperature as 25°C or 298K, you can calculate [H+] using _____.
If you are given [Base] and temperature as 25°C or 298K, you can calculate [H+] using Kw.
The value of Kw at 298K is given in the data sheet.
