Chemistry: Acids & Bases
pH, acid-base reactions, buffers, and titration fundamentals.
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According to the Arrhenius definition, what is an acid?
An Arrhenius acid is a substance that increases the concentration of hydrogen ions (H+) when dissolved in water.
What is the mathematical definition of pH?
pH is defined as the negative base-10 logarithm of the molar hydronium ion concentration: pH = -log[H3O+].
What is the conjugate base of the strong acid H2SO4?
The conjugate base is the hydrogen sulfate ion, HSO4-.
What are the two primary products of a neutralization reaction between a strong acid and a strong base?
The products are liquid water (H2O) and an ionic salt.
List three examples of common strong acids.
Common strong acids include Hydrochloric acid (HCl), Nitric acid (HNO3), and Perchloric acid (HClO4).
If a solution has a pH of 4.5 at 25°C, what is its pOH?
The pOH is 9.5, calculated using the relationship pH + pOH = 14.00.
How does the Brønsted-Lowry theory define a base?
A Brønsted-Lowry base is a substance that acts as a proton (H+) acceptor.
Define a Lewis acid and provide an example of one that does not contain hydrogen.
A Lewis acid is an electron-pair acceptor. An example is Boron trifluoride (BF3).
What is the mathematical relationship between Ka, Kb, and Kw for a conjugate acid-base pair?
The product of the acid dissociation constant (Ka) and the base dissociation constant (Kb) equals the ion-product constant of water (Kw), which is 1.0 x 10^-14 at 25°C.
Why can the pH of a 0.1 M weak acid (HA) not be calculated as -log(0.1)?
Weak acids do not fully dissociate; therefore, the equilibrium concentration of H3O+ is significantly less than the initial concentration of the acid.
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