10.1 - Acids and Bases

H+ is produced by Arrhenius acid, OH- is generated by Arrhenius base in aqueous solutions.
- Acids taste sour, sting, and neutralize the foundations.
- Bases are bitter, slippery, and acid-neutralizing.
Simple anionic acids use a prefix, whereas ic or ous acids are named with oxygen-containing polyatomic anions.

10.2 - Brønsted–Lowry Acids and Bases

Acids are H+ donors and bases are H+ acceptors, according to Brønsted–Lowry theory.
- The loss or gain of one H+ is linked to a conjugate acid-base pair.
- The F- is the conjugate base, for example, when the HF acid gives H+. H3O+/H2O would be the other acid-base pair.

Strong acids are totally dissociated in water, and H+ is accepted as a basis for H2O.
- Slightly dissociate weak acids in water, producing little H3O+.
The hydroxides of the 1A(1) and 2A(2) groups are strong bases and fully dissociate from water.
- Ammonia, NH3, is an important weak base.

In a reversible reaction, the chemical balance occurs if the rate of the reverse reaction is equal to its rates.
- At equilibrium, reactants and products are not further affected as reverse and forward reactions continue.
When reactants are removed or products are added to a balanced mixture, the system moves to reactants to restore balance
- When reactants are added or products are removed from the balanced mix, the system moves toward the product to restore balance.

A few water molecules in pure waters transfer H+ to other water molecules, which produce small but equal H3O+ and OH- amounts.
- The molar levels of H3O+ and OH- are 1,0 * 10-7 M in pure water each.
- Kw = [H3O+] The expression of water dissociation = 1,0 * 10-14 at 25 degrees Celsius.
- [H3O+] is higher than [OH-] in acidic solutions.
- The [OH-] is larger than the [H3O+] in basic solutions.

H2O and OH Concentrations vs. Acidity of solution

The pH scale is the [H3O+] of solution for a range of numbers, typically 0 to 14.
A pH of 7.0 is available in a neutral solution.
- The pH is lower than 7.0 is acidic solutions; the pH in basic solutions is higher than 7.0.
The negative logarithm of pH ion concentration, pH = -log[H3O+], is the mathematical pH.

In the production of hydrogen gas and salt, an acid reacts with a metal.
The carbonate or bicarbonate reaction of acid produces carbon dioxide, water, and salt.
- An acid reacts with a basis for water and salt in neutralization.
- An acid sample with a known amount of a base is neutralized in the titration.
The acid concentration is calculated based on the volume and molarity of the base.

When small amounts of acid or base are added, a buffer solution resists pH changes.
- A buffer has either a faint acid, salt, or a weak base, and salt
A buffer with the addition of OH reacts with weak acid, and the salt anion reacts with the addition of H3O+.

H+ is produced by Arrhenius acid, OH- is generated by Arrhenius base in aqueous solutions.
- Acids taste sour, sting, and neutralize the foundations.
- Bases are bitter, slippery, and acid-neutralizing.
Simple anionic acids use a prefix, whereas ic or ous acids are named with oxygen-containing polyatomic anions.

Acids are H+ donors and bases are H+ acceptors, according to Brønsted–Lowry theory.
- The loss or gain of one H+ is linked to a conjugate acid-base pair.
- The F- is the conjugate base, for example, when the HF acid gives H+. H3O+/H2O would be the other acid-base pair.

Strong acids are totally dissociated in water, and H+ is accepted as a basis for H2O.
- Slightly dissociate weak acids in water, producing little H3O+.
The hydroxides of the 1A(1) and 2A(2) groups are strong bases and fully dissociate from water.
- Ammonia, NH3, is an important weak base.

In a reversible reaction, the chemical balance occurs if the rate of the reverse reaction is equal to its rates.
- At equilibrium, reactants and products are not further affected as reverse and forward reactions continue.
When reactants are removed or products are added to a balanced mixture, the system moves to reactants to restore balance
- When reactants are added or products are removed from the balanced mix, the system moves toward the product to restore balance.

A few water molecules in pure waters transfer H+ to other water molecules, which produce small but equal H3O+ and OH- amounts.
- The molar levels of H3O+ and OH- are 1,0 * 10-7 M in pure water each.
- Kw = [H3O+] The expression of water dissociation = 1,0 * 10-14 at 25 degrees Celsius.
- [H3O+] is higher than [OH-] in acidic solutions.
- The [OH-] is larger than the [H3O+] in basic solutions.

H2O and OH Concentrations vs. Acidity of solution

The pH scale is the [H3O+] of solution for a range of numbers, typically 0 to 14.
A pH of 7.0 is available in a neutral solution.
- The pH is lower than 7.0 is acidic solutions; the pH in basic solutions is higher than 7.0.
The negative logarithm of pH ion concentration, pH = -log[H3O+], is the mathematical pH.

In the production of hydrogen gas and salt, an acid reacts with a metal.
The carbonate or bicarbonate reaction of acid produces carbon dioxide, water, and salt.
- An acid reacts with a basis for water and salt in neutralization.
- An acid sample with a known amount of a base is neutralized in the titration.
The acid concentration is calculated based on the volume and molarity of the base.

When small amounts of acid or base are added, a buffer solution resists pH changes.
- A buffer has either a faint acid, salt, or a weak base, and salt
A buffer with the addition of OH reacts with weak acid, and the salt anion reacts with the addition of H3O+.