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.

10.3 - Strengths of Acids and Bases

• 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.

10.4 - Acid–Base Equilibrium

• 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.

10.5 - Dissociation of Water

• 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.

10.6 - The pH Scale

• 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.

10.7 - Reactions of Acids and Bases

• 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.

10.8 - Buffers

• 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+.