10.1 Acids and Bases

10.1 Acids and Bases

• In health, industry, and the environment acids and bases are important substances.
• Lemons and grapefruits have acids that make them sour.
• Lactic acid is produced when we exercise.

• The production of yogurt and cottage cheese is affected by acid frombacteria.

• Acidic water is electrolytes.
• In water, hydrogen chlorides give hydrogen ion, H+, and chloride ion, Cl-.

• A hydrogen ion and a negative ion can be produced by acids dissolving in water.
• Hcl is an acid that is named hydrocyanic acid.

• The hydrogen ion and the presence of acids can be produced by an acid dissolving in water.

• Group 7A 17 can form more than two acids.

• Antacids, drain openers, and oven cleaners are some of the household bases you may be familiar with.

• It's completely in the water to give Na+) and OH-.

• An Arrhenius base makes cations and OH- anions.

• Give the name for H2CO3 if you identify it as an acid or a base.

• There are conjugate acid-base pairs for Bronsted-Lowry acids.

• The definition of acids and bases was expanded by J. N. Bronsted and T. M. Lowry in 1923.

• H+ is donated by a substance called a bronsted-lowry acid.

• A bronsted-lowry base can accept H+.

• There is no free hydrogen ion in water.

• A transfer of H+ from hydrogen chloride to water can be written as a hydrochloric acid solution.
• Water is acting as a base by accepting an H+ in the reaction.

• ammonia acts as a base when it reacts with water.
• Water acts as an acid by donating H+ because the nitrogen atom of NH3 has a stronger attraction for H+ than oxygen.

• Water acts as a Bronsted-Lowry base when HNO3 reacts with it.

• Every acid-base reaction has two conjugate acid-base pairs because an H+ is transferred in both directions.
• The conjugate base F- is formed when an acid loses one H+.
• H3O+ is formed when the base H2O gains an H+.

• The conjugate acid-base pairs can be identified using the relationship of loss and gain of one H+.

• The loss and gain of one H+ is related to 2O/OH-.

• Water can act as an acid when it donates H+ or as a base when it accepts H+.
• The basic behavior of water depends on the other reactant.
• Water donates H+ when it reacts with a stronger base and accepts H+ when it reacts with a stronger acid.
• Bicarbonate is an amphoteric substance.
• HCO3 acts as an acid and donates one H+ to give CO 2 3

• The acid that loses H+ is identified.
• H+ was donated to form the product.
• The acid and the conjugate base are named after it.

• The base is the reactant that gains H+.

• NH3 is the base and NH4 is the conjugate acid.