Binary Acids
A binary compound consists of two elements. Binary acids have the prefix hydro in front of the full name of the nonmetallic element. They have the ending -ic. Examples include hydrochloric and hydrofluoric acid.
Hydrofluoric Acid - HF
Hydrochloric Acid - HCl
Perchloric Acid - HClO4
Sulfuric Acid - H2SO4
Sulfurous Acid - H2SO3
Phosphoric Acid - H3PO4
Phosphorous Acid - H3PO3
Carbonic Acid - H2CO3
Acetic Acid - HC2H3O2
Oxalic Acid - H2C2O4
Boric Acid - H3BO3
Silicic Acid - H2SiO3
Bases
Sodium Hydroxide - NaOH
Potassium Hydroxide - KOH
Ammonium Hydroxide - NH4OH
Calcium Hydroxide - Ca(OH)2
Magnesium Hydroxide - Mg(OH)2
Barium Hydroxide - Ba(OH)2
Aluminum Hydroxide - Al(OH)3
Ferrous Hydroxide or Iron (II) Hydroxide - Fe(OH)2
Ferric Hydroxide or Iron (III) Hydroxide - Fe(OH)3
Zinc Hydroxide - Zn(OH)2
Lithium Hydroxide - LiOH
Hydrobromic Acid - HBr
Hydroiodic Acid - HI
Hydrosulfuric Acid - H2S
Ternary Acids
Ternary acids commonly contain hydrogen, a nonmetal, and oxygen. The name of the most common form of the acid consists of the nonmetal root name with the -ic ending, The acid containing one less oxygen atom than the most common form is designated by the -ous ending. An acid containing one less oxygen atom than the -ousacid has the prefix hypo- and the -ousending. The acid containing one more oxygen than the most common acid has the per- prefix and the -icending.
Nitric Acid - HNO3
Nitrous Acid - HNO2
Hypochlorous Acid - HClO
Chlorous Acid - HClO2
Chloric Acid - HClO3
Examples of acids include hydrochloric acid, citric acid, and sulfuric acid. Examples of bases include sodium hydroxide, ammonia, and magnesium hydroxide. Examples of neutrals include water, carbon dioxide, and ethanol.
Identifying Weak acids and bases depend on: When The Elements of these acids react they completely ionise with water and form Strong salts without being in the oh- situation, then its a strong Acid.
Substances that can neutralize acids are called bases. Bases can react with acids to form salt and water through a chemical reaction called neutralization. Examples of bases include sodium hydroxide, potassium hydroxide, and ammonia.
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Amphoteric elements are elements that can act as either acids or bases. Common examples include aluminum, zinc, and lead. These elements can form salts both with acids and bases.
Acids and bases are not salts.
Bases are substances that can undergo neutralization reactions with acids. Hydroxides of Group 1 and 2 can be given as examples for bases.
Buffers are weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH....
orange juice
Examples of acids include hydrochloric acid, citric acid, and sulfuric acid. Examples of bases include sodium hydroxide, ammonia, and magnesium hydroxide. Examples of neutrals include water, carbon dioxide, and ethanol.
Identifying Weak acids and bases depend on: When The Elements of these acids react they completely ionise with water and form Strong salts without being in the oh- situation, then its a strong Acid.
Substances that can neutralize acids are called bases. Bases can react with acids to form salt and water through a chemical reaction called neutralization. Examples of bases include sodium hydroxide, potassium hydroxide, and ammonia.
Examples: hydrochloric acid, sodium chloride
Yes, concentrated acids and bases are more corrosive than dilute acids and bases
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Of course they are. They are many acids and bases
bases neutralise the acids