Acids, Bases and Salts Quiz

Chemical substances that taste sour and turn blue litmus paper red.

A common acid, often represented as HCl.

Produces salt, water, and carbon dioxide gas.

Turning limewater milky confirms CO2 presence.

A compound containing a metal and carbonate ion (CO3-2).

Burning a splinter near soap bubble containing hydrogen gas.

A brisk bubbling or fizzing produced by a gas escaping from a liquid.

Acids found in various natural sources like fruits and foods.

Adding water to an acid/base to decrease its concentration.

Acids release H+ ions in water, forming hydronium (H3O+) ions.

Bases release OH- ions in water.

Reaction between an acid and a base to produce a salt and water.

Add acid to water, never the other way around, stirring constantly to prevent splashing.

A chemical reaction where an acid and a base react to form water and a salt.

H+ ions released by acids combine with water molecules to form hydronium ions (H3O+).

Bases usually contain a metal hydroxide (MOH).

Substances that change color in acidic solutions, used to identify acids.

Substances that change color in alkaline (basic) solutions, used to identify bases.

Indicator derived from natural sources, like plants.

Indicator made in a lab or factory, not from nature.

Mixture of indicators showing different colors at various hydrogen ion concentrations (pH levels).

Indicator whose smell changes in acidic or basic mediums.

Depends on the number of H+ ions produced.

Depends on the number of OH- ions produced.

Chemical name: Sodium chloride; chemical formula: NaCl. Made from the reaction of hydrochloric acid and sodium hydroxide or extracted from sea water or rock salt.

Chemical name: Sodium hydroxide; chemical formula: NaOH. Formed through electrolysis of sodium chloride solution (brine).

Neutral pH, neither acidic nor basic.

Salt formed from a strong acid and weak base.

Salt formed from a strong base and weak acid.

Electrolytic process that produces sodium hydroxide (caustic soda) and chlorine from sodium chloride (brine).

A substance that changes color depending on whether it is in an acidic or alkaline solution.

Sodium hydrogen carbonate, commonly known as baking soda, is used in baking powder to create carbon dioxide gas, which makes bread and cakes rise and become fluffy. This occurs when baking powder mixes with water or heat.

Beyond baking, sodium hydrogen carbonate also acts as an antacid, neutralizing stomach acid for relief. It's used in fire extinguishers and as a preservative for milk, preventing souring by reacting with lactic acid.

Washing soda is the common name for sodium carbonate decahydrate, a white crystalline solid with a chemical formula Na₂CO₃·10H₂O.

Washing soda's solution in water is alkaline, turning litmus blue. Its key property is dissolving dirt and grease, making it a cleaning agent for laundry.

Washing soda is prepared by heating baking soda, which decomposes it to sodium carbonate. Recrystallization from water then forms sodium carbonate decahydrate.

Washing soda finds applications in glass, soap, and paper industries. It's used to make other sodium compounds like borax and to remove permanent hardness from water.

Plaster of Paris is the common name for calcium sulfate hemihydrate, with a chemical formula CaSO₄·½H₂O. It's a white powder that hardens when mixed with water.

Plaster of Paris is made by heating gypsum (CaSO₄·2H₂O) at 373 K. This process removes water molecules, converting gypsum to calcium sulfate hemihydrate.

A white powder formed by heating gypsum (CaSO4·2H2O) to 373K, losing some water of crystallization, becoming CaSO4·1/2H2O. It sets hard when mixed with water.

A naturally occurring mineral, chemically calcium sulfate dihydrate (CaSO4·2H2O). It is used for making plaster of Paris.

Plaster of Paris (CaSO4·1/2H2O) reacts with water to form gypsum (CaSO4·2H2O), a harder solid. This process is called setting.

Water molecules that are chemically bound within the crystal structure of a compound. They are an essential part of the crystal's structure.

Salts containing water of crystallization, such as CuSO4·5H2O (copper sulfate pentahydrate) or CaSO4·2H2O (gypsum).

Salts which have lost their water of crystallization, for example, anhydrous copper sulfate (CuSO4).

Anhydrous calcium sulfate (CaSO4) obtained by heating gypsum above 400K. Unlike plaster of Paris, it cannot harden with water.

Heating hydrated salts removes water of crystallisation, resulting in a change of physical properties like shape and color. They become anhydrous salts.