Acid-Base Indicators and Reactions Quiz

Substances like lemon juice, vinegar, and orange juice that taste sour and turn blue litmus paper red.

Substances like soap, baking soda, and antacids that taste bitter and turn red litmus paper blue.

Natural substances like litmus, turmeric, and red cabbage that change color in the presence of acids or bases, indicating their acidic or basic nature.

The reaction of acids and bases that neutralizes their effects, resulting in the formation of salt and water. For example, when baking soda (a base) is added to vinegar (an acid), the mixture fizzes and neutralizes the acidic nature of vinegar.

A substance formed when an acid reacts with a base. For example, when hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH), sodium chloride (NaCl) (table salt) is formed.

Litmus is commonly used as an indicator. When a litmus solution is neither acidic nor basic, its color is purple.

A substance that changes color in the presence of an acid or base, helping to indicate whether a solution is acidic or basic.

Indicators such as methyl orange and phenolphthalein are synthetically produced and used to test for acids and bases.

Substances that change color in the presence of acids or bases, indicating their pH.

A substance with a pH less than 7, typically sour-tasting and can react with metals to produce hydrogen gas.

A substance with a pH greater than 7, typically bitter-tasting and can react with acids to form salts and water.

A chemical compound formed when an acid reacts with a base.

A measure of the acidity or alkalinity of a solution, with a scale ranging from 0 to 14.

A chemical reaction where an acid reacts with a metal to produce a salt and hydrogen gas.

A chemical reaction where a carbonate reacts with an acid to produce carbon dioxide gas, water, and a salt.

A chemical reaction where a base reacts with an acid to produce a salt and water.

A common indicator used to detect the presence of acid or base, turning red in acidic solutions and blue in basic solutions.

A chemical compound known as calcium carbonate, found in limestone, chalk, and marble.

A chemical compound known as sodium bicarbonate, a common ingredient in baking.

A chemical compound formed when a metal reacts with a base. This reaction usually produces hydrogen gas.

A chemical reaction where a metal reacts with a base to produce hydrogen gas.

A type of acid known as acetic acid, commonly found in vinegar.

A type of indicator used to detect the presence of acid or base, turning pink in basic solutions and colorless in acidic solutions.

Metallic oxides react with acids to form a salt and water.

Non-metallic oxides react with bases (like metal hydroxides) to form a salt and water.

These oxides act as bases when they react with acids.

These oxides exhibit acidic properties when they react with bases.

Hydrogen gas (H2) is usually liberated when an acid reacts with a metal. For example, hydrochloric acid (HCl) reacts with zinc (Zn) to produce hydrogen gas (H2) and zinc chloride (ZnCl2).
2HCl(aq) + Zn(s) → ZnCl2(aq) + H2(g)

Carbon dioxide gas (CO2) is usually liberated when an acid reacts with a metal carbonate or metal hydrogencarbonate. For example, hydrochloric acid (HCl) reacts with calcium carbonate (CaCO3) to produce carbon dioxide gas (CO2), calcium chloride (CaCl2), and water (H2O). CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)

A substance that changes color in the presence of an acid or base, indicating their acidic or basic nature. Examples include litmus paper, turmeric, and red cabbage.

Acids generate hydrogen ions (H+) in solution, which are responsible for their acidic properties.

Solutions of acids conduct electricity due to the presence of ions (H+ and anions).

HCl gas is not acidic when dry. It becomes acidic when it dissolves in water and forms H+ ions.

Bases produce hydroxide ions (OH-) in solution, which contribute to their basic properties.

Solutions of bases conduct electricity due to the presence of ions (cations and OH-).

The reaction of an acid with a base to form a salt and water is called neutralization.

A base that dissolves in water. They are soapy to touch, bitter, and corrosive.

A process that occurs when an acid or a base is mixed with water, resulting in a decrease in the concentration of ions (H3O+/OH-) per unit volume.

A scale that measures the concentration of hydrogen ions (H+) in a solution. It ranges from 0 (very acidic) to 14 (very alkaline).

A solution with a pH value less than 7. It has a higher concentration of hydrogen ions (H+).

A solution with a pH value greater than 7. It has a higher concentration of hydroxide ions (OH-).

A solution with a pH value of 7. It has an equal concentration of hydrogen ions (H+) and hydroxide ions (OH-).

The ability of an acid or base to release a large number of ions. Strong acids release a large amount of hydrogen ions (H+), and strong bases release a large amount of hydroxide ions (OH-).

Rain with a pH value less than 5.6. It is caused by air pollution, primarily from sulfur dioxide and nitrogen oxides, which react with water to form acids.

The process of measuring the pH of a solution using a universal indicator. The universal indicator shows different colors at different pH values.

Adding water to an acid or base, resulting in a decrease in concentration of ions (H3O+/OH-).

Substances produced by the reaction of an acid and a base. They are typically ionic compounds formed by the neutralization of an acid by a base.

A highly exothermic process where the acid is always added slowly to water with constant stirring to prevent splashing and burns.

A solution containing a substance that changes color in the presence of different acids or bases, indicating its acidic or basic nature.

A chemical reaction where an acid reacts with a metal hydrogencarbonate, producing carbon dioxide, water, and a salt. The carbon dioxide is what creates the pressure buildup in fire extinguishers.

A measure of the acidity or alkalinity of a substance, ranging from 0 (highly acidic) to 14 (highly alkaline), with 7 being neutral.

A thin strip of paper treated with a chemical indicator that changes color depending on the pH of a solution, providing a quick visual estimate of acidity or alkalinity.

A substance that releases hydrogen ions (H+) in water, making the solution acidic.

A substance that accepts hydrogen ions (H+) in water, making the solution alkaline.

The most common natural source of acid, found in vinegar, is acetic acid.

The breakdown of sugar and food particles in the mouth by bacteria produces acids.

The protective outer layer of teeth, made up of calcium hydroxyapatite, is resistant to water but can be corroded by acids below a pH of 5.5, leading to tooth decay.

A mild base often used to neutralize excess stomach acid and relieve indigestion.

A plant with stinging hairs that inject methanoic acid, causing pain.

A substance that changes color in the presence of acids or bases, indicating their presence.

Salts containing the same positive or negative ions belong to the same family, such as sodium chloride and sodium sulfate, both being sodium salts.

A salt containing water molecules chemically bound within its crystal structure.

A compound where water molecules are chemically bonded to a metal cation, forming a specific ratio within the crystal structure.

CaSO4.1/2H2O, a white powder formed by heating gypsum at 373K, used for making toys, decorations, and smoothing surfaces.

CaSO4.2H2O, a naturally occurring mineral used in building materials and for making cement.

When a metal reacts with an acid, hydrogen gas is released, leaving a salt and water behind.

When an acid reacts with a metal carbonate or hydrogencarbonate, it forms a salt, carbon dioxide gas, and water.

Sodium carbonate (Na2CO3), used for softening hard water.

Calcium hypochlorite (CaOCl2), a strong oxidizing agent used as a bleaching agent and disinfectant.

Sodium bicarbonate (NaHCO3), a compound used for baking, antacids, and cleaning.

The chemical reaction involved in the decomposition of sodium bicarbonate (baking soda) when heated; NaHCO3(s) → Na2CO3(s) + H2O(g) + CO2(g).

The chemical reaction between Plaster of Paris (CaSO4.1/2H2O) and water that forms gypsum (CaSO4.2H2O); CaSO4.1/2H2O + 1 1/2H2O → CaSO4.2H2O.

The common salt used in food is sodium chloride (NaCl). It is formed by the reaction of hydrochloric acid and sodium hydroxide.

The process of separating sodium chloride from seawater or rock salt deposits involves removing impurities and obtaining pure sodium chloride.

A neutral salt is formed when a strong acid reacts with a strong base. It neither shows acidic nor basic properties.

Sodium hydroxide (NaOH) is a strong base commonly known as lye or caustic soda. It is produced by the electrolysis of brine.

The chlor-alkali process is the electrolysis of brine (aqueous sodium chloride) to produce sodium hydroxide, chlorine gas, and hydrogen gas.

Chlorine gas is produced as a byproduct of the chlor-alkali process. It is a yellowish-green gas with a pungent odor.

Hydrogen gas is another byproduct of the chlor-alkali process. It is the lightest element and is highly flammable.

Bleaching powder is a white powder used as a bleaching agent and disinfectant. It is produced by reacting chlorine gas with dry slaked lime.

Baking powder is a mixture of baking soda (sodium hydrogencarbonate) and a mild edible acid. It releases carbon dioxide when heated, making baked goods rise.

Washing soda is sodium carbonate decahydrate (Na2CO3.10H2O). It is used in various industries and for cleaning.

Hydrated copper sulfate (CuSO4.5H2O) is a blue crystalline salt containing five water molecules per formula unit. It turns white upon heating due to the loss of water.

The process of removing water of crystallization from a hydrated salt by heating is called dehydration.