What is the product of hydrogen ion and hydroxide ion in a neutralization reaction?

This is part of the HSC Chemistry course under the topic Properties of Acids and Bases.

HSC Chemistry Syllabus

• Predict the products of acid reactions and write balanced equations to represent:
  • acids and bases (neutralisation)
  • acids and carbonates
  • acids and metals (ACSCH067)

What type of reactions involve acids and bases?

This video explores various reactions involving acids and bases including reactions between:

• acid and metal hydroxide (neutralisation)
• acid and metal
• acid and metal oxide
• acid and metal (hydrogen) carbonate

Acid and Base Reactions

• Acid/base reactions encompass a wide range of different reactions. They are more commonly referred to as neutralisation reactions because acids and bases neutralise each other’s chemical properties.

 $$HCl(aq) + H_2O(l) \rightarrow Cl^-(aq) + H_3O^+(aq)$$

 acid           base     conj. base    conj. acid

General equation: acid + metal hydroxide → salt + water

• Reaction between acid and metal hydroxide is considered an acid-base reaction in both the Arrhenius and Brønsted-Lowry definition.

• Acid-base reactions, in the Arrhenius theory always produce water (in addition to salt) because H+ ions (produced by acids) and OH– ions (produced by bases) react in aqueous solution to form water.

 $$HCl(aq) + NaOH(aq) \rightarrow NaCl(aq) + H_2O(l)$$

  acid            base              salt            water

Net ionic equation of an Arrhenius acid-base reaction:

$$H^+(aq) + OH^-(aq) \rightarrow H_2O(l)$$

The reaction between an acid and an Arrhenius base can be simply understood as the neutralisation between hydrogen ions and hydroxide ions.

Brønsted-Lowry Acid-base Reactions

• Acid-base reactions, in the Brønsted-Lowry theory, are reactions that involve transfer of protons or H+ This type of reaction is best exemplified by the dissociation of acid (or base) in water. In this reaction, water acts as both a solvent and base because it accepts a proton from the acid.

• Not all neutralisations produce water. For example, the reaction between ammonia (base) and hydrogen chloride (acid):

$$NH_3(g) + HCl(g) \leftrightharpoons NH_4Cl(s)$$

base          acid            salt

• All reactions with acids form salts which are defined as an ionic compound that consists of an anion of acid and a cation of base. In other words, a salt consists of a conjugate base and a conjugate acid. The ions which make up the salt are spectator ions because they remain dissolved as ions.

Acid and Metal Reactions

General equation: acids + metal → salt + hydrogen gas 

Overall equation

 $$2HCl(aq) + 2Na(s) \rightarrow 2NaCl(aq) + H_2(g)$$

Sodium metal reacts with water to form sodium hydroxide and hydrogen gas:

$$Na(s) + 2H_2O(l) \rightarrow 2NaOH(aq) + H_2(g)$$

Sodium hydroxide then undergoes neutralisation with hydrochloric acid (HCl) to produce salt and water:

 $$NaOH(aq) + HCl(aq) \rightarrow NaCl(aq) + H_2O(l)$$

• The reaction between active metals (low ionisation energy) and dilute acids are extremely volatile. The products are, salt, hydrogen gas and heat – latter two react to produce explosions.

• The production of hydrogen gas can be observed from bubbling and tested by conducting a ‘pop’ test. When hydrogen gas is lit in the presence of oxygen, they react to form water while producing a squeaky pop sound. The water condenses inside the test tube.

 $$H_2(g) + O_2(g) \rightarrow H_2O(l)$$

• Some metals e.g. copper can react with acid to form gases other than hydrogen gas. For example, the reaction between copper metal and concentrated sulfuric acid produces sulfur dioxide.

 $$Cu(s) + H_2SO_4(aq) + 2H^+(aq) \rightarrow Cu^{2+}(aq) + SO_2(g) + 2H_2O(l)$$

• Acids also undergo oxidation-reduction reactions with metals. The hydrogen ions from an acid gain electron from metals (reduction) to produce hydrogen gas. Conversely, metals lose electrons (oxidation) to produce cations.

 $$HCl(aq) + NaOH(aq) \rightarrow NaCl(aq) + H_2O(l)$$

Acid and Metal Oxide Reactions

General equation: acid + metal oxide → salt + water

 $$MgO(s) + 2HCl(aq) \rightarrow MgCl_2(aq) + H_2O(l)$$

Stepwise equations

Metal oxides are considered basic oxides because they react with water to produce metal hydroxides which in turn produce OH– ions in water.

 $$MgO(s) + H_2O(l) \rightarrow Mg(OH)_2(aq)$$

The resultant metal hydroxide neutralises with acid to produce salt and water

 $$Mg(OH)_2(aq) + 2HCl(aq) \rightarrow MgCl_2(aq) + H_2O(l)$$

Acid and Metal (Hydrogen) Carbonate Reactions

General equation: acid + metal carbonates/hydrogen carbonates → salt + water + carbon dioxide

• Carbonates and hydrogen carbonates are Brønsted-Lowry bases because they are able to accept proton(s).

• Carbonates and hydrogen carbonates are not considered as bases in the Arrhenius theory because they do not dissociate into hydroxide ions in aqueous solution.

• Reactions between acids and carbonates/hydrogen carbonates produce salts, water and carbon dioxide.

Lime water test for carbon dioxide

• Carbon dioxide can be identified using the lime water test. Bubbling carbon dioxide in calcium hydroxide, Ca(OH)2 to form milky calcium carbonate, CaCO3.

 $$Ca(OH)_2(aq) + CO_2(aq) \rightarrow CaCO_3(aq) + H_2O(l)$$

BACK TO MODULE 6: ACID/BASE REACTIONS

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What is one of a referee's most significant characteristics? An impartial referee (neutral) is essential. They can't provide one team an advantage over the other. Being neutral in chemistry implies not being an acid or a basic. A neutral material is, for instance, pure water. An acid and a base interact to generate neutral products, such as water, in several chemical processes. As you read this article, you'll see how it all transpires.

NEUTRALIZATION REACTION

A neutralization reaction is a chemical reaction that occurs when an acid and a base react quantitatively to produce water and salt as products.

Before we go further in this topic, let’s understand what acid and base are.

Acid: When an acid dissolves in water, it creates positive hydrogen ions (H ) and negative non-metallic ions. (Ions are atoms that have gained or lost electrons and have become charged.) A good example of an acid is hydrochloric acid (HCl).

Base: A base is a compound that yields negative hydroxide ions (OH-) and positive metal ions when dissolved in water.

ACID-BASE INTERACTION

Acid + base(alkali) → salt + water

A neutral solution is formed when equal quantities of a strong acid, such as hydrochloric acid, are combined with a strong base, such as sodium hydroxide. The reaction's products don't have the properties of an acid or a base. The balanced chemical equation is shown below.

A net ionic equation is a more precise representation of chemical processes that occur in an aqueous solution. The following is the complete ionic equation for the neutralization of hydrochloric acid by sodium hydroxide:

Because the acid and base both are strong, they are totally ionized and, like the NaCl generated, as a result, are recorded as ions. The sodium and chloride ions are spectator ions in the process; hence the net ionic reaction is as follows.

The net ionic reaction of hydrogen ions interacting with the hydroxide ion to form water simplifies all neutralization reactions of a strong acid with a strong base.

CONCLUSION

• A neutralization reaction is a chemical reaction that occurs when an acid and a base react quantitatively to produce water and salt as products.
• A net ionic equation is a more precise representation of chemical processes that occur in an aqueous solution.

FAQs:

1. What is the net ionic reaction for the neutralization reaction between an acid and a base?

When a strong acid, as well as a strong base, are combined, they react using the net-ionic equation below:

2. Which is the net ionic equation for the neutralization reaction of a strong acid with a weak base?

When a weak base and a strong acid are combined, they react as follows:

The pH of the resultant solution may be estimated by studying the equilibrium interaction of HB with water if the acid and base are equimolar.

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