Question

Write a balanced net ionic equation for the reaction of sulfuric acid with (a) \(\mathrm{CaCO}_{3}(s)\) (b) a solution of \(\mathrm{NaOH}\).

Short answer

Question: Write the balanced net ionic equations for the reaction of sulfuric acid with (a) calcium carbonate and (b) sodium hydroxide. Answer: (a) H2SO4 (aq) + CaCO3 (s) -> CaSO4 (s) + H2O (l) + CO2 (g) (b) H+ (aq) + OH- (aq) -> H2O (l)

Step-by-step solution

(a) Reaction of Sulfuric Acid with Calcium Carbonate

First, write the complete balanced equation for the reaction between sulfuric acid (H2SO4) and calcium carbonate (CaCO3): H2SO4 (aq) + CaCO3 (s) -> CaSO4 (s) + H2O (l) + CO2 (g) Now, identify spectator ions. Since calcium carbonate is a solid and there are no aqueous ions, there are no spectator ions in this reaction. So the net ionic equation remains the same as the complete balanced equation: H2SO4 (aq) + CaCO3 (s) -> CaSO4 (s) + H2O (l) + CO2 (g)

(b) Reaction of Sulfuric Acid with Sodium Hydroxide

First, write the complete balanced equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH): H2SO4 (aq) + 2NaOH (aq) -> Na2SO4 (aq) + 2H2O (l) Now, identify spectator ions. Sodium (Na+) and sulfate (SO4²⁻) ions are spectator ions in this reaction. The net ionic equation will be as follows: 2H+ (aq) + 2OH- (aq) -> 2H2O (l) And after dividing by 2 to simplify: H+ (aq) + OH- (aq) -> H2O (l)

Key concepts

Understanding Chemical Reactions

In the study of chemistry, a chemical reaction is a process where substances, known as reactants, are transformed into different substances called products. These changes involve the breaking and forming of chemical bonds. Chemical reactions are represented by chemical equations that show the reactants and products along with their respective quantities.

When writing chemical equations, it is crucial to ensure the equation is balanced, meaning the number of atoms of each element is the same on both sides of the equation. This abides by the Law of Conservation of Mass, which states that matter is neither created nor destroyed in a chemical reaction.

To better understand these reactions, net ionic equations are used to highlight the actual chemical change without including the spectator ions that do not participate in the reaction. These equations provide clarity on the ions involved in the reaction and can be particularly insightful when dealing with reactions in aqueous solutions.

Diving Into Acid-Base Reactions

An acid-base reaction is a type of chemical reaction that involves the transfer of protons (H+) between a pair of compounds. Acids are species that can donate protons, whereas bases are species that can accept protons. When an acid and base react, they can form water and a salt in a neutralization reaction.

For instance, when sulfuric acid reacts with sodium hydroxide, the hydrogen ions (H+) from the acid combine with the hydroxide ions (OH⁻) from the base to form water (H2O). The ions that remain (sodium and sulfate in this case) typically form a salt, which in our example is sodium sulfate (Na2SO4).

Understanding the concept of acid-base reactions is essential as it not only applies to laboratory experiments but also to many biological processes and industrial applications. When balancing acid-base reactions, it is also important to pay attention to the states of matter of the reactants and products, as demonstrated in the provided exercise.

The Role of Stoichiometry in Chemical Equations

The term stoichiometry is derived from Greek words that essentially mean 'measuring elements'. It involves calculations based on the quantities of reactants and products in a chemical reaction. The principles of stoichiometry are used to predict the amounts of products that will be formed in a reaction from a given amount of reactants or to determine the amount of reactants needed to produce a desired quantity of product.

Stoichiometry is deeply connected to the mole concept which allows chemists to count particles by weighing them. The balanced chemical equations provide the ratio of moles of reactants and products, and this mole ratio is used to carry out stoichiometric calculations. When we refer to balancing the net ionic equation, we're essentially applying the principles of stoichiometry. This highlights the importance of the balanced equation prior to breaking it down into its net ionic form, ensuring the proportionality of reactants and products is retained.

As we improve our understanding of stoichiometry, we unlock the ability to solve complex problems involving mass-to-mass conversions, limiting reactants, and percentage yield, all of which are crucial skills in the field of chemistry.