Question

Write a chemical equation to show the neutralization of nitric acid (HNO \(_{3}\) ) by strontium hydroxide ( \(\mathrm{Sr}(\mathrm{OH})_{2}\) ).

Short answer

The balanced chemical equation for the neutralization of nitric acid by strontium hydroxide is 2HNO_{3} + Sr(OH)_{2} -> Sr(NO3)_{2} + 2H2O.

Step-by-step solution

Identify the reactants

The first step is to identify the reactants in the neutralization reaction which are nitric acid (HNO_{3}) and strontium hydroxide (Sr(OH)_{2}).

Write the unbalanced chemical equation

Next, write the chemical formula for the reaction with the reactants on the left side and the products, which are water (H2O) and a salt, on the right side. The salt formed here is strontium nitrate (Sr(NO3)_{2}). The unbalanced chemical equation is: HNO_{3} + Sr(OH)_{2} -> Sr(NO3)_{2} + H2O.

Balance the chemical equation

Now count the number of atoms of each element on both sides of the equation and add coefficients to balance the equation. The balanced equation is: 2HNO_{3} + Sr(OH)_{2} -> Sr(NO3)_{2} + 2H2O.

Key concepts

Chemical Equation Balancing

Understanding how to balance chemical equations is a fundamental skill in chemistry and is crucial in accurately representing a chemical reaction. In a balanced chemical equation, the number of atoms of each element must be the same on both sides of the equation. This respects the Law of Conservation of Mass, which states that in a closed system, mass is neither created nor destroyed during a chemical reaction.

To balance an equation, you'll often start by listing the number of atoms of each element in the reactants and products. Then, adjust coefficients—these are the numbers placed before the chemical formulas—to ensure that the same number of atoms for each element appears on both sides. For instance, in the reaction between nitric acid and strontium hydroxide, we look at the elements hydrogen (H), nitrogen (N), oxygen (O), and strontium (Sr) and adjust the coefficients to balance the reaction. It's important not to change the chemical formulas of the reactants or products themselves. Balancing becomes easier with practice, and soon enough, spotting which coefficients to change becomes more intuitive.

Nitric Acid and Strontium Hydroxide Reaction

The reaction between nitric acid (HNO_{3}) and strontium hydroxide (Sr(OH)_{2}) is a specific type of acid-base reaction where an acid reacts with a base to form water and a salt. Nitric acid is a strong acid well-known for its reactivity and corrosive nature, while strontium hydroxide is a strong base, making them quite reactive when combined.

During this reaction, the hydrogen ions (H+) from nitric acid combine with the hydroxide ions (OH-) from strontium hydroxide, resulting in the formation of water (H_{2}O). The remaining ions, strontium (Sr^{2+}) and nitrate (NO_{3}^-), associate to form the salt strontium nitrate (Sr(NO_{3})_{2}). This reaction is exothermic, releasing energy in the form of heat. Furthermore, knowing the specific reactants in this reaction allows us to predict the products and balance the equation accordingly.

Formation of Water and Salt in Neutralization

Neutralization reactions are a subset of acid-base reactions where an acid reacts with a base to produce water and a salt. This is described by the general equation: Acid + Base → Salt + Water. The concept of neutralization is important because it is a powerful tool in many practical applications, such as titration in laboratories, antacid formulations, and wastewater treatment.

In the context of the reaction between nitric acid and strontium hydroxide, the acid (nitric acid) and base (strontium hydroxide) react to neutralize each other. The OH- ions from the base react with the H+ ions from the acid to form water (H2O), one of the hallmarks of a neutralization reaction. Meanwhile, the other ions from the acid and base combine to form a salt, which, in this case, is strontium nitrate (Sr(NO3)_2). The neutrality of the reaction refers to the resulting salt solution, which typically has a pH closer to 7, depending on the strength of the reactants.