Chapter 14: Problem 45
Predict the products of each reaction. (a) \(\mathrm{HClO}_{4}(a q)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Sr}(\mathrm{s}) \longrightarrow\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{KOH}(a q) \longrightarrow\)
Short Answer
Expert verified
The products are: (a) Iron(III) perchlorate and water, (b) Strontium sulfate and hydrogen gas, (c) Potassium phosphate and water.
Step by step solution
01
Inspect the first reaction - HClO4 and Fe2O3
Consider the reactivity and solubility of reactants. HClO4 is a strong acid, and Fe2O3 is a metal oxide which typically reacts with strong acids to form a salt and water. Therefore, HClO4 will react with Fe2O3 to form iron(III) perchlorate (Fe(ClO4)3) and water (H2O).
02
Write the balanced equation for the first reaction
Balance the chemical equation by ensuring that the number of atoms of each element on the reactant side is equal to the number on the product side. The equation becomes: \(3 \mathrm{HClO}_{4}(aq) + \mathrm{Fe}_{2}\mathrm{O}_{3}(s) \longrightarrow 2 \mathrm{Fe(ClO_{4})}_{3}(aq) + 3 \mathrm{H}_2\mathrm{O}(l)\).
03
Inspect the second reaction - H2SO4 and Sr
Looking at the reactants, H2SO4 is a strong acid and Sr is a reactive metal. Such a metal will typically react with strong acids to form a salt and hydrogen gas. In this case, strontium sulfate (SrSO4) and hydrogen gas (H2) will be produced.
04
Write the balanced equation for the second reaction
The reaction between H2SO4 and Sr must be balanced to comply with the Law of Conservation of Mass. The balanced chemical equation is: \(\mathrm{H}_{2}\mathrm{SO}_{4}(aq) + \mathrm{Sr}(s) \longrightarrow \mathrm{SrSO}_{4}(s) + \mathrm{H}_2(g)\).
05
Inspect the third reaction - H3PO4 and KOH
Given that H3PO4 is a weak acid and KOH is a strong base, they will react to form a salt and water in a neutralization reaction. The products will be potassium phosphate (K3PO4) and water (H2O).
06
Write the balanced equation for the third reaction
In order to balance the neutralization reaction, coefficients must be adjusted so the number of each type of atom, as well as charge, is the same on both sides. The balanced equation is: \(\mathrm{H}_{3}\mathrm{PO}_{4}(aq) + 3 \mathrm{KOH}(aq) \longrightarrow \mathrm{K}_3\mathrm{PO}_{4}(aq) + 3\mathrm{H}_2\mathrm{O}(l)\).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chemical Equation Balancing
Understanding the principle of chemical equation balancing is crucial for studying chemistry. It's a fundamental skill that ensures the Law of Conservation of Mass is obeyed in every chemical reaction. This law states that mass is neither created nor destroyed in a chemical reaction, which means all atoms present in the reactants must be accounted for in the products.
To balance a chemical equation, start by writing down the unbalanced equation. Then, systematically adjust the coefficients—the numbers placed before chemical formulas—to achieve the same number of each type of atom on both sides of the equation. It's akin to solving a puzzle, ensuring that each move keeps the whole picture intact.
For example, looking at the provided exercise, the reaction between HClO4 and Fe2O3 had to be balanced by making sure the iron, chlorine, oxygen, and hydrogen atoms were equal on both sides. This was achieved by adjusting coefficients to balance the charges and the atoms, leading to a balanced equation that reflects the mass conservation.
To balance a chemical equation, start by writing down the unbalanced equation. Then, systematically adjust the coefficients—the numbers placed before chemical formulas—to achieve the same number of each type of atom on both sides of the equation. It's akin to solving a puzzle, ensuring that each move keeps the whole picture intact.
For example, looking at the provided exercise, the reaction between HClO4 and Fe2O3 had to be balanced by making sure the iron, chlorine, oxygen, and hydrogen atoms were equal on both sides. This was achieved by adjusting coefficients to balance the charges and the atoms, leading to a balanced equation that reflects the mass conservation.
Acid-Base Neutralization Reactions
Acid-base neutralization reactions are a particular type of chemical reaction where an acid reacts with a base to form a salt and usually water. These reactions are pivotal for many everyday processes, from digestion in our bodies to environmental applications like neutralizing acid rain.
In a neutralization reaction, the hydrogen ions (H+) from the acid combine with the hydroxide ions (OH−) from the base to produce water (H2O). The remaining ions from the acid and base form a salt. For instance, as seen in the case of H3PO4 reacting with KOH, the result is potassium phosphate (K3PO4) and water.
Neutralization reactions are also a great example of double replacement reactions, where the constituent ions switch partners. These reactions require careful balancing to ensure that the final equation is accurate, consistent with stoichiometry, and obeys the conservation of mass and charge principles.
In a neutralization reaction, the hydrogen ions (H+) from the acid combine with the hydroxide ions (OH−) from the base to produce water (H2O). The remaining ions from the acid and base form a salt. For instance, as seen in the case of H3PO4 reacting with KOH, the result is potassium phosphate (K3PO4) and water.
Neutralization reactions are also a great example of double replacement reactions, where the constituent ions switch partners. These reactions require careful balancing to ensure that the final equation is accurate, consistent with stoichiometry, and obeys the conservation of mass and charge principles.
Reaction Between Acids and Metals
Interactions between acids and metals can be quite dynamic and are another class of reactions important for students to understand. When an acid reacts with a metal, the outcome is typically a salt plus hydrogen gas. This type of reaction can be vigorous, as metal atoms release electrons to the hydrogen ions from the acid, producing H2 gas.
In the given problem set, strontium, a reactive metal, is combined with sulfuric acid. The reaction produces strontium sulfate and hydrogen gas. Metals that are above hydrogen in the reactivity series can displace hydrogen from acids, with the reactivity of the metal often indicating the vigor of the reaction. Metals lower in the series don't react as violently, and some, like gold and platinum, do not react at all under normal conditions.
It's essential for students to observe and understand the patterns of reactivity and be able to predict the products of such reactions by considering the reactivity of the metal and the strength of the acid involved.
In the given problem set, strontium, a reactive metal, is combined with sulfuric acid. The reaction produces strontium sulfate and hydrogen gas. Metals that are above hydrogen in the reactivity series can displace hydrogen from acids, with the reactivity of the metal often indicating the vigor of the reaction. Metals lower in the series don't react as violently, and some, like gold and platinum, do not react at all under normal conditions.
It's essential for students to observe and understand the patterns of reactivity and be able to predict the products of such reactions by considering the reactivity of the metal and the strength of the acid involved.
Solubility and Reactivity Rules
Solubility and reactivity rules are guidelines that help predict the outcome of chemical reactions, especially with regard to the formation of precipitates (solid products that form in solution). Solubility rules outline which ionic compounds are soluble in water and which are not. If an ionic compound is not soluble, it precipitates out of the solution.
Reactivity rules, on the other hand, provide insight into which elements or compounds are likely to undergo a reaction. For example, the reactivity series of metals can predict whether a metal will displace another in a compound. These rules are incredibly valuable for predicting the products of reactions and understanding the driving forces behind chemical changes.
Applying these rules to the exercises provided, one can predict that iron(III) perchlorate will remain in solution due to the soluble nature of most perchlorates, while strontium sulfate will form a precipitate as it is generally insoluble. Knowing these rules not only helps in predicting the products of reactions but also in understanding why certain reactions occur and others do not.
Reactivity rules, on the other hand, provide insight into which elements or compounds are likely to undergo a reaction. For example, the reactivity series of metals can predict whether a metal will displace another in a compound. These rules are incredibly valuable for predicting the products of reactions and understanding the driving forces behind chemical changes.
Applying these rules to the exercises provided, one can predict that iron(III) perchlorate will remain in solution due to the soluble nature of most perchlorates, while strontium sulfate will form a precipitate as it is generally insoluble. Knowing these rules not only helps in predicting the products of reactions but also in understanding why certain reactions occur and others do not.
