15 Aug, 2024
· Chemistry

Balanced reaction, ionic equation, net ionic equation for HNO3(aq)+CsOH(aq)

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Long Explanation

Explanation

Balanced Reaction

The balanced chemical reaction for the combination of nitric acid (HNO3\mathrm{HNO_3}) and cesium hydroxide (CsOH\mathrm{CsOH}) can be written as:

HNO3(aq)+CsOH(aq)→CsNO3(aq)+H2O(l)\mathrm{HNO_3(aq) + CsOH(aq) \rightarrow CsNO_3(aq) + H_2O(l)}

Ionic Equation

In the ionic equation, we express all strong electrolytes as ions:

H+(aq)+NO3−(aq)+Cs+(aq)+OH−(aq)→\mathrm{H^+(aq) + NO_3^-(aq) + Cs^+(aq) + OH^-(aq)} \rightarrow →Cs+(aq)+NO3−(aq)+H2O(l)\rightarrow \mathrm{Cs^+(aq) + NO_3^-(aq) + H_2O(l)}

Net Ionic Equation

For the net ionic equation, we eliminate the spectator ions (ions that appear on both sides of the equation):

H+(aq)+OH−(aq)→H2O(l)\mathrm{H^+(aq) + OH^-(aq) \rightarrow H_2O(l)}

Key Points:

  • The balanced reaction shows the full molecular forms of the reactants and products.
  • The ionic equation displays all strong electrolytes dissociated into ions.
  • The net ionic equation simplifies this by removing ions that do not participate directly in the reaction, focusing only on the substances that change during the reaction.

This results in the final, simplified equation which highlights the neutralization process where hydrogen ions (H+\mathrm{H^+}) react with hydroxide ions (OH−\mathrm{OH^-}) to form water (H2O\mathrm{H_2O}).

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Johnathan Clark

Chemistry Content Writer at Math AI

Johnathan Clark, with a Master's in Chemistry from the University of São Paulo, is a young high school chemistry teacher and part-time contract writer. His engaging classroom experiments translate into compelling written content that makes chemistry exciting and practical.

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Concept

Balanced Chemical Equation Representation

Balanced chemical equation representation

In chemistry, a balanced chemical equation is a symbolic representation of a chemical reaction where the number of atoms for each element is the same on both the reactant and product sides. This balance adheres to the Law of Conservation of Mass, which states that matter cannot be created or destroyed in a chemical reaction.

How to balance a chemical equation

  1. Write the unbalanced equation: Begin by writing the skeleton equation with the correct formulas for the reactants and products.

  2. Count the atoms of each element: Tally the number of atoms for each element in the reactants and products.

  3. Use coefficients to balance the atoms: Adjust the coefficients (numbers placed before the chemical formulas) to balance the atoms for each element on both sides.

  4. Check your work: Ensure that the total number of each type of atom is the same on both sides of the equation.

Example

Consider the reaction where hydrogen gas reacts with oxygen gas to form water:

Unbalanced:H2+O2→H2O\text{Unbalanced:} \quad \text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O}

Counting the atoms, we have:

  • Reactants: 2 Hydrogen (H), 2 Oxygen (O)
  • Products: 2 Hydrogen (H), 1 Oxygen (O)

To balance the oxygen atoms, we adjust the coefficients:

H2+O2→2H2O\text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O}

Now we have:

  • Reactants: 2 Hydrogen (H), 2 Oxygen (O)
  • Products: 4 Hydrogen (H), 2 Oxygen (O)

Therefore, we need to adjust the coefficient for H2\text{H}_2:

2H2+O2→2H2O2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O}

Now the equation is balanced:

  • Reactants: 4 Hydrogen (H), 2 Oxygen (O)
  • Products: 4 Hydrogen (H), 2 Oxygen (O)

Important considerations

  • Subscripts vs. Coefficients: Only adjust coefficients to balance an equation, not the subscripts within a chemical formula.
  • Polyatomic Ions: If a reaction involves polyatomic ions that remain unchanged on both sides of the equation, you can balance them as a unit.

Conclusion

Balancing chemical equations ensures that the law of conservation of mass is obeyed and that the theoretical stoichiometry (proportions of reactants and products) is correct. It is a foundational concept in stoichiometry and is essential for accurately describing chemical reactions.

Concept

Ionic Dissociation For Strong Electrolytes

Explanation

Ionic dissociation is a process in which an ionic compound separates into its individual ions when it dissolves in a solvent, typically water. This occurs because the polar nature of water molecules interacts with the ions, breaking the ionic bonds and allowing the ions to disperse throughout the solution.

Strong Electrolytes

A strong electrolyte is a substance that completely dissociates into its ions when dissolved in a solvent. Strong electrolytes include strong acids, strong bases, and most salts. Because they fully dissociate, they conduct electricity very well in solution.

Dissociation Equation

When a strong electrolyte dissolves in water, it breaks apart completely into its constituent ions. For example, consider the dissociation of sodium chloride (NaCl) in water:

NaCl(s)→Na+(aq)+Cl−(aq)\text{NaCl}(s) \rightarrow \text{Na}^{+}(aq) + \text{Cl}^{-}(aq)

General Form of Dissociation

For a generic strong electrolyte AB, the dissociation in water is represented as:

AB(s)→A+(aq)+B−(aq)\begin{equation*} \text{AB}(s) \rightarrow \text{A}^{+}(aq) + \text{B}^{-}(aq) \end{equation*}

Important Characteristics

  • Complete Dissociation: Strong electrolytes dissociate nearly 100% in a solution.
  • Electrical Conductivity: Due to the presence of free-moving ions, solutions of strong electrolytes are excellent conductors of electricity.
  • Examples:
    • Strong Acids: HCl, HNO₃, H₂SO₄
    • Strong Bases: NaOH, KOH
    • Salts: NaCl, KBr

Applications

Understanding ionic dissociation for strong electrolytes is crucial in fields such as:

  • Electrochemistry: Studying how ions interact and facilitate electrical conduction.
  • Medicine: Electrolyte balance and management in bodily fluids.
  • Industrial chemistry: Processes like electroplating and battery design.

By grasping this concept, we can better predict and manipulate the behavior of ionic compounds in various chemical and biological systems.