Question

Write equations showing the ions present after the following strong electrolytes are dissolved in water. a. \(\mathrm{HNO}_{3}\) f. \(\mathrm{NH}_{4} \mathrm{Br}\) b. \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) g. \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) h. \(\mathrm{CuSO}_{4}\) d. \(\mathrm{SrBr}_{2}\) i. \(\mathrm{NaOH}\) e. \(\mathrm{KClO}_{4}\)

Short answer

The ions present after the strong electrolytes are dissolved in water are: a. \(\mathrm{HNO}_{3} \rightarrow \mathrm{H}^{+} + \mathrm{NO}_{3}^{-}\) f. \(\mathrm{NH}_{4} \mathrm{Br} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{Br}^{-}\) b. \(\mathrm{Na}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{Na}^{+} + \mathrm{SO}_{4}^{2-}\) g. \(\mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{NO}_{3}^{-}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} \rightarrow \mathrm{Al}^{3+} + 3 \mathrm{NO}_{3}^{-}\) h. \(\mathrm{CuSO}_{4} \rightarrow \mathrm{Cu}^{2+} + \mathrm{SO}_{4}^{2-}\) d. \(\mathrm{SrBr}_{2} \rightarrow \mathrm{Sr}^{2+} + 2 \mathrm{Br}^{-}\) i. \(\mathrm{NaOH} \rightarrow \mathrm{Na}^{+} + \mathrm{OH}^{-}\) e. \(\mathrm{KClO}_{4} \rightarrow \mathrm{K}^{+} + \mathrm{ClO}_{4}^{-}\)

Step-by-step solution

Write the dissociation reaction

When \(\mathrm{HNO}_{3}\) dissolves in water, it dissociates into its ions: a hydrogen ion (H+) and a nitrate ion (NO3-). The reaction can be written as: \[\mathrm{HNO}_{3} \rightarrow \mathrm{H}^{+} + \mathrm{NO}_{3}^{-}\] #f. \(\mathrm{NH}_{4} \mathrm{Br}\)#

Write the dissociation reaction

When \(\mathrm{NH}_{4} \mathrm{Br}\) dissolves in water, it dissociates into ammonium ion (NH4+) and a bromide ion (Br-). The reaction can be written as: \[\mathrm{NH}_{4} \mathrm{Br} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{Br}^{-}\] #b. \(\mathrm{Na}_{2} \mathrm{SO}_{4}\)#

Write the dissociation reaction

When \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) dissolves in water, it dissociates into 2 sodium ions (Na+) and a sulfate ion (SO4^2-). The reaction can be written as: \[\mathrm{Na}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{Na}^{+} + \mathrm{SO}_{4}^{2-}\] #g. \(\mathrm{NH}_{4} \mathrm{NO}_{3}\)#

Write the dissociation reaction

When \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) dissolves in water, it dissociates into ammonium ion (NH4+) and a nitrate ion (NO3-). The reaction can be written as: \[\mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{NO}_{3}^{-}\] #c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\)#

Write the dissociation reaction

When \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) dissolves in water, it dissociates into an aluminum ion (Al3+) and 3 nitrate ions (NO3-). The reaction can be written as: \[\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} \rightarrow \mathrm{Al}^{3+} + 3 \mathrm{NO}_{3}^{-}\] #h. \(\mathrm{CuSO}_{4}\)#

Write the dissociation reaction

When \(\mathrm{CuSO}_{4}\) dissolves in water, it dissociates into a copper ion (Cu2+) and a sulfate ion (SO4^2-). The reaction can be written as: \[\mathrm{CuSO}_{4} \rightarrow \mathrm{Cu}^{2+} + \mathrm{SO}_{4}^{2-}\] #d. \(\mathrm{SrBr}_{2}\)#

Write the dissociation reaction

When \(\mathrm{SrBr}_{2}\) dissolves in water, it dissociates into a strontium ion (Sr2+) and 2 bromide ions (Br-). The reaction can be written as: \[\mathrm{SrBr}_{2} \rightarrow \mathrm{Sr}^{2+} + 2 \mathrm{Br}^{-}\] #i. \(\mathrm{NaOH}\)#

Write the dissociation reaction

When \(\mathrm{NaOH}\) dissolves in water, it dissociates into a sodium ion (Na+) and a hydroxide ion (OH-). The reaction can be written as: \[\mathrm{NaOH} \rightarrow \mathrm{Na}^{+} + \mathrm{OH}^{-}\] #e. \(\mathrm{KClO}_{4}\)#

Write the dissociation reaction

When \(\mathrm{KClO}_{4}\) dissolves in water, it dissociates into a potassium ion (K+) and a perchlorate ion (ClO4-). The reaction can be written as: \[\mathrm{KClO}_{4} \rightarrow \mathrm{K}^{+} + \mathrm{ClO}_{4}^{-}\]

Key concepts

Strong Electrolytes

Strong electrolytes are substances that completely dissociate into ions when they dissolve in water. This means they break down entirely into their constituent ions, making them excellent conductors of electricity in aqueous solutions. Examples of strong electrolytes include strong acids like nitric acid \((\mathrm{HNO}_{3})\) and strong bases such as sodium hydroxide \((\mathrm{NaOH})\), as well as various salts.Understanding strong electrolytes is crucial because they are often involved in various chemical processes and reactions. When they dissolve, they produce ions that participate in electrical conduction and chemical reactions:

• This property is why solutions of strong electrolytes are frequently used in batteries, electrolysis, and other electrical applications.
• Identifying strong electrolytes helps predict the outcomes of chemical reactions, especially in predicting precipitate formation or gas evolution.

To recognize strong electrolytes in a chemical equation, observe if the compounds dissociate completely in water. This total dissociation enables free-moving ions, resulting in high conductivity.

Aqueous Solution

An aqueous solution is a solution in which water is the solvent. In chemical reactions, aqueous solutions are frequently used because water's properties as a solvent make it ideal for dissolving a wide range of substances, particularly ionic compounds.The significance of aqueous solutions includes:

• Water's polar nature enables it to dissolve many compounds, making aqueous solutions the most common reaction medium in chemistry.
• In aqueous solutions, solute particles are uniformly dispersed, allowing for consistent reaction conditions and product formation.

When ions like \(\mathrm{Na^+}\), \(\mathrm{NH_4^+}\), \(\mathrm{NO_3^-}\), and \(\mathrm{ClO_4^-}\) are mentioned in dissociation reactions, they are in aqueous form. This means they are surrounded and stabilized by a shell of water molecules.Effective dissolving is crucial for certain calculations and applications, including titrations, where precise reaction amounts are needed. Thus, understanding the properties of water as a solvent is fundamental when dealing with aqueous solutions.

Chemical Reactions

In chemistry, reactions involve the transformation of substances through the breaking and forming of bonds. Chemical reactions in aqueous solutions often provide insight into the behavior of reactants when dissolved in water.Key aspects of chemical reactions include:

• In the context of ionic dissociation, these reactions can show what ions are formed and how they interact.
• An example is when \(\mathrm{CuSO_4}\) dissociates in water to form copper ions \((\mathrm{Cu^{2+}})\) and sulfate ions \((\mathrm{SO_4^{2-}})\).
• This ionic interaction in aqueous solutions is essential for predicting the formation of precipitates, gases, or conducting successful titrations.

Reactants and products in chemical equations can be affected by their forms in aqueous solutions. It is crucial to balance these equations to accurately represent the conservation of mass and charge.With chemical reactions in solutions, particularly with strong electrolytes, reaching a state of equilibrium or completion can depend significantly on how the ions interact and dissociate. Recognizing these interactions aids in predicting the pathway and outcome of the reactions in practical applications.