Chapter 7: Problem 26
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely to occur, so indicate. a. sodium sulfate and potassium chloride b. potassium sulfide and calcium nitrate c. sodium hydroxide and silver nitrate d. sodium carbonate and iron(III) chloride e. ammonium phosphate and aluminum chloride f. barium nitrate and potassium chloride
Short Answer
Expert verified
a. No reaction occurs.
b. \(S^{2-} (aq) + Ca^{2+} (aq) \rightarrow CaS (s)\)
c. \(OH^- (aq) + Ag^+ (aq) \rightarrow AgOH (s)\)
d. \(CO_3^{2-} (aq) + 2 Fe^{3+} (aq) \rightarrow Fe_2(CO_3)_3 (s)\)
e. \(PO_4^{3-} (aq) + Al^{3+} (aq) \rightarrow AlPO_4 (s)\)
f. No reaction occurs.
Step by step solution
01
a. Sodium sulfate and potassium chloride
1. Chemical formulas: Na2SO4 (sodium sulfate) and KCl (potassium chloride)
2. Possible products: NaCl (sodium chloride) and K2SO4 (potassium sulfate)
3. Balanced molecular equation: Na2SO4 (aq) + 2 KCl (aq) -> 2 NaCl (aq) + K2SO4 (aq)
4. Balanced ionic equation: 2 Na^+ (aq) + SO4^2- (aq) + 2 K^+ (aq) + 2 Cl^- (aq) -> 2 Na^+ (aq) + 2 Cl^- (aq) + 2 K^+ (aq) + SO4^2- (aq)
5. Spectator ions: Na^+, K^+, Cl^-, SO4^2-
No reaction occurs.
02
b. Potassium sulfide and calcium nitrate
1. Chemical formulas: K2S (potassium sulfide) and Ca(NO3)2 (calcium nitrate)
2. Possible products: KNO3 (potassium nitrate) and CaS (calcium sulfide)
3. Balanced molecular equation: K2S (aq) + Ca(NO3)2 (aq) -> 2 KNO3 (aq) + CaS (s)
4. Balanced ionic equation: 2 K^+ (aq) + S^2- (aq) + Ca^2+ (aq) + 2 NO3^- (aq) -> 2 K^+ (aq) + 2 NO3^- (aq) + CaS (s)
5. Spectator ions: K^+, NO3^-
6. Balanced net ionic equation: S^2- (aq) + Ca^2+ (aq) -> CaS (s)
03
c. Sodium hydroxide and silver nitrate
1. Chemical formulas: NaOH (sodium hydroxide) and AgNO3 (silver nitrate)
2. Possible products: NaNO3 (sodium nitrate) and AgOH (silver hydroxide)
3. Balanced molecular equation: NaOH (aq) + AgNO3 (aq) -> NaNO3 (aq) + AgOH (s)
4. Balanced ionic equation: Na^+ (aq) + OH^- (aq) + Ag^+ (aq) + NO3^- (aq) -> Na^+ (aq) + NO3^- (aq) + AgOH (s)
5. Spectator ions: Na^+, NO3^-
6. Balanced net ionic equation: OH^- (aq) + Ag^+ (aq) -> AgOH (s)
04
d. Sodium carbonate and iron(III) chloride
1. Chemical formulas: Na2CO3 (sodium carbonate) and FeCl3 (iron(III) chloride)
2. Possible products: NaCl (sodium chloride) and Fe2(CO3)3 (iron(III) carbonate)
3. Balanced molecular equation: Na2CO3 (aq) + 2 FeCl3 (aq) -> 6 NaCl (aq) + Fe2(CO3)3 (s)
4. Balanced ionic equation: 2 Na^+ (aq) + CO3^2- (aq) + 2 Fe^3+ (aq) + 6 Cl^- (aq) -> 6 Na^+ (aq) + 6 Cl^- (aq) + Fe2(CO3)3 (s)
5. Spectator ions: Na^+, Cl^-
6. Balanced net ionic equation: CO3^2- (aq) + 2 Fe^3+ (aq) -> Fe2(CO3)3 (s)
05
e. Ammonium phosphate and aluminum chloride
1. Chemical formulas: (NH4)3PO4 (ammonium phosphate) and AlCl3 (aluminum chloride)
2. Possible products: NH4Cl (ammonium chloride) and AlPO4 (aluminum phosphate)
3. Balanced molecular equation: (NH4)3PO4 (aq) + AlCl3 (aq) -> 3 NH4Cl (aq) + AlPO4 (s)
4. Balanced ionic equation: 3 NH4^+ (aq) + PO4^3- (aq) + Al^3+ (aq) + 3 Cl^- (aq) -> 3 NH4^+ (aq) + 3 Cl^- (aq) + AlPO4 (s)
5. Spectator ions: NH4^+, Cl^-
6. Balanced net ionic equation: PO4^3- (aq) + Al^3+ (aq) -> AlPO4 (s)
06
f. Barium nitrate and potassium chloride
1. Chemical formulas: Ba(NO3)2 (barium nitrate) and KCl (potassium chloride)
2. Possible products: BaCl2 (barium chloride) and KNO3 (potassium nitrate)
3. Balanced molecular equation: Ba(NO3)2 (aq) + 2 KCl (aq) -> BaCl2 (aq) + 2 KNO3 (aq)
4. Balanced ionic equation: Ba^2+ (aq) + 2 NO3^- (aq) + 2 K^+ (aq) + 2 Cl^- (aq) -> Ba^2+ (aq) + 2 Cl^- (aq) + 2 K^+ (aq) + 2 NO3^- (aq)
5. Spectator ions: Ba^2+, K^+, Cl^-, NO3^-
No reaction occurs.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Balanced Chemical Equations
Balanced chemical equations are crucial for representing chemical reactions accurately. They ensure that the number of atoms for each element is the same on both sides of the equation, adhering to the Law of Conservation of Mass.
This law states that mass cannot be created or destroyed in a chemical reaction, which means all atoms must be accounted for.
For example, when sodium sulfate (\[ \text{Na}_2\text{SO}_4 \]) reacts with potassium chloride (\[ \text{KCl} \]), the balanced equation is:
\[ \text{Na}_2\text{SO}_4 \text{(aq)} + 2 \text{KCl} \text{(aq)} \rightarrow 2 \text{NaCl} \text{(aq)} + \text{K}_2\text{SO}_4 \text{(aq)} \] This indicates that in the reaction, all sodium, sulfate, potassium, and chloride ions are properly balanced.
Balancing chemical equations involves adjusting the number of coefficients (the numbers placed in front of compounds) so that the types and numbers of atoms are the same on each side. Always start with the most complex compound, and balance elements one at a time. Remember, the goal is to have equal numbers of each type of atom on both sides of the "reaction arrow".
This law states that mass cannot be created or destroyed in a chemical reaction, which means all atoms must be accounted for.
For example, when sodium sulfate (\[ \text{Na}_2\text{SO}_4 \]) reacts with potassium chloride (\[ \text{KCl} \]), the balanced equation is:
\[ \text{Na}_2\text{SO}_4 \text{(aq)} + 2 \text{KCl} \text{(aq)} \rightarrow 2 \text{NaCl} \text{(aq)} + \text{K}_2\text{SO}_4 \text{(aq)} \] This indicates that in the reaction, all sodium, sulfate, potassium, and chloride ions are properly balanced.
Balancing chemical equations involves adjusting the number of coefficients (the numbers placed in front of compounds) so that the types and numbers of atoms are the same on each side. Always start with the most complex compound, and balance elements one at a time. Remember, the goal is to have equal numbers of each type of atom on both sides of the "reaction arrow".
Spectator Ions
Spectator ions are ions that exist in the same form on both the reactant and product sides of a chemical equation.
They do not participate directly in the chemical reaction but are there to keep the system neutral and balanced.
Identifying these ions is essential for simplifying equations into net ionic equations, which highlight the reaction's active components.
For instance, in the reaction of sodium sulfate with potassium chloride, the balanced ionic equation is:
\[ 2 \text{Na}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} + 2 \text{K}^+ \text{(aq)} + 2 \text{Cl}^- \text{(aq)} \rightarrow 2 \text{Na}^+ \text{(aq)} + 2 \text{Cl}^- \text{(aq)} + 2 \text{K}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \] The spectator ions in this case are \(\text{Na}^+, \text{K}^+, \text{Cl}^-,\) and \(\text{SO}_4^{2-}\). By removing these ions from both sides, we can see that no reaction occurs, as the net ionic equation would be void.
They do not participate directly in the chemical reaction but are there to keep the system neutral and balanced.
Identifying these ions is essential for simplifying equations into net ionic equations, which highlight the reaction's active components.
For instance, in the reaction of sodium sulfate with potassium chloride, the balanced ionic equation is:
\[ 2 \text{Na}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} + 2 \text{K}^+ \text{(aq)} + 2 \text{Cl}^- \text{(aq)} \rightarrow 2 \text{Na}^+ \text{(aq)} + 2 \text{Cl}^- \text{(aq)} + 2 \text{K}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \] The spectator ions in this case are \(\text{Na}^+, \text{K}^+, \text{Cl}^-,\) and \(\text{SO}_4^{2-}\). By removing these ions from both sides, we can see that no reaction occurs, as the net ionic equation would be void.
Aqueous Solutions
Aqueous solutions are solutions where the solvent is water, and they are an important aspect of many chemical reactions dealt with in chemistry.
When dealing with aqueous solutions, it's crucial to understand that solutes are dissolved in water and usually dissociate into ions.
This dissociation is what allows many reactions to occur, especially those involving ionic compounds.
For example, when sodium sulfate and potassium chloride are mixed in water, they separate into their respective ions:
- Sodium sulfate: \[ \text{Na}_2\text{SO}_4 \text{(aq)} \rightarrow 2 \text{Na}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \]- Potassium chloride: \[ \text{KCl} \text{(aq)} \rightarrow \text{K}^+ \text{(aq)} + \text{Cl}^- \text{(aq)} \] This ion separation allows reactions to take place between the different ions when solutions are mixed.
When dealing with aqueous solutions, it's crucial to understand that solutes are dissolved in water and usually dissociate into ions.
This dissociation is what allows many reactions to occur, especially those involving ionic compounds.
For example, when sodium sulfate and potassium chloride are mixed in water, they separate into their respective ions:
- Sodium sulfate: \[ \text{Na}_2\text{SO}_4 \text{(aq)} \rightarrow 2 \text{Na}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \]- Potassium chloride: \[ \text{KCl} \text{(aq)} \rightarrow \text{K}^+ \text{(aq)} + \text{Cl}^- \text{(aq)} \] This ion separation allows reactions to take place between the different ions when solutions are mixed.
Chemical Reactions
Chemical reactions involve the interaction of substances to form new substances, often with unique properties. They can be categorized into various types like synthesis, decomposition, single replacement, double replacement, and combustion.
In aqueous solutions, reactions often involve the exchange of ions, leading to the formation of new compounds.
For example, the double replacement reaction of potassium sulfide with calcium nitrate is represented by the balanced equation:
\[ \text{K}_2\text{S} \text{(aq)} + \text{Ca(NO}_3\text{)}_2 \text{(aq)} \rightarrow 2 \text{KNO}_3 \text{(aq)} + \text{CaS} \text{(s)} \] In this example, calcium sulfide, which forms a solid precipitate (\(\text{CaS} \text{(s)} \)), is a new product indicating a chemical change has occurred.
When writing chemical equations, after predicting products, always confirm by checking the states of the products and if a reaction indeed takes place, as highlighted in the net ionic equations.
In aqueous solutions, reactions often involve the exchange of ions, leading to the formation of new compounds.
For example, the double replacement reaction of potassium sulfide with calcium nitrate is represented by the balanced equation:
\[ \text{K}_2\text{S} \text{(aq)} + \text{Ca(NO}_3\text{)}_2 \text{(aq)} \rightarrow 2 \text{KNO}_3 \text{(aq)} + \text{CaS} \text{(s)} \] In this example, calcium sulfide, which forms a solid precipitate (\(\text{CaS} \text{(s)} \)), is a new product indicating a chemical change has occurred.
When writing chemical equations, after predicting products, always confirm by checking the states of the products and if a reaction indeed takes place, as highlighted in the net ionic equations.
Reaction Products
Reaction products are the new substances formed as a result of a chemical reaction. In chemical equations, these are located on the right side of the reaction arrow.
Identifying the products of a reaction helps in understanding both the process and the usefulness of the reaction in practical applications.
In a reaction between sodium hydroxide and silver nitrate, the products are sodium nitrate and silver hydroxide. The equation:
\[ \text{NaOH} \text{(aq)} + \text{AgNO}_3 \text{(aq)} \rightarrow \text{NaNO}_3 \text{(aq)} + \text{AgOH} \text{(s)} \] Silver hydroxide (\(\text{AgOH} \text{(s)} \)) forms as a solid, which shows that a significant chemical reaction has occurred since this compound precipitates out of solution.
When predicting reaction products, consider the solubility rules and reactivity series, as these can influence whether a reaction will take place or what form the products will take.
Identifying the products of a reaction helps in understanding both the process and the usefulness of the reaction in practical applications.
In a reaction between sodium hydroxide and silver nitrate, the products are sodium nitrate and silver hydroxide. The equation:
\[ \text{NaOH} \text{(aq)} + \text{AgNO}_3 \text{(aq)} \rightarrow \text{NaNO}_3 \text{(aq)} + \text{AgOH} \text{(s)} \] Silver hydroxide (\(\text{AgOH} \text{(s)} \)) forms as a solid, which shows that a significant chemical reaction has occurred since this compound precipitates out of solution.
When predicting reaction products, consider the solubility rules and reactivity series, as these can influence whether a reaction will take place or what form the products will take.
