Chapter 5: Problem 75
Aqueous solutions of sodium sulfate and lead(II) nitrate are mixed and a white solid forms. Identify the solid.
Short Answer
Expert verified
The white solid formed in the reaction is lead(II) Sulfate (\(PbSO4\)).
Step by step solution
01
Write Down the Initial Reactants
Write down the reaction between sodium sulfate \(Na2SO4\) and lead (II) nitrate \(Pb(NO3)2\). The reaction in the aqueous solution will be: \(Na2SO4(aq) + Pb(NO3)2(aq) \to ?\). The question mark indicates that we'll be identifying the products of this reaction.
02
Predict the Exchange Products
Sodium sulfate and lead(II) nitrate are both salts and will dissociate into their ions in solution. The sulphate ion from sodium sulfate will combine with the lead ion from lead nitrate, and the nitrate ion from lead nitrate will combine with the sodium ion from sodium sulfate. This will form two potential exchange products: sodium nitrate (NaNO3) and lead(II) sulfate (PbSO4). Therefore, the predicted reaction becomes: \(Na2SO4(aq) + Pb(NO3)2(aq) \to NaNO3(aq) + PbSO4(s)\). However, we need to balance the chemical reaction.
03
Balance the Chemical Reaction
Balance the chemical reaction so that there are equal numbers of each type of atom on each side of the equation. In this case, a balanced equation would be: \(Na2SO4(aq) + Pb(NO3)2(aq) \to 2NaNO3(aq) + PbSO4(s)\).
04
Identifying the Solid Precipitate
Given that a white solid forms, the solid is likely the result of one product being insoluble in water. According to the solubility rules, most nitrate salts are soluble, so sodium nitrate would stay dissociated in the solution. However, most sulphate salts are soluble, except for those with barium, lead and calcium. Therefore, the white precipitate is lead (II) sulphate (PbSO4).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Solubility Rules
Understanding solubility rules is crucial when predicting the outcome of a chemical reaction, particularly when dealing with aqueous solutions. Solubility rules give chemists a systematic way to know which compounds will dissolve in water (soluble) and which will form precipitates (insoluble).
For instance, there are general patterns like all nitrates (\(NO_3^-\)) are soluble, and most sulfates (\(SO_4^{2-}\)) are soluble with notable exceptions including barium sulfate (\(BaSO_4\)), calcium sulfate (\(CaSO_4\)), and notably for our example, lead(II) sulfate (\(PbSO_4\)). Knowing these rules helps predict that when aqueous solutions of sodium sulfate (\(Na_2SO_4\)) and lead(II) nitrate (\(Pb(NO_3)_2\)) are mixed, the lead(II) sulfate is the component that forms a solid precipitate due to its low solubility in water.
To enhance student understanding, incorporating visual aids like solubility charts or flow diagrams can be extremely helpful. Additionally, emphasizing the practical use of these rules in pollution controls, medication formulation, and chemical syntheses could further pique student interest.
For instance, there are general patterns like all nitrates (\(NO_3^-\)) are soluble, and most sulfates (\(SO_4^{2-}\)) are soluble with notable exceptions including barium sulfate (\(BaSO_4\)), calcium sulfate (\(CaSO_4\)), and notably for our example, lead(II) sulfate (\(PbSO_4\)). Knowing these rules helps predict that when aqueous solutions of sodium sulfate (\(Na_2SO_4\)) and lead(II) nitrate (\(Pb(NO_3)_2\)) are mixed, the lead(II) sulfate is the component that forms a solid precipitate due to its low solubility in water.
To enhance student understanding, incorporating visual aids like solubility charts or flow diagrams can be extremely helpful. Additionally, emphasizing the practical use of these rules in pollution controls, medication formulation, and chemical syntheses could further pique student interest.
Chemical Reaction Balancing
Balancing chemical reactions is a basic yet vital skill in chemistry, ensuring that the law of conservation of mass is observed. This principle states that mass cannot be created or destroyed in a chemical reaction, therefore the number of atoms of each element must be the same on both sides of the equation.
Let's take the example from our exercise: we start with the unbalanced equation for the reaction between sodium sulfate (\(Na_2SO_4\)) and lead(II) nitrate (\(Pb(NO_3)_2\)). To balance it, we make sure that there are equal numbers of sodium, lead, nitrogen, and oxygen atoms on both the reactant and product sides. After balancing, we arrive at a complete reaction: \[Na_2SO_4(aq) + Pb(NO_3)_2(aq) \to 2NaNO_3(aq) + PbSO_4(s)\]^1.
Teaching tip: Students often find balancing equations challenging, so breaking down the process into manageable steps is essential. Encourage students to start with the most complex molecule and to only change coefficients, not subscripts. A handy exercise is to balance equations with progressively increasing complexity, offering frequent practice and reinforcement of the concept.
Let's take the example from our exercise: we start with the unbalanced equation for the reaction between sodium sulfate (\(Na_2SO_4\)) and lead(II) nitrate (\(Pb(NO_3)_2\)). To balance it, we make sure that there are equal numbers of sodium, lead, nitrogen, and oxygen atoms on both the reactant and product sides. After balancing, we arrive at a complete reaction: \[Na_2SO_4(aq) + Pb(NO_3)_2(aq) \to 2NaNO_3(aq) + PbSO_4(s)\]^1.
Teaching tip: Students often find balancing equations challenging, so breaking down the process into manageable steps is essential. Encourage students to start with the most complex molecule and to only change coefficients, not subscripts. A handy exercise is to balance equations with progressively increasing complexity, offering frequent practice and reinforcement of the concept.
Double Displacement Reaction
A double displacement reaction, also known as a metathesis reaction, involves the exchange of parts between two compounds. In an aqueous solution, the cations and anions of two different compounds switch places, forming two new compounds. One of these is typically a precipitate, a gas, or a weakly dissociating compound like water.
In our example, sodium sulfate (\(Na_2SO_4\)) and lead(II) nitrate (\(Pb(NO_3)_2\)) undergo a double displacement reaction to produce sodium nitrate (\(NaNO_3\)) and lead(II) sulfate (\(PbSO_4\)), with the latter being the precipitate due to its low solubility. This type of reaction is not only significant in scientific studies but also has practical applications in wastewater treatment, where it can be used to remove contaminants.
For improvement in understanding, students should be encouraged to write out the full ionic equations and to study the physical states of the reactants and products. Hands-on laboratory experiments and simulations can greatly help deepen the comprehension of the double displacement mechanism and outcome.
In our example, sodium sulfate (\(Na_2SO_4\)) and lead(II) nitrate (\(Pb(NO_3)_2\)) undergo a double displacement reaction to produce sodium nitrate (\(NaNO_3\)) and lead(II) sulfate (\(PbSO_4\)), with the latter being the precipitate due to its low solubility. This type of reaction is not only significant in scientific studies but also has practical applications in wastewater treatment, where it can be used to remove contaminants.
For improvement in understanding, students should be encouraged to write out the full ionic equations and to study the physical states of the reactants and products. Hands-on laboratory experiments and simulations can greatly help deepen the comprehension of the double displacement mechanism and outcome.
