Chemical reaction between sodium chloride and silver nitrate solutions, demonstrating mass conservation with a white precipitate formation.

Problem Analysis:

The question describes a chemical reaction between sodium chloride (NaCl) solution and silver nitrate (AgNO₃) solution. This is a classic example of a precipitation reaction, where an insoluble compound forms as a result of the reaction.

#### Given Information:
- Sodium chloride (NaCl) solution is mixed with silver nitrate (AgNO₃) solution.
- The reaction is carried out in a test tube, and the mass before and after the reaction is measured using a balance.
- Initial mass: 300.23 g
- Final mass: 300.23 g

Solution to Each Part:

#### a) What change did you observe? Or Define the reaction?
When sodium chloride (NaCl) reacts with silver nitrate (AgNO₃), a white precipitate forms immediately. This is because silver chloride (AgCl) is insoluble in water and precipitates out of the solution. The reaction is a double-displacement reaction, where the cations and anions switch places to form new compounds.

Observation: A white precipitate forms in the solution.

---

#### b) Which insoluble substance is formed?
The insoluble substance formed in this reaction is silver chloride (AgCl). Silver chloride is a white, solid compound that is not soluble in water.

Answer: Silver chloride (AgCl)

---

#### c) Is there any change in the weight?
From the given information, the initial mass of the system (before the reaction) is 300.23 g, and the final mass (after the reaction) is also 300.23 g. There is no change in the total mass of the system.

Answer: No, there is no change in the weight.

---

#### d) Which law followed by the reaction?
The reaction follows the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. The total mass of the reactants must equal the total mass of the products.

Answer: Law of conservation of mass

---

#### e) State the law of conservation of mass
The law of conservation of mass states that in a closed system, the total mass of the substances before a chemical reaction is equal to the total mass of the substances after the reaction. In other words, mass is neither created nor destroyed during a chemical reaction.

Answer: The total mass of the reactants equals the total mass of the products.

---

#### f) What are the product(s) of the reaction?
The products of the reaction between sodium chloride (NaCl) and silver nitrate (AgNO₃) are:
1. Silver chloride (AgCl): An insoluble white precipitate.
2. Sodium nitrate (NaNO₃): A soluble salt that remains in the solution.

Answer: Silver chloride (AgCl) and sodium nitrate (NaNO₃)

---

#### g) Write the chemical equation for the reaction?
The balanced chemical equation for the reaction is:

\[
\text{NaCl (aq)} + \text{AgNO}_3 (\text{aq}) \rightarrow \text{AgCl (s)} \downarrow + \text{NaNO}_3 (\text{aq})
\]

Here:
- NaCl (aq): Sodium chloride (aqueous)
- AgNO₃ (aq): Silver nitrate (aqueous)
- AgCl (s): Silver chloride (solid, precipitate)
- NaNO₃ (aq): Sodium nitrate (aqueous)

---

#### h) Did the reaction result in the white precipitate as a product?
Yes, the reaction resulted in the formation of a white precipitate, which is silver chloride (AgCl).

Answer: Yes

---

Final Answer:

\[
\boxed{
\begin{array}{ll}
\text{a)} & \text{A white precipitate forms.} \\
\text{b)} & \text{Silver chloride (AgCl)} \\
\text{c)} & \text{No change in weight.} \\
\text{d)} & \text{Law of conservation of mass} \\
\text{e)} & \text{Mass is conserved; total mass of reactants = total mass of products.} \\
\text{f)} & \text{Silver chloride (AgCl) and sodium nitrate (NaNO₃)} \\
\text{g)} & \text{NaCl (aq) + AgNO₃ (aq) → AgCl (s) ↓ + NaNO₃ (aq)} \\
\text{h)} & \text{Yes, the reaction resulted in a white precipitate.}
\end{array}
}
\]