Pre-lab Questions:
- A double replacement reaction takes place between two ionic compounds that are dissolved in an aqueous solution and form two new compounds. An example of one is when Sodium phosphate and silver nitrate combine to yield sodium nitrate and silver phosphate. The algebraic equation for this would be Na3PO4 (aq) + 3 AgNO3 (aq) → 3 NaNO3 (aq) + Ag3PO4 (s).
2. A color change, the formation of a precipitate or the production of gas or water are the types of evidence that indicate a double replacement reaction has occurred between the aqueous ionic compounds.
3. In this investigation, the type of evidence specifically being looked for is the formation of a precipitate.
4. Silver nitrate is a toxic, and can cause stains to the skin and clothing. When performing this lab, the participant should wear goggles and a lab apron at all times. During the investigation all the chemicals should be handled with care to avoid spills and contact with skin.
5. Here are the elements of group 1A: hydrogen, lithium, sodium, potassium, rubidium, cesium, and francium.
6. An aqueous ion is an element that is soluble in water.
Post-lab Questions: Critical Thinking
Analysis and Conclusions:
1. The combination of solutions in B2, B4, C2, and C4 as shown in the prediction data table did not perform a precipitate. According to our observation table, all the products of these no reactions were soluble in water. The products were
2. Based on the observations the positive ion of silver (Ag) reacted to form the greatest number of precipitates. This is true because according to the prediction table the silver compounds always produced a precipitate.
Application:
1. AgNO3 + NaCl → AgCl + NaNO3
2. No there will be no reaction. This is because all of the compounds are aqueous meaning no precipitate will be formed, and no gas will be produced. To have a reaction, there has to be a solid forming or a gas producing in the equation.