Initial Conditions:
- Temperature of the iron ball = 40°C
- Temperature of the water in the container = 46°C

Explanation:
When the 40°C iron ball is dropped into the container with water at 46°C, heat transfer will occur between the iron ball and the water until they reach thermal equilibrium. This means that the heat energy will flow from the hotter object (water at 46°C) to the cooler object (iron ball at 40°C) until they both reach the same temperature.

Heat Transfer:
- The heat from the water will transfer to the iron ball, causing the iron ball to heat up.
- At the same time, the water will lose heat energy and start to cool down.

Final Temperature Calculation:
- To calculate the final temperature of the container, we can use the principle of conservation of energy. The heat gained by the iron ball is equal to the heat lost by the water.
- The formula for heat transfer is: Q = mcΔT, where Q is the heat transferred, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
- By equating the heat gained and lost, we can calculate the final temperature of the container.

Final Temperature:
- By calculating the final temperature using the principle of conservation of energy, we find that the final temperature of the container will be approximately 43°C.
Therefore, the temperature of the container after the iron ball is dropped into the water at 46°C is 43°C. Heat transfer between the iron ball and the water results in the final equilibrium temperature.