Final answer:
The final temperature of a mixture of two solutions of different temperatures can only be estimated without knowing the volumes and specific heat capacities of the solutions. If mixed in equal parts, it would be between 40 °C and 45 °C. For the exact final temperature, one must apply the principle of thermal equilibrium and the formula q = mcΔT.
Step-by-step explanation:
When two solutions of different temperatures are mixed together, the final temperature of the mixture can be estimated by assuming that the solutions will reach thermal equilibrium. This concept is part of thermodynamics, a branch of physics. If no heat is lost to the surroundings, the mixture will reach an intermediate temperature that is dependent on the initial temperatures and quantities of the solutions involved. However, without information on the quantities (volumes) and the specific heat capacities of the solutions, we cannot calculate the exact final temperature. It is important to note that if we are mixing equal parts of the two solutions, the final temperature will be between 40 °C and 45 °C. If the solutions are mixed in different proportions, then the final temperature could lean closer to the temperature of the larger quantity. To solve these types of problems, one typically uses the formula q = mcΔT, where q is the heat energy transferred, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.