When 50.0 mL of 0.400 M Ca(NO₃)₂ is added to 50.0 mL of 0.800 M NaF,CaF₂ precipitates,as shown in the net ionic equation below.The initial temperature of both solutions is 25.00°C.Assuming that the reaction goes to completion,and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C),calculate the final temperature of the solution. Ca²⁺(aq)+ 2 F^-(aq)→ CaF₂(s)ΔH° = -11.5 kJ A)24.45°C B)25.55°C C)26.10°C D)26.65°C

Question

Quizplus · Accepted Answer

The reaction releases heat (exothermic, ΔH° = -11.5 kJ), which increases the temperature of the solution. The heat released is calculated using the moles of CaF2 formed and ΔH°. The temperature change is then found using q = mcΔT.

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