2. An almond weighs 0.823 grams. When the almond is burned in a calorimeter that co 124.2 grams of water, the water temperature changes from 23.5 °C to 45.7 °C. The water MSDT "uncombusted remains" of the almond weighs 0.615 grams. Q: amount of heat absorbed by liquid iwater a) Calculate the change in temperature (AT) of the water. 2 m: mass of liquid water s specific heat of liquid water AT: Change in temper" 5.7°C-235%= 22.2°C b) Calculate the amount of energy that was released from the almond sample. Assume that all of the energy released from the almond was transferred to the water. M:R42 Use the specific heat (S) of water (1.000 cal/g °C), the mass of the water that was in watters: the flask, and the temperature change (AT) of the water to calculate the amount of energy (0) that was transferred to the water, and thus the amount of energy that was Qalmond-q water released from almond. Cal 2g x1.000 9°C X22.2°C ● =2757.21 cal =1-2757 cal amount of heat released from almond is 2757 calories =2757.24 cal c) Calculate the mass of the almond that was "completely combusted". This is done by subtracting the mass of "uncombusted remains" of the almond from the original mass of the almond. Massot uncombusted of almond: 0.615- Original mass of almond; 0.8239 Mass of completely combusted of almond: 0.8239-0.6159

A chemistry student weighs out 0.112 g of formic acid (HCHO2) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0800M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits.

A chemist makes 410. mL of magnesium fluoride (MgF₂) working solution by adding distilled water to 280. mL of a mol 0.00188 stock solution of magnesium fluoride in water. L Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits. mol L X 5 F 00 18 Ar

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