In a calorimeter, 300 mL of 0.22 mol/L of calcium chloride is mixed with 200 mL of 0.33 mol/L of sodium phosphate. The initial temperature of the two solutions is 15.00°C. After mixing, the final temperature is 19.75°C. The density of the aqueous solutions is 1.02 g/mL, and its specific heat capacity is equal to that of water. Calculate the molar enthalpy of solution for NaCl. (7 T) *Hint: you need to write a balanced chemical equation first

For the molecule shown below, provide the names for all of the indicated functional groups: O 3 1 aspirin 1. Functional group 1: 2. Functional group 2: 3. Functional group 3: 2 OH;

A 100.0 mL sample of 0.250 M NaOH is mixed with a 150.0 mL sample of 0.280 M HNO3 in a coffee cup calorimeter.  Both solutions were initially at 35.00°C and after mixing, the temperature of the resulting solution was recorded as 37.00°C. Determine the enthalpy of neutralization (ΔH°neutralization rxn) (in units of kJ/mol) for the neutralization reaction between aqueous NaOH and HNO3.  The specific heat capacity of water = 4.184 J/g°C and density of water = 1.00 g/mL Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.    Hint: Heat of neutralization is the enthalpy change per mol of water formed in a neutralization reaction. Write the balanced equation, calculate the limiting reactant and the mol of water formed in the reaction. Enter the numerical value clearly indicating whether it is endothermic or exothermic.

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