In this exercise, you will calculate molar value of ΔH (in kJ/mol) for dissolving NH4H2PO4 in Part D of the Calorimetry lab. What temperature change did you find for dissolving NH4H2PO4 in Part D of the experiment? (Include the + or - sign in your answer.)

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)