Write the balanced K, and K, reactions for HSo, in K.:

A solution is formed from dissolving 1 mole of Al(NO3)3 into enough water to have a total volume of 1 liter. The heat of the solution from this dissolution process was found to be 175 kJ/mol. if the lattice energy for the aluminum nitrate is 5960 kJ/mol in the heat of the hydration for the aluminum (III) cation is -4606 kJ/mol What is the heat of hydration for the nitrate ion in kJ/mol?

An instant cold pack purchased in a pharmacy contains a packet of solid ammonium nitrate surrounded by a pouch of water. When the packet of NH4NO3 is broken, the solid dissolves in water and cooling of the mixture occurs because the solution process for NH4NO3 is endothermic. Explain, in terms of what happens to the molecules and ions, why this mixing occurs spontaneously. Select all that apply. In solution, the ions NH4* and NO3 are highly ordered throughout the solvent. In the solid, the ions in NH4NO3 are highly ordered. In solution, the ions NH4+ and NO3 are randomly distributed throughout the solvent. The increase in randomness makes the process spontaneous. The decrease in randomness makes the process spontaneous.

4. An experiment is to be performed to determine the standard molar enthalpy of neutralization of a  strong acid by a strong base. Standard school laboratory equipment and a supply of standardized 1.00  mol/L HCl and standardized 1.00 mol/L NaOH are available.   a. What equipment would be needed? List them. b. What measurements should be taken? List them.  c. Without performing calculations, briefly describe how the resulting data should be used to  obtain the standard molar enthalpy of neutralization.  d. When a class of students performed this experiment, the average of the results was -55.0  kJ/mol. The accepted value for the standard molar enthalpy of neutralization of a strong acid by  a strong base is -57.7 kilojoules per mole. Briefly describe two likely sources of experimental error that could account for the result  obtained by the class. Mistakes, blunders, or miscalculations are not types of experimental error.

21.1 g of magnesium metal is burned in air to produce magnesium oxide, which is then dissolved in 1.89 L of water to produce a basic solution. What concentration of hydroxide is present in the solution?

Ko is related to Ko by the equation K, = Kc (RT)An, What is the value of An for the reaction below? N2 (g) + 3H2 (g)= 2NH3 (g)

7. NaCl(ag) +

Calculate the pH for 0.0150 M H₂CrO solution. For H₂CRO4, Ka, is very large and Kais 3.10 x 10³. 2 4

Calculate the heat of reaction per mole of water if addition of 25.0 mL of 0.101 M A H2SO4 to 50.0 mL of 0.103 M NaOH causes the temperature to rise by 0.99°C. Assume that for both solutions the density is 1.00 g/mol and the specific heat (s) = 4.184 J/g°C. %3D

Consider an unknown solution. Experimental work determined that the aqueous solution contained some intact molecule as well as product ions. When exposed to red cabbage juice the solution turned bluish-green. Choose all molecules that align with the experimental results. O NaOH O Ca(OH), O NH, O HCH,O2 OH,PO D HCl O HNO,