Silver nitrate has a lattice energy of -820 kJ/mol and a heat of solution of 22.6 kJ/mol. Calculate the heat of hydration for silver nitrate.

Video transcript

hey everyone in this example we need to calculate entropy of hydration. For sodium hydroxide were given its lattice entropy and the heat of the solution. So what we should recall is the following formula where we have our entropy of our solution equal to the entropy of our salute and then added to that are entropy of hydration of our salute. So what we would find is that also our entropy of our salute is equal to the negative value of the entropy of our lattice. So the prompt gives us the heat of our solution and we would recognize this also as the entropy of our solution. And for our entropy of our salute Above we stated that's equal to the negative value of our entropy of our lattice. So we would have negative one times negative 887.0 Kayla jewels per mole. Because the prompt gives us our entropy of our lattice here as negative 887 And so negative one times this negative value gives us an entropy of our salute equal to positive 887. Kayla jewels per So we're going to reorganize our formula above To solve for the entropy of our hydration of our salute. And this is going to equal the difference between the entropy of our solution which above we stated is negative 44.51 kg joules per mole from the prompt subtracted from Our entropy of our salute which we stated above is 887.0 kg joules per mole. And this difference here gives us our entropy of hydration of our salute, sodium hydroxide equal to a value of negative 931.5 kg jewels per mole. So this would be our final answer here for the entropy of hydration for sodium hydroxide. So I hope that everything I went through was clear. If you have any questions, please leave them down below and I will see everyone in the next practice video.