Calcium hypochlorite ( ca(ocl)2ca(ocl)2 , mw = 142.983 g/mol) is often used as the source of the hypochlorite ion ( ocl−ocl− , mw = 51.452 g/mol) in solutions used for water treatment. a student must prepare 50.0 ml of a 20.020.0 ppm ocl−ocl− solution from solid ca(ocl)2ca(ocl)2 , which has a purity of 92.092.0 %. calculate the mass of the impure reagent required to prepare the solution. assume the density of the solution is 1.00 g/ml.

it have destructive character

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

it takes on an electronical energy