How many mL of 0.650 M solution can be prepared by dissolving 15.0 g of copper(II) nitrate in water?

123.1L

Explanation:

Given parameters:

Molarity of Cu(NO₃)₂  = 0.650M

Mass of  Cu(NO₃)₂ = 15g

Unknown:

Volume of  Cu(NO₃)₂ = ?

Solution:

To solve this problem, we have to first find the number of moles of the given mass;

  Number of moles of Cu(NO₃)₂  =

   Molar mass of Cu(NO₃)₂  = 63.5 + 2 (14 + 3(16)) = 187.5g/mol

 Number of moles of Cu(NO₃)₂  =  = 0.08 mol

Molarity is given as;

  Molarity  =  

         Volume  =  

  Insert the parameters and solve;

        Volume  =  = 0.12L

Now mL;

         1L  = 1000mL

        0.12L will give 1000 x 0.12  = 123.1L

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: