2 L of an unknown concentration of the weak base ammonia are standardized. 50.0 mL of the basic solution are titrated with 0.200 M HCl. The end point occurs after 86.8 mL of acid are added. What is the concentration of ammonia in the 2 L flask

i'm not sure

explanation:

i'll try whatever you got

"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"