What mass of CuSO4 are needed to prepare 100 mL of a 0.10 M solution? grams
1 answer:
1.596 grams is the mass of CuSO4 needed to prepare 100 ml solution of 0.1 M solution.
Explanation:
Data given:
Volume of the solution = 100 ml or 0.1 litre
molarity of the solution = 0.10 M
mass of CuS = ?
atomic mass of CuS = 159.6 grams/mole
The mass will calculated by using the following relations:
number of moles = equation 1
molarity = equation 2
putting the value of number of moles in equation 2
molarity =
mass = molarity x atomic mass x volume
mass = 0.1 x 0.1 x 159.6
= 1.596 grams
1.596 grams will form 100ml solution 0.1 M
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Answer:
Here's what I get
Explanation:
(a) Intermediates
The three structures below represent one contributor to the resonance-stabilized intermediate, in which the lone pair electrons on the heteroatom are participating (the + charge on the heteroatoms do not show up very well).
(b) Relative Stabilities
The relative stabilities decrease in the order shown.
N is more basic than O, so NH₂ is the best electron donating group (EDG) and will best stabilize the positive charge in the ring. However, the lone pair electrons on the N in acetanilide are also involved in resonance with the carbonyl group, so they are not as available for stabilization of the ring.
(c) Relative reactivities
The relative reactivities would be
C₆H₅-NH₂ > C₆H₅-OCH₃ > C₆H₅-NHCOCH₃
