The amount of anhydrous Na2CO3 present in
250 ml of 0.25 M solution is
(1) 6.225 g
(3) 6.0 g
(2) 66.25 g
(4) 6.625 g
Answers
Answered by
2
Answer:
option C is correct
Explanation:
M= mole of solute/volume of solution ×1000
0.25 =no. of mole of solute/ 250× 1000
no. of mole of solute = o.625
molar mass of Na2CO3= 106g
mole=given mass /molar mass
given mass=mole × molar mass
given mass = o.625 ×106
given mass = 66.25
Answered by
0
Answer:
M=no. of moles of solute /vol. of solution in lt*1000
no. of moles of solute =wt/molar mass
let wt =X, molar mass =106
no of moles of solute =x/106
molarity =0.25
vol. of solution =250
M=x*1000/Molar mass *vol. of solution
0.25=x*1000/106*250
x=1000/0.25*250*106
x= 8
amount of anhydrous =8
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