i) molarity of mixer = M1V1+M2V2/V1+V2
= (50*0.025+100*0.15)/150
= 0.1083 M
molarity of Zn^2+ = 0.1083 M
ii)
50 ml = 0.5 dl
150 micrograms = 0.15 mg
concentration of milk = 0.15/0.5 = 0.3 mg/dl
i)
from standard solution
90 grams HNO3 present in 100 grams solution
volume of solution = m/density = 100/1.51 = 66.22 ml
Molarity of standard solution = (90/63)*(1000/66.22) = 21.57 M
dilution formula
M1V1 = M2V2
21.57*V1 = 0.25*500
V1 = 5.8 ml
take 5.8 ml standard solution and add water up to 500 ml
ii)
150 ppm means
150 mg present in 1 liter solution
Molarity of OH- = (0.15/17)*(1/1) = 0.0088 M
1 mol Ba(OH)2 = 2 mol OH-
No of mol of Ba(OH)2 required = 0.0088/2 = 0.0044 mol
mass of Ba(OH)2 MUST DISSOLVE = 0.0044*171.34 = 0.754 grams
Help. Determine the new concentration of Zn^2+ ion in grams per liter after mixing 50 ml...
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