Concentrated aqueous sulphuric acid is 98 pure by mass and has a density of 1.84g/cm. What volume of sulphuric acid is required to make 5l of 0.5m of sulphuric acid ?
Answers
Answered by
4
Answer:
Explanation:
Mass = 98
Density = 1.84g/cm
M1 = density × 10 × % by mass / atomic mass
Thus,
M1 = 98×1.80×10 / 98 = 18
Number of moles = Given mass/ mass = 98/98 = 1 mole
Calculating the volume of solution -
Density = Mass/Volume
Volume = Mass/density
V = 100/1.80 = 0.55g
According to the neutralization law - M1V1 = M2V2
where M1=18, M2=0.1, V2=1L
So, V1= M2V2 / M1
V1 = 0.1×1 /18 (1L=1000ml)
= 5.5ml
Similar questions