What volume of concentrated aquies sulphuric acid which is 98% H2SO4by mass and has density of 1.84gml-1 is required to prepare 10lof 0.2m.H2SO4 solution
Answers
Answer:
Volume of acid required to make one litre of 0.1M H_2SO_4H2SO4
solution is 5.5 ml.
Explanation: Given: H_2SO_4H2SO4 is labelled as 98% by weight means 98 gram of H_2SO_4H2SO4 is dissolved in 100 g of solution.
To calculate the moles, we use the equation:
Density of solution= 1.80 g/ml
Now we have to calculate the volume of solution.
Density=\frac{Mass}{Volume}Density=Volume Mass
Volume=\frac{mass}{Density}=\frac{100g}{1.80g/ml}==55.5mlVolume=
Density mass = 1.80g/ml 100g =55.5ml
Molarity : It is defined as the number of moles of solute present per liter of the solution.
Formula used :
Molarity=\frac{n\times 1000}{V_s}Molarity= Vs n×1000
where,
n= moles of solute
V_sV s = volume of solution in ml
Molarity=\frac{1\times 1000}{55.5ml}=18M
Molarity= 55.5ml 1×1000 =18M
According to the neutralization law,
M_1V_1=M_2V_2M1
V1 =M2
V2 18\times V_2= 0.1\times 1000ml18×V2 =0.1×1000ml.....(1L=1000ml)
V_2=5.5mlV2 =5.5ml