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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 |
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Answer» Volume of ACID required to make one litre of 0.1M H_2SO_4H2SO4solution 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/mlNow we have to calculate the volume of solution.Density=\frac{Mass}{Volume}Density=Volume MassVolume=\frac{mass}{Density}=\frac{100g}{1.80g/ml}==55.5mlVolume=Density mass = 1.80g/ml 100g =55.5mlMolarity : 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×1000where,n= moles of soluteV_sV s = volume of solution in mlMolarity=\frac{1\times 1000}{55.5ml}=18MMolarity= 55.5ml 1×1000 =18MAccording to the neutralization law,M_1V_1=M_2V_2M1V1 =M2V2 18\times V_2= 0.1\times 1000ml18×V2 =0.1×1000ml.....(1L=1000ml)V_2=5.5mlV2 =5.5mlhope it helps plz mark my ANSWER as the brainliestthank you |
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