Grade 11General Physics
100 ml of 50% w/w HCL (aq) solutions.Density 1.46 g/ml is mixed with 100 ml of water calculate Molarity.
100 ml of 50% w/w HCL (aq) solutions.Density 1.46 g/ml is mixed with 100 ml of water calculate Molarity.
2 Answers
Norman Manchu
Approved Tutor Answer8 Years agoMolarity of mixture of two or more components is given by-
For calculating M1 which is the molarity of HCl we can use the formula-
Where x is percent weight and rho indicates density
M1=2x10^-1
Molarity of water is calculated by n(water)/V Thus-M2=5x10^-2
The total molarity can hence be calculated and the final answer would be 125x10^-3Molar
Kapil Hitesh Gupta
This problem is a classical problem of dilution(as it involves decrease in conc. of sol. or change in volume due to only increase in volume of solvent).
So, there is a general and intuitive concept in dilution that Moles of solute before dilution = Moles of solute before dilution
This is so as in dilution we have two ways to dilute the solution:
1. Decrease the solute
2. Increase the volume of solution/solvent(while solute is const.)
In 99.99% cases we go with 2nd method as its practically way more easier than 1
Here's how we approach the answer to problem
Before this, formulas you need to know M= nsolute/Volume of solution(L)
i.e., n =M×Vol.
According to the concept M1V1=M2V2
M1= Molarity of solution before
M2= Molarity of solution after
V1= Volume of solution before
V2= Volume of solution after
Mass of solution = 100 × 1.46 = 146 g (m= density×volume.)
As 50% (W/W) solution 73 g HCl and 73 g H2O
So, n solute = 73/36.5 = 2
M1 = 2/0.1L=20M and V1=100ml, V2=200(100ml sol.+ 100ml added water
M1V1=M2V2
20×100ml = M2×200ml
M2= 10M
Therfore the molariy of solution after dilution with 100ml water is 10 molar/M
NOTE: Be careful with the answers you see as the other answer provided is wrong(Though I'm not an IITian but I can clearly tell right and wrong)
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