100ml H2SO4 solution having molarity 1M and density 1.5g/ml is mixed with 400ml of water. Calculate final molarity of H2SO4 solution, if final density is 1.25g/ml.
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first, make sure you have a good grasp of the definition of molarity
well i know how to solve the question but i think the question is wrong
Not the answer you are looking for? Search for more explanations.
well then type the correct question
then show your solution
ok 1st i'll show the solution and then i'll show how the question is wrong
for h2so4 :- 1M=n(moles)/0.1
total weight of final solution = 100 x 1.5 +400 = 550gm
volume of final solution = 550/1.25 = 440ml = 0.440L
molarity of h2so4 in final solution = 0.1/0.440 = 0.227M
it is given that the final density is 1.25g/ml
the final mix has h2so4 and h2o
total mass of final mixture as calculated above is = 550gm
total volume of final mix. = vol. of h2so4 + vol. of h2o = 100+400 = 500
so final density of final solution = mass/volume = 550/500 = 1.1gm/ml but in the question the final density given is 1.25gm/ml now how is that possible??
when you dilute a solution, does the density increase or decrease?
prove it mathematically
well i don't know how to do so??
can you use the density formula?
the way i showed that the final density is 1.1 is also correct.
@hwyl how will you prove that density is not 1.1 and its 1.25??
You are meant to calculate the concentration of H2SO4 and then to use that to find the final density of the solution and CHECK that it is 1.25.
Conentration = molarity
@ShizukaTheOtaku no we don't have to check whether the density given is correct or not rather we are given the density to find the molarity. But i wished to check whether the density given was correct or not and in the calculation above which i posted the density is comming out to be different from what is given in the question.