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Concentrated sulfuric acid (18.4 molar) has a density of 11.84 g/ml

Concentrated sulfuric acid (18.4 molar) has a density of 11.84 g per ml
dilution with water to 5.20 molar, density of 1.38 g per ml
can be used as an a electroyte is lead batterys.

What is the molality of the 5.20 molar H2SO4 solution?

well im not exactly sure where to start, but i know that i need to find moles of solute/kg of solvent. i think i should start with grams in one liter and use that to find the number of grams or moles of solution, but other than that i am pretty lost.

where am i wrong and whats next?
 

Answers and Replies

Borek
Mentor
28,129
2,636
Start with 1L of solution, calculate number of moles of sulfuric acid (easy part), mass of solvent (not that hard - start with mass of solution, subtract mass of sulfuric acid) and you are ready to calculate molality.
<Moderator edited out link: "Cheat sheets" are not an effective method of learning chemistry.>

Borek
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Last edited by a moderator:
can someone give me a lil more help, i understand what borek is saying, but how do i find the mass of the solvent, and what method do i use when given the density
 
Moonbear
Staff Emeritus
Science Advisor
Gold Member
11,349
51
can someone give me a lil more help, i understand what borek is saying, but how do i find the mass of the solvent, and what method do i use when given the density
Do you recall the units for molecular weight and how to determine that using information in the periodic table? You'll need that to help you solve the problem.
 

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