Original post by nnn121337
Some 1.0 mol dm–3 solutions were mixed using equal volumes of each solution.
Which pair of solutions would give the greatest mass of solid?
A Ba(OH)2 and MgCl2
B Ba(OH)2 and MgSO4
C Ba(OH)2 and NaCl
D Ba(OH)2 and Na2SO4
Which pair of solutions would give the greatest mass of solid?
A Ba(OH)2 and MgCl2
B Ba(OH)2 and MgSO4
C Ba(OH)2 and NaCl
D Ba(OH)2 and Na2SO4
What are you thinking so far?
Reply 2
I am also struggling with this questions right now. I'm thinking the answer would be the compounds with the greatest mr because concentration and volume are the same so the thing that must be different is their moles so as mass=mrxmoles the greatest mr would be the answer but that would give an answer of C.
Original post by lanadelslay1989
I am also struggling with this questions right now. I'm thinking the answer would be the compounds with the greatest mr because concentration and volume are the same so the thing that must be different is their moles so as mass=mrxmoles the greatest mr would be the answer but that would give an answer of C.
You have the molar volume mol/dm³ and you need to convert it to molar mass g/mol and if you got it, you can finally calculate the mass with the molar mass by the help of the known moles of the compounds:
molar mass * moles = mass.
(edited 1 year ago)
Reply 4
Original post by Kallisto
You have the molar volume mol/dm³ and you need to convert it to molar mass g/mol and if you got it, you can finally calculate the mass with the molar mass by the help of the known moles of the compounds:
molar mass * moles = mass.
molar mass * moles = mass.
Original post by Kallisto
You have the molar volume mol/dm³ and you need to convert it to molar mass g/mol and if you got it, you can finally calculate the mass with the molar mass by the help of the known moles of the compounds:
molar mass * moles = mass.
molar mass * moles = mass.
How can you work out the molar mass from mol/dm³? Surely you need the mass and moles to work that out
Reply 6
Original post by Spark321
How can you work out the molar mass from mol/dm³? Surely you need the mass and moles to work that out
You don’t need molar masses or anything. There is no need to calculate anything.
Assume all solutions have the same concentrations and are used in equal volumes in each case.
Think in terms of what reaction takes place in each case and whether the products are soluble in water. Are there any cases where you form two water insoluble products?
(edited 5 months ago)
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