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can help with chem?

B

Beige

Senior member
A 3.50g sample of solid Mg(OH)2 was treated with 50.0 ml of 0.500 molar H2SO4. After the reaction was over, some of the Mg(OH)2 remained undisolved. Calculate how many g of solid Mg(OH)2 would have remained.

I forgot how to set it up 🙁...
 
Probably easiest to convert everything to moles, then using the balanced equation find out how much excess Mg(OH)2 remains. I.e. how much Mg(OH)2 do you need exactly to react with the amount of H2SO4, and subtract that value from the amount of Mg(OH)2 you have
 
Originally posted by: EarthwormJim
Probably easiest to convert everything to moles, then using the balanced equation find out how much excess Mg(OH)2 remains. I.e. how much Mg(OH)2 do you need exactly to react with the amount of H2SO4, and subtract that value from the amount of Mg(OH)2 you have
Click to expand...

yep, convert everything to moles, assume the reaction goes to completion and it should be pretty straightforward.
 
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