what volume of 0.1moldm^3 solution of tetraoxosulphate(vi)acid would be needed to dissolve 2.86g of sodium...

what volume of 0.1moldm^3 solution of tetraoxosulphate(vi)acid would be needed to dissolve 2.86g of sodium trioxocarbonate(iv)DECA hydrate crystal?

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Answers (2)

GDMGT
1 month ago
Solution:
Equation of reaction:
H2SO4 + Na2CO3.10H2O = Na2SO4 + 11H2O +CO2
From this we see that 1 mole of tetraoxosulphate(vi)acid (H2SO4) dissolves 1 mole of sodiumtrioxocarbonate(iv)DECA hydrate crystal Na2CO3.10H2O.
Molar masses of elements:
H = 1, C = 12, O = 16, Na = 23 and S = 32.
Step 1: Find how many moles are in 2.86g of sodiumtrioxocarbonate(iv)DECA hydrate crystal.
solution:
number of moles = mass/molarmass of compound,
molar mass of compound = (2*23) + 12 + (3*16) + 10(2+16) = 46 + 12 + 48 + 180 = 286g mass = 2.86g
number of moles = 2.86/286 = 0.01 moles.
Since 1 mole of tetraoxosulphate(vi)acid dissolves 1 mole of sodiumtrioxocarbonate(iv)DECA hydrate crystal then 0.01 moles of sodiumtrioxocarbonate(iv)DECA hydrate crystal will also be dissolved by 0.01 moles of tetraoxosulphate(vi)acid.
Step 2: find volume of the acidic solution needed for dissolving crystal
Solution: volume = number of moles/ concentration of tetraoxosulphate(vi)acid = 0.01/0.1=0.1
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