Question
Calculate (a) the moles and (b) the mass of magnesium carbonate at the start if 0.2 moles of sulfuric acid is added to the magnesium carbonate and the excess sulfuric acid made up to a 250 cm3 solution. 25 cm3 of this solution required 0.03 moles of sodium hydroxide for neutralisation.
MgCO3 + H2SO4 ¨ MgSO4 + H2O + CO2 H2SO4 + 2
NaOH ¨ NaCl + H2O
MgCO3 + H2SO4 ¨ MgSO4 + H2O + CO2 H2SO4 + 2
NaOH ¨ NaCl + H2O
Answers
the actual mass (g) = Number of moles x Molar mass,
or m = n x M
Number of moles of solute = Concentration (mol. L) x Volume of solution (liters) -1
or n = C x V
or m = n x M
Number of moles of solute = Concentration (mol. L) x Volume of solution (liters) -1
or n = C x V
The question is wrong by the way, the product of H2SO4 reacting with 2 NaOH should be Na2SO4 + 2 H2O
Related Questions
in a soda-acid fire extinguisher, concentrateed sulfuric acid reacts with sodium hydrogen carbonate...
500.0 g of ammonia react with 51.0 moles of sulfuric acid to produce ammonium sulfate. How many mole...
calculate the moles of sulfuric acid that remained in the solution after reaction with the carbonate...
In a soda acid fire extinguisher, concentrated sulfuric acid reacts with sodium hydrogen carbonate t...