Titration question help
1. 100 cm3 of concentrated hydrochloric acid was diluted accurately to 1000 cm3 with distilled water. The diluted acid was titrated against 25.0 cm3 of 0.5 mol dm-3 sodium carbonate, which required 27.2 cm3 of acid for neutralisation, using methyl orange indicator. What was the concentration of the original acid?
4. When 0.203 g of hydrated magnesium chloride, MgClm.xH2O, was dissolved in water and titrated with 0.100 mol dm-3 silver nitrate (AgNO3) solution, 20.0 cm3 of the latter were required. A sample of the hydrated chloride lost 53.2% of its mass when heated in a stream of hydrogen chloride, leaving a residue of anhydrous magnesium chloride. From these figures, calculate the values of m and x.
[Hint: Ignore the water of crystallisation (xH2O) when considering the titration data]
Any help with these two questions would be very much appreciated! Thank you!
4. When 0.203 g of hydrated magnesium chloride, MgClm.xH2O, was dissolved in water and titrated with 0.100 mol dm-3 silver nitrate (AgNO3) solution, 20.0 cm3 of the latter were required. A sample of the hydrated chloride lost 53.2% of its mass when heated in a stream of hydrogen chloride, leaving a residue of anhydrous magnesium chloride. From these figures, calculate the values of m and x.
[Hint: Ignore the water of crystallisation (xH2O) when considering the titration data]
Any help with these two questions would be very much appreciated! Thank you!
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4. When 0.203 g of hydrated magnesium chloride, MgClm.xH2O, was dissolved in water and titrated with 0.100 mol dm-3 silver nitrate (AgNO3) solution, 20.0 cm3 of the latter were required. A sample of the hydrated chloride lost 53.2% of its mass when heated in a stream of hydrogen chloride, leaving a residue of anhydrous magnesium chloride. From these figures, calculate the values of m and x.
A sample (0.203 g) of hydrated magnesium chloride (MgClm.nH2O) was dissolved in water and titrated with silver nitrate solution (0.100 mol dm-3), 20.0 cm3 being required. Another sample of the hydrated chloride lost 53.2 % of its mass when heated in a stream of hydrogen chloride, leaving aresidue of anhydrous magnesium chloride. Calculate the values of m and n
Original post by nushhi
A sample (0.203 g) of hydrated magnesium chloride (MgClm.nH2O) was dissolved in water and titrated with silver nitrate solution (0.100 mol dm-3), 20.0 cm3 being required. Another sample of the hydrated chloride lost 53.2 % of its mass when heated in a stream of hydrogen chloride, leaving a residue of anhydrous magnesium chloride. Calculate the values of m and n
PART 1
When the sample of hydrated magnesium chloride dissolves in water all of the chloride ions are then released into solution.
MgClm.nH2O ==> Mg2+(aq) + mCl-(aq)
Silver ions react in a 1:1 ratio with chloride ions.
Hence mol silver ions = mol chloride ions.
PART 2
Moles of water = mass loss/Mr(water)
Can you try it now?
(edited 1 year ago)
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