- Messages
- 6
- Reaction score
- 3
- Points
- 13
Problem 1: A saturated aqueous solution of magnesium methanoate, Mg(HCOO)2, has a solubility of approximately 150 g dm-3 at room temperature. Its exact solubility can be determined by titrating magnesium methanote against aqueous potassium manganate (VII).
During the titration, the methanoate ion, HCOO-, is oxidizes to carbon dioxide while the manganate (VII) ion, MnO4-, is reduced to Mn2+.
You are supplied with
A saturated aqueous solution of Mg(HCOO)2
Aqueous potassium manganate (VII), KMnO4, of concentration 0.0200 mol dm-3
(a) (i). write the half equations for the oxidation of HCOO-(aq) to CO2(g) and the reduction of MnO4-(aq) to Mn2+ (aq) in acid solution.
(ii) Using the approximately solubility above, calculate the concentration, in mol dm-3, of the saturated aqueous magnesium methanoate and the concentration of the methanoate ions present in this solution
(Ai: H, 1.0, C, 12.0, O, 16.0, Mg, 24.3)
(iii) In order to obtain a reliable titre value, the saturated solution of magnesium methanoate needs to be diluted.
Describe how you would accurately measure a 5.0cm3 sample of saturated magnesium methanate solution and use it to prepare a solution fifty times more dilute than the saturated solution.
(vi) 1 mol of acidified MnO4- ions reacts with 2.5 mol of HCOO- ions.
25.0 cm3 of the diluted solution prepared in (iii) required 25.5 cm3 of 0.0200 mol dm-3 potassium manganate (VII) solution to reach the end point.
Use this information to calculate the concentration, in mol dm-3, of HCOO- ions in the diluted solution.
(Vii) use your answer to calculate the concentration of the saturated solution of magnesium methanoate
Can someone help me with vii
During the titration, the methanoate ion, HCOO-, is oxidizes to carbon dioxide while the manganate (VII) ion, MnO4-, is reduced to Mn2+.
You are supplied with
A saturated aqueous solution of Mg(HCOO)2
Aqueous potassium manganate (VII), KMnO4, of concentration 0.0200 mol dm-3
(a) (i). write the half equations for the oxidation of HCOO-(aq) to CO2(g) and the reduction of MnO4-(aq) to Mn2+ (aq) in acid solution.
(ii) Using the approximately solubility above, calculate the concentration, in mol dm-3, of the saturated aqueous magnesium methanoate and the concentration of the methanoate ions present in this solution
(Ai: H, 1.0, C, 12.0, O, 16.0, Mg, 24.3)
(iii) In order to obtain a reliable titre value, the saturated solution of magnesium methanoate needs to be diluted.
Describe how you would accurately measure a 5.0cm3 sample of saturated magnesium methanate solution and use it to prepare a solution fifty times more dilute than the saturated solution.
(vi) 1 mol of acidified MnO4- ions reacts with 2.5 mol of HCOO- ions.
25.0 cm3 of the diluted solution prepared in (iii) required 25.5 cm3 of 0.0200 mol dm-3 potassium manganate (VII) solution to reach the end point.
Use this information to calculate the concentration, in mol dm-3, of HCOO- ions in the diluted solution.
(Vii) use your answer to calculate the concentration of the saturated solution of magnesium methanoate
Can someone help me with vii
