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QUESTION 1 Minnie Mouse did the Ka by Titrimetry experiment last week. Minnie used 28.63 mL...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and...
An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and will be used in an experiment to determine the percentage of iron in a sample of ammonium iron (II) sulfate hexahydrate. The titration is self-indicating because at the equivalence point the products are a different colour than the original reactants. The two half reactions are: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l) Fe^2+(aq) ---> Fe^3+(aq) + e- a) What is a redox...
A 0.898 grain sample of an unknown monoprotic acid is dissolved in 50.0 mL of water...
A 0.898 grain sample of an unknown monoprotic acid is dissolved in 50.0 mL of water and titrated with a 0.372 M aqueous sodium hydroxide solution. It is observed that after 15.0 milliliters of sodium hydroxide have been added, the pH is 5.053 and that an additional 6.90 mL of the sodium hydroxide solution is required to reach the equivalence point. What is the molecular weight of the acid? g/mol What is the value of K_a for the acid?
4.5e Question 1 Question 2 We now know the moles of hydroxide used in the titration....
4.5e Question 1
Question 2
We now know the moles of hydroxide used in the titration. But, remember that, of the 100 mL of solution made from the ashes, only 20 mL were used for the titration. What is the total amount of hydroxide produced by the ashes? Volume HCl used: 5.44 mlL Concentration HCI solution 0.10 M 5.44x 10 mol HCl used 5.44 x 104 mol OH in 20 ml. solution mol OH A 1.527-g sample of an unknown...
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium...
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...
(2) Find the oxidation numbers of the bold-labelled atoms in the following species: (a) CrF4 (b)...
(2) Find the oxidation numbers of the bold-labelled atoms in the following species: (a) CrF4 (b) UO3 (c) HReO4 (d) FeO42- (e) BrO3- (f) PH4+ (3) Suppose you have a 2.30 M solution of rubidium hydroxide and you are asked to make up 500.0 mL of 5.00 x 10-3M rubidium hydroxide. How much of the stock solution do you need? (4) How many grams of sodium formate (NaCHO2) do you need to make 250.0mL of 7.50 x 10-3M solution? (5)...
A 1.28 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water...
A 1.28 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.203 M aqueous barium hydroxide solution. It is observed that after 7.86 milliliters of barium hydroxide have been added, the pH is 3.000 and that an additional 16.6 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of Ka for the...
A 1.53 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water...
A 1.53 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.234 M aqueous barium hydroxide solution. It is observed that after 16.3 milliliters of barium hydroxide have been added, the pH is 4.924 and that an additional 10.0 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for the...
A 1.20 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water...
A 1.20 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.485 M aqucous potassium hydroxide solution. It is observed that after 7.33 milliliters of potassium hydroxide have been added, the pH is 4.515 and that an additional 13.3 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of K, for the...
A 1.48 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water...
A 1.48 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.291 M aqueous barium hydroxide solution. It is observed that after 7.15 milliliters of barium hydroxide have been added, the pH is 9.104 and that an additional 13.2 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol 2) What is the value of K_a for...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
A 0.898 grain sample of an unknown monoprotic acid is dissolved in 50.0 mL of water and titrated with a 0.372 M aqueous sodium hydroxide solution. It is observed that after 15.0 milliliters of sodium hydroxide have been added, the pH is 5.053 and that an additional 6.90 mL of the sodium hydroxide solution is required to reach the equivalence point. What is the molecular weight of the acid? g/mol What is the value of K_a for the acid?
4.5e Question 1
Question 2
We now know the moles of hydroxide used in the titration. But, remember that, of the 100 mL of solution made from the ashes, only 20 mL were used for the titration. What is the total amount of hydroxide produced by the ashes? Volume HCl used: 5.44 mlL Concentration HCI solution 0.10 M 5.44x 10 mol HCl used 5.44 x 104 mol OH in 20 ml. solution mol OH A 1.527-g sample of an unknown...
A 1.20 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.485 M aqucous potassium hydroxide solution. It is observed that after 7.33 milliliters of potassium hydroxide have been added, the pH is 4.515 and that an additional 13.3 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of K, for the...
A 1.48 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.291 M aqueous barium hydroxide solution. It is observed that after 7.15 milliliters of barium hydroxide have been added, the pH is 9.104 and that an additional 13.2 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol 2) What is the value of K_a for...
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