A titration was conducted to determine the concentration of a potassium permanganate (KMnO4) solution. Three trials were used. KMnO4 (which has a purple color) was placed into a buret. The KMnO4 solution was slowly titrated into an Erlenmeyer flask containing 20.00 mL of an acidified solution of 1.000 M Fe(NO3)2 (which is colorless). The unbalanced chemical reaction that takes place when permanganate mixes with iron (II) under acidic conditions is shown below. MnO4- + Fe2+ ⟶⟶ Mn2+ + Fe3+ At the end point of this titration, permanganate will have mixed with iron (II) in the correct stoichiometric amount (according to the balanced equation) to produce manganese (II) and iron (III) which are both colorless. Trial #1 required 23.86 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter. Trial #2 required 23.48 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter. Trial #3 required 23.92 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter. Using the unrounded values of [KMnO4] for all three trials, determine the average [KMnO4] in moles/liter. The accepted value for the [KMnO4] for this experiment is 1.670 x 10-1 M KMnO4. Using the unrounded average [KMnO4] as your experimental value, calculated the percent error for this outcome.
A titration was conducted to determine the concentration of a potassium permanganate (KMnO4) solution. Three trials were used. KMnO4 (which has a purple color) was placed into a buret. The KMnO4 solution was slowly titrated into an Erlenmeyer flask containing 20.00 mL of an acidified solution of 1.000 M Fe(NO3)2 (which is colorless). The unbalanced
MnO4- + Fe2+ ⟶⟶ Mn2+ + Fe3+
At the end point of this titration, permanganate will have mixed with iron (II) in the correct stoichiometric amount (according to the balanced equation) to produce manganese (II) and iron (III) which are both colorless.
Trial #1 required 23.86 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter.
Trial #2 required 23.48 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter.
Trial #3 required 23.92 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter.
Using the unrounded values of [KMnO4] for all three trials, determine the average [KMnO4] in moles/liter.
The accepted value for the [KMnO4] for this experiment is 1.670 x 10-1 M KMnO4. Using the unrounded average [KMnO4] as your experimental value, calculated the percent error for this outcome.
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