30 ml KMnO4 solution is required to titrate 25 ml M/50 oxalic acid solution.find the molarity of KMnO4 solution and g/L also.
To find the molarity of the KMnO4 solution and its concentration in g/L, we can use the equation:
Molarity (M) = (moles of solute) / (volume of solution in liters)
First, let's calculate the moles of oxalic acid in the M/50 solution:
Moles of Oxalic Acid = Molarity × Volume (in liters)
= (1/50) × 0.025
= 0.0005 moles
Now, let's find the moles of KMnO4 required for the reaction by using the balanced equation:
5 C2H2O4 + 2 MnO4^- + 6 H+ -> 10 CO2 + 2 Mn^2+ + 8 H2O
From the balanced equation, we can see that the stoichiometric ratio between oxalic acid and potassium permanganate (KMnO4) is 5:2. Therefore, the moles of KMnO4 required will be:
Moles of KMnO4 = (5/2) × 0.0005
= 0.00125 moles
Given that the volume of KMnO4 solution used is 30 ml (which is 0.03 liters), we can now calculate the molarity of KMnO4:
Molarity of KMnO4 = (moles of solute) / (volume of solution in liters)
= 0.00125 moles / 0.03 liters
= 0.0417 M (rounded to 4 decimal places)
To determine the concentration of KMnO4 in g/L, we need to know the molar mass of KMnO4:
Molar mass of KMnO4 = atomic mass of K + atomic mass of Mn + (4 × atomic mass of O)
= 39.1 + 54.9 + (4 × 16.0)
= 158.0 g/mol
Now, let's calculate the concentration of KMnO4 in g/L:
Concentration (g/L) = (Molarity) × (Molar mass of KMnO4)
= 0.0417 M × 158.0 g/mol
= 6.575 g/L (rounded to 3 decimal places)
Therefore, the molarity of the KMnO4 solution is 0.0417 M, and its concentration is 6.575 g/L.
To find the molarity of the KMnO4 solution, we can use the concept of stoichiometry and the balanced chemical equation between KMnO4 and oxalic acid.
The balanced equation for the reaction between KMnO4 and oxalic acid is:
5C2H2O4 + 2KMnO4 + 3H2SO4 → 2MnSO4 + 10CO2 + 8H2O + K2SO4
From the balanced equation, we can deduce that 2 moles of KMnO4 react with 5 moles of oxalic acid. This means that the mole ratio between KMnO4 and oxalic acid is 2:5.
Given that 30 ml of KMnO4 solution is required to titrate 25 ml of M/50 oxalic acid solution, we can set up the following proportion:
(30 ml KMnO4) / (25 ml oxalic acid) = (Molarity of KMnO4) / (Molarity of oxalic acid)
Since the molarity of the oxalic acid solution is M/50, we can substitute that value into the equation:
(30 ml KMnO4) / (25 ml oxalic acid) = (Molarity of KMnO4) / (M/50)
Now we can solve for the molarity of the KMnO4 solution:
Molarity of KMnO4 = (30 ml KMnO4) / (25 ml oxalic acid) * (M/50)
To find the g/L (grams per liter) concentration of KMnO4, we need to convert the molarity to grams. The molar mass of KMnO4 is 158.03 g/mol.
To convert from moles to grams, we can use the formula:
Grams = Moles * Molar Mass
So, to find the g/L concentration, we need to multiply the molarity by the molar mass of KMnO4 and convert from mL to L:
g/L concentration = (Molarity of KMnO4) * (Molar Mass of KMnO4) * (1000 mL / 1 L)
By substituting the values, you can calculate the molarity of the KMnO4 solution and its g/L concentration.