Question

How many miles of K2CRO
are present

Answer 1

To prepare a 0.1 N solution of K2Cr2O7, approximately 29.42 grams of the substance is required per liter. This calculation considers the molar mass and the definition of normality for the given compound.

To prepare a 0.1 N (Normal) solution of K2Cr2O7, you need to consider the molar mass and the definition of normality. The molar mass of K2Cr2O7 is 294.19 g/mol.

The formula for normality (N) is given by:

`\[ N = \frac{{\text{{Number of equivalents}}}}{{\text{{Volume of solution in liters}}}} \]`

For K2Cr2O7, each mole provides 6 equivalents of
`\(CrO_4^(2-)\)` ions, as the oxidation state of chromium changes from +6 to +3. Therefore, the number of equivalents is 6 times the moles of K2Cr2O7.

Given that the desired normality is 0.1 N, you can set up the equation:

`\[ 0.1 \, \text{N} = \frac{{\text{{6 equivalents}}}}{{\text{{Volume in liters}}}} \]`

Solving for the volume in liters gives:

`\[ \text{{Volume}} = \frac{{\text{{Number of equivalents}}}}{{0.1 \, \text{N}}} = \frac{{6}}{{0.1}} = 60 \, \text{L} \]`

Now, convert liters to milliliters (1 L = 1000 mL):

`\[ \text{{Volume in mL}} = 60 \, \text{L} * 1000 \, \text{mL/L} = 60000 \, \text{mL} \]`

Finally, calculate the mass using the molar mass:

`\[ \text{{Mass}} = \text{{Number of moles}} * \text{{Molar mass}} \]`

`\[ \text{{Mass}} = 0.1 \, \text{mol/L} * 294.19 \, \text{g/mol} = 29.419 \, \text{g/L} \]`

For 1 liter, you need 29.419 grams of K2Cr2O7. Therefore, for 1 liter of a 0.1 N solution, you would require approximately 29.42 grams of K2Cr2O7.

Note: Calculations are based on ideal conditions, and it's advisable to weigh the substance accurately and perform experimental verification for precise results.

The probable question may be:

How many grams of k2cr2o7 substance are required to make one litre of 0.1 n solution?