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ANTONII [103]
3 years ago
7

In how many grams of water should 25.31 g of potassium nitrate (kno3) be dissolved to prepare a 0.1982 m solution?

Chemistry
2 answers:
Alex_Xolod [135]3 years ago
8 0

<u>Answer:</u> The mass of water that is needed to dissolve the given amount of potassium nitrate is 1263.1g

<u>Explanation:</u>

To calculate the mass of solvent for given molality of solution, we use the equation:

\text{Molality of solution}=\frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}

where,

Molality of the solution = 0.1982 m

m_{solute} = Given mass of solute (KNO_3) = 25.31 g

M_{solute} = Molar mass of solute (KNO_3) = 101.1 g/mol

W_{solvent}= Mass of solvent (water) = ?

Putting values in above equation, we get:

0.1982=\frac{25.31\times 1000}{101.1\times \text{Mass of water}}\\\\\text{Mass of water}=\frac{25.31\times 1000}{101.1\times 0.1982}=1263.1g

Hence, the mass of water that is needed to dissolve the given amount of potassium nitrate is 1263.1g

Artyom0805 [142]3 years ago
6 0

Solution:

Molality:-It is a measure of the concentration of a solute in a solution in terms of amount of substance in a specified amount of mass of the solvent

Therefore,  

Molality = moles solute / kg solvent  

Therefore kg solvent = moles solute / molality  

moles solute = mass / molar mass  

= 25.31 g / 101.1 g/mole  

= 0.2503 mole

kg solvent = 0.2503 mole / 0.1982 m  

= 1.263 kg  

= 1263 g

This is the required answer.

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