Question

What mass of agno3 must be dissolved in 200g of water to prepare a 0.250m solution

Answer 1

Answer:

$5.31 g AgNO3$

Explanation:

Your strategy here will be to

use the molality and mass of water to calculate how many moles of solute you have in your solution

use the molar mass of silver nitrate to convert the moles to grams

As you know, molality is defined as moles of solute, which in your case is silver nitrate, per kilogram of solvent. This means that a solution's molality essentially tells you the number of moles of solute present in 1 kg  of solvent

In your case, a  0.250 molal solution would contain  0.250 moles of solute for every moles of solute for every  1 kg

The problem tells you that you have $125 g$ of solvent available. Use the solution's molality as a conversion factor to calculate how many moles of silver nitrate it must contain -- do not forget to convert the mass of solvent from grams to kilograms

 

 $125g⋅1kg103g⋅= 0.250 molal0.250 moles AgNO31kg solvent=0.03125 moles AgNO3$

Now, you know that silver nitrate has a molar mass of $169.87g$ $moles$ of silver nitrate has a mass of $169.87 g$        You can thus say that$0.03123$ moles of silver nitrate will have a mass of  this statement ..........hope it's help u$0.03125moles AgNO3⋅169.87 g1mole AgNO3=∣∣∣∣¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯aa5.31 gaa∣∣−−−−−−−−−−$

Answer 2

Answer:

5.31 g Ag No3. will be the answer.

Explanation:

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