If 5wt% of silver nitrate solution is required, determine how many grams of silver nitrate is
need for an aqueous solution of 100ml.
What's the density of this 100 mL of SOLUTION? I don't know and can't answer the question without it.
5% w/w means 5 g AgNO3 in 100 g solution. IF you assume the density of this 100 mL is 1.00 g/mL, then the 100 mL will have a mass of 100 g. So you would need 5 g AgNO3 and 95 g H2O to make 5 g AgNO3/100 g solution which is 5 g AgNO3/100 mL if the density is 1.0 g/mL.
To determine the number of grams of silver nitrate needed for a 5wt% solution, we can use the formula:
Weight % = (weight of solute / weight of solution) * 100
Given that the desired weight % is 5% and the volume of the solution is 100 ml, we need to find the weight of silver nitrate.
Step 1: Convert the volume of the solution from ml to grams.
Since 1 ml of water is approximately equal to 1 gram, the volume of the solution is already in grams. Therefore, we have:
Weight of solution = 100 grams
Step 2: Rearrange the formula to find the weight of solute.
Weight of solute = (Weight % / 100) * Weight of solution
Weight of solute = (5 / 100) * 100 grams
Weight of solute = 5 grams
Therefore, you will need 5 grams of silver nitrate for an aqueous solution of 100 ml with a 5wt% concentration.