Calculating Maximum Silver Plating from AgNO3 Solution

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To calculate the maximum amount of silver that can be plated from a 4.6 L AgNO3 solution with 3.7% silver by mass, first determine the mass of the solution using its density of 1.01 g/mL. The total mass of the solution is approximately 4660 g (4.6 L x 1000 mL/L x 1.01 g/mL). Next, apply the mass percent formula to find the mass of silver: 3.7% of 4660 g yields about 172.42 g of silver. This calculation confirms the maximum amount of silver that can be plated from the solution. The problem illustrates the importance of understanding mass percent and solution density in quantitative chemistry.
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Homework Statement



Silver nitrate solutions are often used to plate silver onto other metals. What is the maximum amount of silver (in grams) that can be plated out of 4.6 L of an AgNO3 solution containing 3.7% Ag by mass? Assume that the density of the solution is 1.01g/mL .


Homework Equations


m=moles of solute/ mass of solvent (kg)
mass percent=(mass of component/ total mass of solution)*100%


The Attempt at a Solution


I have no idea how to even approach this problem so maybe just a hint can help me gain some sort of insight.
 
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Start finding mass of the solution, then apply percentage information.
 
Thank you so much, I figured it out and got it right. :smile:
 
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