Silver Plating Formula
How do I solve this chemistry problem?
The information that I am given is:
Silver chloride, often used in silver plating, contains 75.27% Ag.
I must calculate the mass of silver chloride required to plate 285mg of pure silver.
Can you show me the formula I must use, please?
75.27% Ag means that it is not pure, so more is required than as per the equation. Ag + Cl -> AgCl.
285 mg of pure silver equals 285 Ag mg/107.868 g/mol = 2.64 mmol Ag. This equals 2.64 mmol * 143.3 = 378.8 mg of AgCl. Now we need more Ag, because the Ag is only 75.27%. This makes it 378.8 mg/75.27% = 503.25 mg of AgCl.
Hope this helps.
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