Silver chloride, often used in silver plating, contains 75.27% Ag.
Calculate the mass of silver chloride required to plate 195mg of pure silver.
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To calculate the mass of silver chloride required to plate 195mg of pure silver, we need to determine the mass ratio between silver and silver chloride.
Since silver chloride contains 75.27% Ag, the remaining percentage is Cl (chlorine). Thus, the percentage of chlorine is 100% - 75.27% = 24.73%.
Given that the mass of silver chloride is the sum of the mass of Ag and Cl, we can calculate the mass ratio as follows:
Mass ratio of Ag to AgCl = 75.27% Ag / (75.27% Ag + 24.73% Cl) = 75.27 / 100 = 0.7527
To find the mass of silver chloride required, we divide the mass of pure silver by the mass ratio:
Mass of AgCl = Mass of Ag / Mass ratio of Ag to AgCl = 195mg / 0.7527 ≈ 259.02mg
Therefore, the mass of silver chloride required to plate 195mg of pure silver is approximately 259.02mg.
To calculate the mass of silver chloride required to plate 195 mg of pure silver, we need to first determine the amount of silver present in 195 mg of pure silver.
Given that silver chloride contains 75.27% silver, we can calculate the amount of silver in 195 mg of pure silver as follows:
Amount of silver = (75.27% / 100%) x 195 mg
= (0.7527) x 195 mg
= 146.7415 mg
Now that we know the amount of silver required, we can calculate the mass of silver chloride needed. Since silver chloride contains 75.27% silver, we can set up the following equation:
Amount of silver chloride / Total mass of silver chloride = Amount of silver / Total mass of silver chloride
Let x be the mass of silver chloride required.
(0.7527) = 146.7415 mg / (x + 146.7415 mg)
Solving for x:
(0.7527) (x + 146.7415 mg) = 146.7415 mg
0.7527x + 110.3521 mg = 146.7415 mg
0.7527x = 36.3894 mg
x = 36.3894 mg / 0.7527
Therefore, the mass of silver chloride required to plate 195 mg of pure silver is approximately 48.37 mg.
0.7527 x mass AgCl = 195 mg.
Solve for mass AgCl.