Mercury (I) sulfate (Hg 2 SO 4 ) was often used in electrochemical cells in the

Question

Mercury (I) sulfate (Hg2SO4) was often used in electrochemical cells in the early 1900s. A ship carrying Mercury (I) sulfate electrodes from New York to Amsterdam unknowingly took on water during the journey. Upon reaching Amsterdan, the captain found that the compartment holding the electrodes took on 50.0L of seawater. The Ksp of Hg2SO4 = 6.5x10-7  

1. Calculate the concentration of Hg2SO4 in the seawater. Seawater has a typical [SO42-] = 0.028M

2. How many grams of Hg2SO4 were lost (dissolved in water) during the journey?

Explanation / Answer

1.

Hg2SO4 (s) = 2Hg+ (aq.) + SO42- (aq.)

Ksp = [Hg+]2[SO42-]

6.5 * 10-7 = [Hg+] * ( 0.028)

[Hg+] = 2.32 * 10-5 M

Therefore,

[[Hg2SO4] = (1/2)*[Hg+] = 1.16 * 10-5 M

2.

Molarity = moles / volume

Moles of Hg2SO4 = 1.16 * 10-5 * 50.0 = 5.80 * 10-4 mol

Mass of Hg2SO4 = moles * molar mass = 5.80 * 10-4 * 497.2 = 0.288 g.

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