Silver chloride ( $AgCI$ ) is relatively insoluble in water. At 25 C, $1.3 x 10^3$ L of water is needed to dissolve 2.5 g of $AgCl$ . What mass (in milligrams) of $AgCl$ will dissolve in 1.0 L of water?

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Silver chloride ( $AgCI$ ) is relatively insoluble in water. At 25 C, $1.3 x 10^3$ L of water is needed to dissolve 2.5 g of $AgCl$ . What mass (in milligrams) of $AgCl$ will dissolve in 1.0 L of water?

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Answer 1 · 2016-09-05T08:13:52

Approx. $2*mg$

Explanation:

$"Solubility"$ $=$ $"Moles of solute"/"Volume of solution"$ .

For silver chloride we are given that: $2.5*g$ wil dissolve in over $1$ $m^3$ of water.

And thus, $"Solubility"$ $=$ $(2.5*g)/(143.32*g*mol^-1)xx1/(1.3xx10^3*L)$ $=$ $1.34xx10^-5*mol*L^-1$ .

And thus silver chloride solute in 1L of saturated water $=$ $1.34xx10^-5*mol*L^-1xx143.32*g*mol^-1xx1L$ $~=$ $2*mg$

Typically, you are quoted a $K_"sp"$ for these insoluble salts. $K_"sp "AgCl=1.77xx10^-10$ . $K_"sp"$ values can be shown to depend on the molar solubilities.

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Silver chloride ( $AgCI$ ) is relatively insoluble in water. At 25 C, $1.3 x 10^3$ L of water is needed to dissolve 2.5 g of $AgCl$ . What mass (in milligrams) of $AgCl$ will dissolve in 1.0 L of water?

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Explanation:

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Silver chloride (AgCIAgCI) is relatively insoluble in water. At 25 C, 1.3 x 10^31.3 x 10^3 L of water is needed to dissolve 2.5 g of AgClAgCl. What mass (in milligrams) of AgClAgCl will dissolve in 1.0 L of water?

1 Answer

Explanation:

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Silver chloride ( $AgCI$ ) is relatively insoluble in water. At 25 C, $1.3 x 10^3$ L of water is needed to dissolve 2.5 g of $AgCl$ . What mass (in milligrams) of $AgCl$ will dissolve in 1.0 L of water?