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Consider the salt aluminum hydroxide Al(OH)3 at 25°C. a. Calculate the solubility of Al3+ at a...

Consider the salt aluminum hydroxide Al(OH)3 at 25°C.

a. Calculate the solubility of Al3+ at a pH of 6.00, assuming that it is controlled by
the hydroxide. Express the concentration in mmol/L and ppm.

b. Calculate the pH value at which the solubility of Al3+ will be 1.74 ppm.

c. Explain, in terms of Le Chatelier's principle, how raising the pH affects the
solubility of Al3+.
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Answer #1

solution c) Le Chatelier principle: when a system experiences a disturbance (such as concentration, temperature, or pressure changes), it will respond to restore a new equilibrium state. so when we will increase the reactant the equilibrium will shift to forward and on increasing product equilibrium will shift to backward. so in this problem on increasing the ph we are indirectly increasing the concentration of OH- which means the equilibrium will shift to backward direction and solubility will decrease that's why solubility at pH 6 is less than the solubility at pH 4.64.

and also on lower ph means in acidic medium H+ will react with the formed OH- so it will decrease the concentration of product hence more the acidic medium more will be the solubility.

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