Sorry, I have a question within a question. I think the ka value for the aluminum ion is used for when we have a solution like AlCl3, right? When you dissociate it, the Cl ion has a very large ka value...so we use the ka for Al instead? I hope I'm making sense. :)
You're right. It doesn't make sense. Cl^- is a Bronsted-Lowry base BUT a very weak one. It won't even displace H from HOH. The acidity of AlCl3 solutions and Al2(SO4)3 solutions is due to the hydration of the Al^+3 ion and the Ka given in the problem is the one for which I wrote the ionization above although it may have shown H2O as part of the reaction. You work those problem just like the Ka for a weak acid, HA. Note: Gardener's put Al2(SO4)3 in their soil to increase the acidity (lower the pH of the soil) in order to accommodate plants that require an acid soil to grow. Plants like hydrangea (the flowers) actually turn color, pink for acid and blue for basic.
the lead (II) nitrate in 25.49 ml of a 0.1338M solution reacts with all of the aluminum sulfate in 25.00 ml solution. What is the molar concentration of the aluminum sulfate in the original aluminum sulfate solution? For a
the lead (II) nitrate in 25.49 ml of a 0.1338M solution reacts with all of the aluminum sulfate in 25.00 ml solution. What is the molar concentration of the aluminum sulfate in the original aluminum sulfate solution?
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