<p>Here is the question:</p>
<p>The reaction of barium chloride and sodium sulfate does not go to completion </p>
<p>BECAUSE </p>
<p>the compound barium sulfate is formed as an insoluble precipitate.</p>
<p>The answer is (F, T).</p>
<p>Can someone please explain why the first one is false and the second one is true? I don't really understand the question at all... and the explanation Barron's gave is vague.</p>
<p>The first one should be false seeing as how “Formation of a precipitate” is classified as one of the three traditional reactions that DO go to completion next to “Formation of a gaseous product” and “Evolution of a primarily non-ionized product”. As for the second statement, it involves application of solubility rules whereby Ba(SO4) is a precipitate since most compounds of barium are insoluble (except for sulfides and hydroxides I believe). </p>
<p><strong>Note SO4 is normally soluble with any other element (except for Ba, Ca, and Pb) so if it was another element then no precipitate would be formed and the reaction would be in equilibrium most likely</strong> </p>
<p>Review solubility rules and reactions that go to completion to become acquainted with the topic.</p>