<p>Can someone explain #65? (It's a long problem that includes a lot of info so I can't type it out)</p>
<p>Also, can someone explain the reasoning behind these questions:</p>
<ol>
<li>The molarity of a solution X is to be determined by a titration procedure. To carry out this procedure, all of the following must be known except the</li>
</ol>
<p>A. Equation for the chem. reaction that occurs during the titration
B. Volume of the solution X that is used
C. Mass of solution X that is used
D. Volume of the solution that reacts with X
E. Molarity of the solution that reacts with X</p>
<p>Answer is C. </p>
<ol>
<li>The primary intermolecular attraction that makes it possible to liquify hydrogen gas is called</li>
</ol>
<p>A. London-dispersion forces
B. Dipole-Dipole
C. Covalent Bonding
D. Ionic Bonding
E. Hydrogen Bonding</p>
<p>Answer is A</p>
<p>I chose E cause I thought the London Dispersion forces were really weak.</p>
<ol>
<li><p>With titration you only deal with volume.
Molarity is mol/L. You need the the staring molarity (E) and you multiply it by Volume (B). You will end up with y mol of reactant. Obviously you need the reaction to calc. the mole to mole ratio to find out how many moles of X (A). Then, you divide it by the Volume of X (D), to find molarity.</p></li>
<li><p>H2 is hydrogen gas. It looks like this H:H. It shares each electron that it has. It only has LDFs.</p></li>
</ol>
<p>Question 62 is asking about the intermolecular attractions though, which makes London Dispersion forces the correct answer, being that H2 is nonpolar. Covalent bonds are not considered intermolecular forces and H2 does not contain hydrogen bonding so (E) is wrong.</p>