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<font size="+1">I got the following question:<br>
<br>
"What do I write in my report about comparing my molar mass to the<br>
actual molar mass and if I’m right or not if I don’t know what the
acid was?"<br>
<br>
You can't actually compare it to the true molar mass because you
don't know<br>
what it is. The Points to Consider ask "Is the molar mass of the
acid reasonable<br>
for an acid which is fairly soluble in water"?<br>
<br>
Well, think about it. Would a MM of 20 g/mol make sense? This
would be<br>
a very small compound, most likely a gas at room temp (O2 has a MM
of<br>
32 g/mol). Most small molecules are gases or liquids at room
temp.<br>
The larger molecules get the more likely they would be solids at
room temp.<br>
If they get too large they wouldn't be soluble. Sugar molecules
like glucose,<br>
<span class="algo-summary">C6H12O6, </span>are very soluble in
water. Starch which is a whole lot of glucose<br>
molecules attached to each other to form what's essentially a
polymer isn't<br>
as soluble.<br>
<br>
KHP from the manual is a monoprotic acid that is fairly soluble in
water.<br>
You used it in part A. Look at it's molar mass. Based on this do
you think<br>
the MM for you acid is a reasonable number for an acid that
dissolves fairly<br>
well in water.<br>
<br>
Dr. Zellmer </font>
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