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<center><b><nowiki>AP</nowiki> Question #2</b></center><br> <br> <i>Answer the following question showing all work. Please put answer in correct sig fig and if necessary scientific notation.</i> Concentrated sulfuric acid (18.4-molar H<sub>2</sub><nowiki>SO</nowiki><sub>4</sub>) has a density of 1.84 grams per millimeter. After dilution with water to 5.20-molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead storage batteries for automobiles. <br> a. Calculate the volume of concentrated acid required to prepare 1.00 liter of 5.20-molar H<sub>2</sub><nowiki>SO</nowiki><sub>4</sub>.<br> <br> b. Determine the mass percent of H<sub>2</sub><nowiki>SO</nowiki><sub>4</sub> in the original concentrated solution.<br> <br> c. Calculate the volume of 5.20-molar H<sub>2</sub><nowiki>SO</nowiki><sub>4</sub> that can be completely neutralized with 10.5 grams of sodium bicarbonate, <nowiki>NaHCO</nowiki><sub>3</sub>.<br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br>
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