{"id":232,"date":"2025-07-01T02:01:09","date_gmt":"2025-07-01T02:01:09","guid":{"rendered":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/?post_type=chapter&#038;p=232"},"modified":"2026-09-16T01:04:32","modified_gmt":"2026-09-16T01:04:32","slug":"introduction-to-density-of-solids","status":"web-only","type":"chapter","link":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/chapter\/introduction-to-density-of-solids\/","title":{"raw":"Laboratory Preparation &amp; Procedure","rendered":"Laboratory Preparation &amp; Procedure"},"content":{"raw":"<h2><strong>Materials:<\/strong><\/h2>\r\n<ul>\r\n \t<li>Copper cylinders<\/li>\r\n \t<li>Analytical balance<\/li>\r\n \t<li>Caliper<\/li>\r\n \t<li>100-mL graduated cylinder<\/li>\r\n \t<li>Distilled water<\/li>\r\n \t<li>Unknown metal cylinder<\/li>\r\n<\/ul>\r\n<h2><strong>Safety:<\/strong><\/h2>\r\nHandle metal cylinders with care. Do not drop metals into glassware.\u00a0 Use calipers carefully as they can pinch fingers if misused. Never force them closed and keep your hands clear when measuring. Avoid spills around the balance.\r\n<h2><strong>Procedure:<\/strong><\/h2>\r\nPart A. Determining the Density of a Copper Cylinder using Volume by Geometry\r\n<ol>\r\n \t<li>Obtain a metal copper cylinder.<\/li>\r\n \t<li>Tare your balance.<\/li>\r\n \t<li>Record the mass of an empty weigh tray in table 1.<\/li>\r\n \t<li>Add your copper cylinder to the weigh tray and record the mass of the weigh tray + copper cylinder in table 1.<\/li>\r\n \t<li>Calculate the mass of the copper cylinder. Show all corresponding work.<\/li>\r\n \t<li>Using the caliper, measure the diameter of the copper cylinder (mm or in). Record all values from the caliper in table 1. Be sure to include the unit.<\/li>\r\n \t<li>Convert the diameter given from your caliper (mm or in) to units of cm in table 1. Show all corresponding work for this conversion.<\/li>\r\n \t<li>Using the diameter (cm), calculate the corresponding radius in table 1. Record your radius to the proper number of significant digits.<\/li>\r\n \t<li>Using the caliper, measure the height of the copper cylinder in table 1 (mm or in). Record all values from the caliper in table 1. Be sure to include the unit.<\/li>\r\n \t<li>Convert the height given from your caliper (mm or in) to units of cm in table 1. Show all corresponding work for this conversion.<\/li>\r\n \t<li>Calculate the volume of the copper cylinder (cm<sup>3<\/sup>) using its appropriate volume formula in table 1. Be sure to record your final volume to the appropriate number of significant figures. Show your calculations.<\/li>\r\n \t<li>Calculate the density of the copper cylinder using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 1.<\/li>\r\n \t<li>Using the actual density of the copper cylinder (8.92 g\/cm<sup>3<\/sup>) calculate your percent error. *Note: Remeasure your copper cylinder if your percent error exceeds 5%.<\/li>\r\n \t<li>Add your density to the class data set at the front of the room.<\/li>\r\n<\/ol>\r\nPart B. Determining the Density of a Copper Cylinder using Volume by Displacement\r\n<ol>\r\n \t<li>Obtain a metal copper cylinder. (Use the same copper cylinder from Part A.)<\/li>\r\n \t<li>Tare your balance.<\/li>\r\n \t<li>Record the mass of an empty weigh tray in table 2, Trial 1.<\/li>\r\n \t<li>Add your copper cylinder to the weigh tray and record the mass of the weigh tray + copper cylinder in table 2, Trial 1.<\/li>\r\n \t<li>Calculate the mass of the copper cylinder. Show all corresponding work.<\/li>\r\n \t<li>Place approximately 50-mL of water in a 100-mL graduated cylinder. Record the initial volume of the water to the correct precision of the graduated cylinder.<\/li>\r\n \t<li>Carefully slide the metal cylinder down the side of the graduated cylinder into the water. Tossing it in can break the bottom of the graduated cylinder.<\/li>\r\n \t<li>With the metal cylinder completely submerged, record the new volume reading. Record this as the volume of water, final in table 2, trial 1. Report this final volume to the correct precision of the graduated cylinder.<\/li>\r\n \t<li>Determine the volume of the metal cylinder (mL) using the volume by displacement measurement method.\u00a0 Show all work.<\/li>\r\n \t<li>Convert your experimental volume (mL) to units of cm<sup>3<\/sup>. Show all work.<\/li>\r\n \t<li>Calculate the density of the copper cylinder (g\/cm<sup>3<\/sup>) using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 2, trial 1.<\/li>\r\n \t<li>Repeat steps 1 - 11 using 75-mL of water as your initial volume of water instead of 50-mL (from step 6). These values will correspond to table 2, trial 2.<\/li>\r\n \t<li>Calculate the average density of your copper cylinder.<\/li>\r\n \t<li>Using the actual density of the copper cylinder (8.92 g\/cm<sup>3<\/sup>) calculate your percent error. NOTE: Your percent error may exceed 5% for these values. You do not need to remeasure as long as your density values between your two trials agree.<\/li>\r\n<\/ol>\r\nPart C. Density of the unknown metal cylinder using volume by geometry\r\n<ol>\r\n \t<li>Obtain an unknown metal cylinder. Record its identifier in your lab notebook.<\/li>\r\n \t<li>Tare your balance.<\/li>\r\n \t<li>Record the mass of an empty weigh tray in table 3.<\/li>\r\n \t<li>Add your unknown metal cylinder to the weigh tray and record the mass of the weigh tray + copper cylinder in table 3.<\/li>\r\n \t<li>Calculate the mass of the unknown metal cylinder. Show all corresponding work.<\/li>\r\n \t<li>Using the caliper, measure the diameter of the unknown metal cylinder (mm or in). Record all values from the caliper in table 3. Be sure to include the unit.<\/li>\r\n \t<li>Convert the diameter given from your caliper (mm or in) to units of cm in table 3. Show all corresponding work for this conversion.<\/li>\r\n \t<li>Using the diameter (cm), calculate the corresponding radius in table 3. Record your radius to the proper number of significant digits.<\/li>\r\n \t<li>Using the caliper, measure the height of the unknown metal cylinder in table 3 (mm or in). Record all values from the caliper in table 3. Be sure to include the unit.<\/li>\r\n \t<li>Convert the height given from your caliper (mm or in) to units of cm in table 3. Show all corresponding work for this conversion.<\/li>\r\n \t<li>Calculate the volume of the copper cylinder (cm<sup>3<\/sup>) using its appropriate volume formula in table 3. Be sure to record your final volume to the appropriate number of significant figures. Show your calculations.<\/li>\r\n \t<li>Calculate the density of the unknown metal cylinder using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 3.<\/li>\r\n \t<li>Use the chart below of known densities to identify your unknown. Calculate the percent error between your calculated value and the theoretical density.<\/li>\r\n<\/ol>\r\n<table style=\"width: 302px;height: 617px\">\r\n<tbody>\r\n<tr>\r\n<th style=\"width: 120px\">Metal<\/th>\r\n<td style=\"width: 168px\">Density (g\/cm<sup>3<\/sup>)<\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Aluminum<\/th>\r\n<td style=\"width: 168px\">2.70 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Zinc<\/th>\r\n<td style=\"width: 168px\">7.14 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Tin<\/th>\r\n<td style=\"width: 168px\">7.31 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Steel<\/th>\r\n<td style=\"width: 168px\">7.85 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Brass<\/th>\r\n<td style=\"width: 168px\">8.73 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Copper<\/th>\r\n<td style=\"width: 168px\">8.92 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Silver<\/th>\r\n<td style=\"width: 168px\">10.49 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Lead<\/th>\r\n<td style=\"width: 168px\">11.34 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 120px\">Gold<\/th>\r\n<td style=\"width: 168px\">19.30 g\/cm<sup>3<\/sup><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nPart D. Determining the Density of an unknown metal cylinder using Volume by Displacement\r\n<ol>\r\n \t<li>Obtain an unknown metal cylinder. (Use the same unknown metal cylinder from Part C.) Record its identifier in your lab notebook.<\/li>\r\n \t<li>Tare your balance.<\/li>\r\n \t<li>Record the mass of an empty weigh tray in table 4, Trial 1.<\/li>\r\n \t<li>Add your unknown metal cylinder to the weigh tray and record the mass of the weigh tray + unknown metal cylinder in table 4, Trial 1.<\/li>\r\n \t<li>Calculate the mass of theunknown metal cylinder. Show all corresponding work.<\/li>\r\n \t<li>Place approximately 50-mL of water in a 100-mL graduated cylinder. Record the initial volume of the water to the correct precision of the graduated cylinder.<\/li>\r\n \t<li>Carefully slide the metal cylinder down the side of the graduated cylinder into the water. Tossing it in can break the bottom of the graduated cylinder.<\/li>\r\n \t<li>With the metal cylinder completely submerged, record the new volume reading. Record this as the volume of water, final in table 4, trial 1. Report this final volume to the correct precision of the graduated cylinder.<\/li>\r\n \t<li>Determine the volume of the metal cylinder (mL) using the volume by displacement measurement method.\u00a0 Show all work.<\/li>\r\n \t<li>Convert your experimental volume (mL) to units of cm<sup>3<\/sup>. Show all work.<\/li>\r\n \t<li>Calculate the density of the unknown metal cylinder (g\/cm<sup>3<\/sup>) using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 4, trial 1.<\/li>\r\n \t<li>Repeat steps 1 - 11 using 75-mL of water as your initial volume of water instead of 50-mL (from step 6). These values will correspond to table 4, trial 2.<\/li>\r\n \t<li>Calculate the average density of your unknown metal cylinder.<\/li>\r\n \t<li>Use the chart above of known densities to identify your unknown. Calculate the percent error between your calculated value (average density) and the theoretical density. NOTE: Your percent error may exceed 5% for these values. You do not need to remeasure as long as your density values between your two trials agree.<\/li>\r\n<\/ol>","rendered":"<h2><strong>Materials:<\/strong><\/h2>\n<ul>\n<li>Copper cylinders<\/li>\n<li>Analytical balance<\/li>\n<li>Caliper<\/li>\n<li>100-mL graduated cylinder<\/li>\n<li>Distilled water<\/li>\n<li>Unknown metal cylinder<\/li>\n<\/ul>\n<h2><strong>Safety:<\/strong><\/h2>\n<p>Handle metal cylinders with care. Do not drop metals into glassware.\u00a0 Use calipers carefully as they can pinch fingers if misused. Never force them closed and keep your hands clear when measuring. Avoid spills around the balance.<\/p>\n<h2><strong>Procedure:<\/strong><\/h2>\n<p>Part A. Determining the Density of a Copper Cylinder using Volume by Geometry<\/p>\n<ol>\n<li>Obtain a metal copper cylinder.<\/li>\n<li>Tare your balance.<\/li>\n<li>Record the mass of an empty weigh tray in table 1.<\/li>\n<li>Add your copper cylinder to the weigh tray and record the mass of the weigh tray + copper cylinder in table 1.<\/li>\n<li>Calculate the mass of the copper cylinder. Show all corresponding work.<\/li>\n<li>Using the caliper, measure the diameter of the copper cylinder (mm or in). Record all values from the caliper in table 1. Be sure to include the unit.<\/li>\n<li>Convert the diameter given from your caliper (mm or in) to units of cm in table 1. Show all corresponding work for this conversion.<\/li>\n<li>Using the diameter (cm), calculate the corresponding radius in table 1. Record your radius to the proper number of significant digits.<\/li>\n<li>Using the caliper, measure the height of the copper cylinder in table 1 (mm or in). Record all values from the caliper in table 1. Be sure to include the unit.<\/li>\n<li>Convert the height given from your caliper (mm or in) to units of cm in table 1. Show all corresponding work for this conversion.<\/li>\n<li>Calculate the volume of the copper cylinder (cm<sup>3<\/sup>) using its appropriate volume formula in table 1. Be sure to record your final volume to the appropriate number of significant figures. Show your calculations.<\/li>\n<li>Calculate the density of the copper cylinder using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 1.<\/li>\n<li>Using the actual density of the copper cylinder (8.92 g\/cm<sup>3<\/sup>) calculate your percent error. *Note: Remeasure your copper cylinder if your percent error exceeds 5%.<\/li>\n<li>Add your density to the class data set at the front of the room.<\/li>\n<\/ol>\n<p>Part B. Determining the Density of a Copper Cylinder using Volume by Displacement<\/p>\n<ol>\n<li>Obtain a metal copper cylinder. (Use the same copper cylinder from Part A.)<\/li>\n<li>Tare your balance.<\/li>\n<li>Record the mass of an empty weigh tray in table 2, Trial 1.<\/li>\n<li>Add your copper cylinder to the weigh tray and record the mass of the weigh tray + copper cylinder in table 2, Trial 1.<\/li>\n<li>Calculate the mass of the copper cylinder. Show all corresponding work.<\/li>\n<li>Place approximately 50-mL of water in a 100-mL graduated cylinder. Record the initial volume of the water to the correct precision of the graduated cylinder.<\/li>\n<li>Carefully slide the metal cylinder down the side of the graduated cylinder into the water. Tossing it in can break the bottom of the graduated cylinder.<\/li>\n<li>With the metal cylinder completely submerged, record the new volume reading. Record this as the volume of water, final in table 2, trial 1. Report this final volume to the correct precision of the graduated cylinder.<\/li>\n<li>Determine the volume of the metal cylinder (mL) using the volume by displacement measurement method.\u00a0 Show all work.<\/li>\n<li>Convert your experimental volume (mL) to units of cm<sup>3<\/sup>. Show all work.<\/li>\n<li>Calculate the density of the copper cylinder (g\/cm<sup>3<\/sup>) using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 2, trial 1.<\/li>\n<li>Repeat steps 1 &#8211; 11 using 75-mL of water as your initial volume of water instead of 50-mL (from step 6). These values will correspond to table 2, trial 2.<\/li>\n<li>Calculate the average density of your copper cylinder.<\/li>\n<li>Using the actual density of the copper cylinder (8.92 g\/cm<sup>3<\/sup>) calculate your percent error. NOTE: Your percent error may exceed 5% for these values. You do not need to remeasure as long as your density values between your two trials agree.<\/li>\n<\/ol>\n<p>Part C. Density of the unknown metal cylinder using volume by geometry<\/p>\n<ol>\n<li>Obtain an unknown metal cylinder. Record its identifier in your lab notebook.<\/li>\n<li>Tare your balance.<\/li>\n<li>Record the mass of an empty weigh tray in table 3.<\/li>\n<li>Add your unknown metal cylinder to the weigh tray and record the mass of the weigh tray + copper cylinder in table 3.<\/li>\n<li>Calculate the mass of the unknown metal cylinder. Show all corresponding work.<\/li>\n<li>Using the caliper, measure the diameter of the unknown metal cylinder (mm or in). Record all values from the caliper in table 3. Be sure to include the unit.<\/li>\n<li>Convert the diameter given from your caliper (mm or in) to units of cm in table 3. Show all corresponding work for this conversion.<\/li>\n<li>Using the diameter (cm), calculate the corresponding radius in table 3. Record your radius to the proper number of significant digits.<\/li>\n<li>Using the caliper, measure the height of the unknown metal cylinder in table 3 (mm or in). Record all values from the caliper in table 3. Be sure to include the unit.<\/li>\n<li>Convert the height given from your caliper (mm or in) to units of cm in table 3. Show all corresponding work for this conversion.<\/li>\n<li>Calculate the volume of the copper cylinder (cm<sup>3<\/sup>) using its appropriate volume formula in table 3. Be sure to record your final volume to the appropriate number of significant figures. Show your calculations.<\/li>\n<li>Calculate the density of the unknown metal cylinder using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 3.<\/li>\n<li>Use the chart below of known densities to identify your unknown. Calculate the percent error between your calculated value and the theoretical density.<\/li>\n<\/ol>\n<table style=\"width: 302px;height: 617px\">\n<tbody>\n<tr>\n<th style=\"width: 120px\">Metal<\/th>\n<td style=\"width: 168px\">Density (g\/cm<sup>3<\/sup>)<\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Aluminum<\/th>\n<td style=\"width: 168px\">2.70 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Zinc<\/th>\n<td style=\"width: 168px\">7.14 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Tin<\/th>\n<td style=\"width: 168px\">7.31 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Steel<\/th>\n<td style=\"width: 168px\">7.85 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Brass<\/th>\n<td style=\"width: 168px\">8.73 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Copper<\/th>\n<td style=\"width: 168px\">8.92 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Silver<\/th>\n<td style=\"width: 168px\">10.49 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Lead<\/th>\n<td style=\"width: 168px\">11.34 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<th style=\"width: 120px\">Gold<\/th>\n<td style=\"width: 168px\">19.30 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Part D. Determining the Density of an unknown metal cylinder using Volume by Displacement<\/p>\n<ol>\n<li>Obtain an unknown metal cylinder. (Use the same unknown metal cylinder from Part C.) Record its identifier in your lab notebook.<\/li>\n<li>Tare your balance.<\/li>\n<li>Record the mass of an empty weigh tray in table 4, Trial 1.<\/li>\n<li>Add your unknown metal cylinder to the weigh tray and record the mass of the weigh tray + unknown metal cylinder in table 4, Trial 1.<\/li>\n<li>Calculate the mass of theunknown metal cylinder. Show all corresponding work.<\/li>\n<li>Place approximately 50-mL of water in a 100-mL graduated cylinder. Record the initial volume of the water to the correct precision of the graduated cylinder.<\/li>\n<li>Carefully slide the metal cylinder down the side of the graduated cylinder into the water. Tossing it in can break the bottom of the graduated cylinder.<\/li>\n<li>With the metal cylinder completely submerged, record the new volume reading. Record this as the volume of water, final in table 4, trial 1. Report this final volume to the correct precision of the graduated cylinder.<\/li>\n<li>Determine the volume of the metal cylinder (mL) using the volume by displacement measurement method.\u00a0 Show all work.<\/li>\n<li>Convert your experimental volume (mL) to units of cm<sup>3<\/sup>. Show all work.<\/li>\n<li>Calculate the density of the unknown metal cylinder (g\/cm<sup>3<\/sup>) using your calculated volume. Be sure to report your final density to the proper number of significant figures in table 4, trial 1.<\/li>\n<li>Repeat steps 1 &#8211; 11 using 75-mL of water as your initial volume of water instead of 50-mL (from step 6). These values will correspond to table 4, trial 2.<\/li>\n<li>Calculate the average density of your unknown metal cylinder.<\/li>\n<li>Use the chart above of known densities to identify your unknown. Calculate the percent error between your calculated value (average density) and the theoretical density. NOTE: Your percent error may exceed 5% for these values. You do not need to remeasure as long as your density values between your two trials agree.<\/li>\n<\/ol>\n","protected":false},"author":125,"menu_order":2,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-232","chapter","type-chapter","status-web-only","hentry"],"part":228,"_links":{"self":[{"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/chapters\/232","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/wp\/v2\/users\/125"}],"version-history":[{"count":17,"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/chapters\/232\/revisions"}],"predecessor-version":[{"id":1064,"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/chapters\/232\/revisions\/1064"}],"part":[{"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/parts\/228"}],"metadata":[{"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/chapters\/232\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/wp\/v2\/media?parent=232"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/pressbooks\/v2\/chapter-type?post=232"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/wp\/v2\/contributor?post=232"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.hcfl.edu\/introchemlabmanual\/wp-json\/wp\/v2\/license?post=232"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}