{"id":45824,"date":"2025-07-01T12:29:16","date_gmt":"2025-07-01T12:29:16","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=45824"},"modified":"2025-07-01T12:29:18","modified_gmt":"2025-07-01T12:29:18","slug":"mass-of-unknown-transferred-mass-of-filter-paper-mass-of-paper-and-dry-baso","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/mass-of-unknown-transferred-mass-of-filter-paper-mass-of-paper-and-dry-baso\/","title":{"rendered":"Mass of unknown transferred Mass of filter paper Mass of paper and dry BaSO"},"content":{"rendered":"\n
Mass of unknown transferred Mass of filter paper Mass of paper and dry BaSO, Trial 1 (Yours) 0.294g 0.907g 1.203g Trial 2 (Partners) 0.253g 0.899g 1.163g Give me the Calculations week 1 Mass of dry BasO Calculated percent sulfate in unknown AVERAGE PERCENT SULFATE<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
To calculate the mass of dry BaSO\u2084 (barium sulfate) and the percentage of sulfate in the unknown sample, we need to follow a step-by-step process using the data provided from both trials.<\/p>\n\n\n\n
Step 1: Calculate the mass of BaSO\u2084 in each trial.<\/h3>\n\n\n\n
Trial 1 (Your Sample):<\/h4>\n\n\n\n
\n
Mass of paper and dry BaSO\u2084: 1.203 g<\/li>\n\n\n\n
Mass of filter paper: 0.907 g<\/li>\n<\/ul>\n\n\n\n
Mass of dry BaSO\u2084 = Mass of paper and dry BaSO\u2084 – Mass of filter paper Mass of dry BaSO\u2084 = 1.203 g – 0.907 g = 0.296 g<\/strong><\/p>\n\n\n\n
Trial 2 (Partner’s Sample):<\/h4>\n\n\n\n
\n
Mass of paper and dry BaSO\u2084: 1.163 g<\/li>\n\n\n\n
Mass of filter paper: 0.899 g<\/li>\n<\/ul>\n\n\n\n
Mass of dry BaSO\u2084 = Mass of paper and dry BaSO\u2084 – Mass of filter paper Mass of dry BaSO\u2084 = 1.163 g – 0.899 g = 0.264 g<\/strong><\/p>\n\n\n\n
Step 2: Calculate the percent sulfate in the unknown sample for each trial.<\/h3>\n\n\n\n
To calculate the percent sulfate in the unknown, we first need to know the molar masses:<\/p>\n\n\n\n
\n
BaSO\u2084 (barium sulfate): Ba = 137.33 g\/mol, S = 32.07 g\/mol, O = 16.00 g\/mol Molar mass of BaSO\u2084 = 137.33 + 32.07 + (4 \u00d7 16.00) = 233.39 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
The percentage of sulfate (SO\u2084) in BaSO\u2084 is calculated as the mass of SO\u2084 divided by the mass of BaSO\u2084, multiplied by 100.<\/p>\n\n\n\n
\n
Molar mass of SO\u2084 = 32.07 + (4 \u00d7 16.00) = 96.07 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
So, the percent sulfate in BaSO\u2084 is:96.07233.39\u00d7100=41.16%\\frac{{96.07}}{{233.39}} \\times 100 = 41.16\\%233.3996.07\u200b\u00d7100=41.16%<\/p>\n\n\n\n
Now we can calculate the percent sulfate in the unknown sample for each trial.<\/p>\n\n\n\n
Trial 1:<\/h4>\n\n\n\n
\n
Mass of dry BaSO\u2084 = 0.296 g<\/li>\n\n\n\n
Percent sulfate in BaSO\u2084 = 41.16%<\/li>\n<\/ul>\n\n\n\n
Mass of dry BaSO\u2084 (Trial 1):<\/strong> 0.296 g<\/li>\n\n\n\n
Mass of dry BaSO\u2084 (Trial 2):<\/strong> 0.264 g<\/li>\n\n\n\n
Percent sulfate in unknown (Trial 1):<\/strong> 12.1%<\/li>\n\n\n\n
Percent sulfate in unknown (Trial 2):<\/strong> 10.9%<\/li>\n\n\n\n
Average percent sulfate in unknown:<\/strong> 11.5%<\/strong><\/li>\n<\/ul>\n\n\n\n
This calculation shows the concentration of sulfate in the unknown sample based on the barium sulfate precipitate formed during the experiment. The average value gives a reliable estimate of the sulfate content across both trials.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Mass of unknown transferred Mass of filter paper Mass of paper and dry BaSO, Trial 1 (Yours) 0.294g 0.907g 1.203g Trial 2 (Partners) 0.253g 0.899g 1.163g Give me the Calculations week 1 Mass of dry BasO Calculated percent sulfate in unknown AVERAGE PERCENT SULFATE The Correct Answer and Explanation is: To calculate the mass of […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-45824","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/45824","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=45824"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/45824\/revisions"}],"predecessor-version":[{"id":45826,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/45824\/revisions\/45826"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=45824"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=45824"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=45824"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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