{"id":84665,"date":"2025-06-01T02:44:55","date_gmt":"2025-06-01T02:44:55","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=84665"},"modified":"2025-06-01T02:44:55","modified_gmt":"2025-06-01T02:44:55","slug":"the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/","title":{"rendered":"The molecular mass of sulphuric acid is 98. If 49 g of the acid is dis"},"content":{"rendered":"

The molecular mass of sulphuric acid is 98. If 49 g of the acid is dissolved in water to make one litre of solution, what will be the strength of the acid?<\/p>\n

[amp_mcq option1=”Two normal” option2=”One normal” option3=”0\u00b75 normal” option4=”Four normal” correct=”option2″]<\/p>\n

\n
\n
This question was previously asked in<\/div>\n
UPSC CDS-1 – 2017<\/div>\n<\/div>\n
Download PDF<\/a>Attempt Online<\/a><\/div>\n<\/div>\n
\nThe molecular mass of sulfuric acid (H\u2082SO\u2084) is 98 g\/mol. 49 g of H\u2082SO\u2084 is dissolved in water to make 1 litre of solution.
\nNumber of moles of H\u2082SO\u2084 = Mass \/ Molar mass = 49 g \/ 98 g\/mol = 0.5 mol.
\nThe molarity of the solution is Moles \/ Volume (L) = 0.5 mol \/ 1 L = 0.5 M.
\nNormality (N) is defined as Molarity (M) multiplied by the n-factor (equivalents per mole). For sulfuric acid acting as an acid, it has two acidic protons (H\u207a) that can be donated, so its n-factor is 2.
\nNormality = Molarity \u00d7 n-factor = 0.5 M \u00d7 2 = 1 N.
\nThe strength of the acid solution is one normal.
\n<\/section>\n
\nNormality is a measure of concentration defined as the number of gram equivalents of solute per litre of solution. For acids, the gram equivalent weight is the molecular weight divided by the number of acidic protons per molecule.
\n<\/section>\n
\nSulfuric acid is a strong diprotic acid, meaning it can donate two protons in acid-base reactions. Its equivalent weight for neutralization reactions is Molecular Weight \/ 2 = 98 \/ 2 = 49 g\/equivalent. Therefore, 49 g of H\u2082SO\u2084 in 1 litre is 1 Normal.
\n<\/section>\n","protected":false},"excerpt":{"rendered":"

The molecular mass of sulphuric acid is 98. If 49 g of the acid is dissolved in water to make one litre of solution, what will be the strength of the acid? [amp_mcq option1=”Two normal” option2=”One normal” option3=”0\u00b75 normal” option4=”Four normal” correct=”option2″] This question was previously asked in UPSC CDS-1 – 2017 Download PDFAttempt Online … <\/p>\n

Detailed SolutionThe molecular mass of sulphuric acid is 98. If 49 g of the acid is dis<\/span><\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1087],"tags":[1101,1202,1096],"class_list":["post-84665","post","type-post","status-publish","format-standard","hentry","category-upsc-cds-1","tag-1101","tag-acid-base-and-salt","tag-chemistry","no-featured-image-padding"],"yoast_head":"\nThe molecular mass of sulphuric acid is 98. If 49 g of the acid is dis<\/title>\n<meta name=\"description\" content=\"The molecular mass of sulfuric acid (H\u2082SO\u2084) is 98 g\/mol. 49 g of H\u2082SO\u2084 is dissolved in water to make 1 litre of solution. Number of moles of H\u2082SO\u2084 = Mass \/ Molar mass = 49 g \/ 98 g\/mol = 0.5 mol. The molarity of the solution is Moles \/ Volume (L) = 0.5 mol \/ 1 L = 0.5 M. Normality (N) is defined as Molarity (M) multiplied by the n-factor (equivalents per mole). For sulfuric acid acting as an acid, it has two acidic protons (H\u207a) that can be donated, so its n-factor is 2. Normality = Molarity \u00d7 n-factor = 0.5 M \u00d7 2 = 1 N. The strength of the acid solution is one normal. Normality is a measure of concentration defined as the number of gram equivalents of solute per litre of solution. For acids, the gram equivalent weight is the molecular weight divided by the number of acidic protons per molecule.\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"The molecular mass of sulphuric acid is 98. If 49 g of the acid is dis\" \/>\n<meta property=\"og:description\" content=\"The molecular mass of sulfuric acid (H\u2082SO\u2084) is 98 g\/mol. 49 g of H\u2082SO\u2084 is dissolved in water to make 1 litre of solution. Number of moles of H\u2082SO\u2084 = Mass \/ Molar mass = 49 g \/ 98 g\/mol = 0.5 mol. The molarity of the solution is Moles \/ Volume (L) = 0.5 mol \/ 1 L = 0.5 M. Normality (N) is defined as Molarity (M) multiplied by the n-factor (equivalents per mole). For sulfuric acid acting as an acid, it has two acidic protons (H\u207a) that can be donated, so its n-factor is 2. Normality = Molarity \u00d7 n-factor = 0.5 M \u00d7 2 = 1 N. The strength of the acid solution is one normal. Normality is a measure of concentration defined as the number of gram equivalents of solute per litre of solution. For acids, the gram equivalent weight is the molecular weight divided by the number of acidic protons per molecule.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T02:44:55+00:00\" \/>\n<meta name=\"author\" content=\"rawan239\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"rawan239\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"1 minute\" \/>\n<!-- \/ Yoast SEO Premium plugin. -->","yoast_head_json":{"title":"The molecular mass of sulphuric acid is 98. If 49 g of the acid is dis","description":"The molecular mass of sulfuric acid (H\u2082SO\u2084) is 98 g\/mol. 49 g of H\u2082SO\u2084 is dissolved in water to make 1 litre of solution. Number of moles of H\u2082SO\u2084 = Mass \/ Molar mass = 49 g \/ 98 g\/mol = 0.5 mol. The molarity of the solution is Moles \/ Volume (L) = 0.5 mol \/ 1 L = 0.5 M. Normality (N) is defined as Molarity (M) multiplied by the n-factor (equivalents per mole). For sulfuric acid acting as an acid, it has two acidic protons (H\u207a) that can be donated, so its n-factor is 2. Normality = Molarity \u00d7 n-factor = 0.5 M \u00d7 2 = 1 N. The strength of the acid solution is one normal. Normality is a measure of concentration defined as the number of gram equivalents of solute per litre of solution. For acids, the gram equivalent weight is the molecular weight divided by the number of acidic protons per molecule.","robots":{"index":"index","follow":"follow","max-snippet":"max-snippet:-1","max-image-preview":"max-image-preview:large","max-video-preview":"max-video-preview:-1"},"canonical":"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/","og_locale":"en_US","og_type":"article","og_title":"The molecular mass of sulphuric acid is 98. If 49 g of the acid is dis","og_description":"The molecular mass of sulfuric acid (H\u2082SO\u2084) is 98 g\/mol. 49 g of H\u2082SO\u2084 is dissolved in water to make 1 litre of solution. Number of moles of H\u2082SO\u2084 = Mass \/ Molar mass = 49 g \/ 98 g\/mol = 0.5 mol. The molarity of the solution is Moles \/ Volume (L) = 0.5 mol \/ 1 L = 0.5 M. Normality (N) is defined as Molarity (M) multiplied by the n-factor (equivalents per mole). For sulfuric acid acting as an acid, it has two acidic protons (H\u207a) that can be donated, so its n-factor is 2. Normality = Molarity \u00d7 n-factor = 0.5 M \u00d7 2 = 1 N. The strength of the acid solution is one normal. Normality is a measure of concentration defined as the number of gram equivalents of solute per litre of solution. For acids, the gram equivalent weight is the molecular weight divided by the number of acidic protons per molecule.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T02:44:55+00:00","author":"rawan239","twitter_card":"summary_large_image","twitter_misc":{"Written by":"rawan239","Est. reading time":"1 minute"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"WebPage","@id":"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/","url":"https:\/\/exam.pscnotes.com\/mcq\/the-molecular-mass-of-sulphuric-acid-is-98-if-49-g-of-the-acid-is-dis\/","name":"The molecular mass of sulphuric acid is 98. If 49 g of the acid is dis","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T02:44:55+00:00","dateModified":"2025-06-01T02:44:55+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"The molecular mass of sulfuric acid (H\u2082SO\u2084) is 98 g\/mol. 49 g of H\u2082SO\u2084 is dissolved in water to make 1 litre of solution. Number of moles of H\u2082SO\u2084 = Mass \/ Molar mass = 49 g \/ 98 g\/mol = 0.5 mol. The molarity of the solution is Moles \/ Volume (L) = 0.5 mol \/ 1 L = 0.5 M. Normality (N) is defined as Molarity (M) multiplied by the n-factor (equivalents per mole). For sulfuric acid acting as an acid, it has two acidic protons (H\u207a) that can be donated, so its n-factor is 2. Normality = Molarity \u00d7 n-factor = 0.5 M \u00d7 2 = 1 N. The strength of the acid solution is one normal. Normality is a measure of concentration defined as the number of gram equivalents of solute per litre of solution. 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