How does the boiling point of a solvent change when a solute is dissolved in it give an example?

{"appState":{"pageLoadApiCallsStatus":true},"articleState":{"article":{"headers":{"creationTime":"2016-03-26T07:53:34+00:00","modifiedTime":"2021-07-23T17:55:04+00:00","timestamp":"2022-06-22T19:36:40+00:00"},"data":{"breadcrumbs":[{"name":"Academics & The Arts","_links":{"self":"//dummies-api.dummies.com/v2/categories/33662"},"slug":"academics-the-arts","categoryId":33662},{"name":"Science","_links":{"self":"//dummies-api.dummies.com/v2/categories/33756"},"slug":"science","categoryId":33756},{"name":"Chemistry","_links":{"self":"//dummies-api.dummies.com/v2/categories/33762"},"slug":"chemistry","categoryId":33762}],"title":"How to Elevate and Calculate Boiling Points of Solvents","strippedTitle":"how to elevate and calculate boiling points of solvents","slug":"how-to-elevate-and-calculate-boiling-points-of-solvents","canonicalUrl":"","seo":{"metaDescription":"A solvent's boiling point tends to increase when an impurity, a solute, is added to it. In fact, the more solute that's added, the greater the increase.","noIndex":0,"noFollow":0},"content":"<i>Boiling point elevation</i> refers to the tendency of a solvent's boiling point to increase when an impurity (a solute) is added to it. In fact, the more solute that is added, the greater the change in the boiling point.\r\n\r\nBoiling point elevations are directly proportional to the molality of a solution, but chemists have found that some solvents are more susceptible to this change than others. The formula for the change in the boiling point of a solution, therefore, contains a proportionality constant, abbreviated <i>K</i>_b, which is a property determined experimentally and must be read from a table such as the one below.\r\n<table><caption>Common <i>K</i>_b Values</caption>\r\n<tbody>\r\n<tr>\r\n<th>Solvent</th>\r\n<th><i>K</i>_b in Degrees C/<i>m</i></th>\r\n<th>Boiling Point in Degrees C</th>\r\n</tr>\r\n<tr>\r\n<td>Acetic acid</td>\r\n<td>3.07</td>\r\n<td>118.1</td>\r\n</tr>\r\n<tr>\r\n<td>Benzene</td>\r\n<td>2.53</td>\r\n<td>80.1</td>\r\n</tr>\r\n<tr>\r\n<td>Camphor</td>\r\n<td>5.95</td>\r\n<td>204.0</td>\r\n</tr>\r\n<tr>\r\n<td>Carbon tetrachloride</td>\r\n<td>4.95</td>\r\n<td>76.7</td>\r\n</tr>\r\n<tr>\r\n<td>Cyclohexane</td>\r\n<td>2.79</td>\r\n<td>80.7</td>\r\n</tr>\r\n<tr>\r\n<td>Ethanol</td>\r\n<td>1.19</td>\r\n<td>78.4</td>\r\n</tr>\r\n<tr>\r\n<td>Phenol</td>\r\n<td>3.56</td>\r\n<td>181.7</td>\r\n</tr>\r\n<tr>\r\n<td>Water</td>\r\n<td>0.512</td>\r\n<td>100.0</td>\r\n</tr>\r\n</tbody>\r\n</table>\r\n<h2 id=\"tab1\" >Here's the formula</h2>\r\nThe formula for the boiling point elevation is\r\n\r\n<img src=\"//sg.cdnki.com/how-does-the-boiling-point-of-a-solvent-change-when-a-solute-is-dissolved-in-it-give-an-example---aHR0cHM6Ly93d3cuZHVtbWllcy5jb20vd3AtY29udGVudC91cGxvYWRzLzQ3NjY2Ny5pbWFnZTAuanBn.webp\" alt=\"image0.jpg\" width=\"120\" height=\"27\" />\r\n\r\nwhere <i>m</i> is molality. Note the use of the Greek letter delta in the formula to indicate that you're calculating a <i>change in</i> the boiling point, not the boiling point itself. You need to add this number to the boiling point of the pure solvent to get the boiling point of the solution. The units of <i>K</i>_b are typically given in degrees Celsius per molality.\r\n<h2 id=\"tab2\" >What causes boiling points to rise?</h2>\r\nBoiling point elevations are a result of the attraction between solvent and solute particles in a solution. Colligative properties such as boiling point elevation depend on only the number of particles <i>in solution.</i> Adding solute particles increases these intermolecular attractions because more particles are around to attract one another. To boil, solvent particles must therefore achieve a greater kinetic energy to overcome this extra attractive force, which translates into a higher boiling point.\r\n<h2 id=\"tab3\" >Here's a sample problem</h2>\r\n<b>Try this example: </b>What is the boiling point of a solution containing 45.2 g of menthol (C₁₀H₂₀O) dissolved in 350 g of acetic acid?\r\n\r\nThe problem asks for the boiling point of the solution, so you know that first you have to calculate the boiling point elevation. This means you need to know the molality of the solution and the <i>K</i>_b value of the solvent (acetic acid). The table tells you that the <i>K</i>_b of acetic acid is 3.07 degrees C/<i>m</i>. To calculate the molality, you must convert 45.2 g of menthol to moles:\r\n\r\n<img src=\"//sg.cdnki.com/how-does-the-boiling-point-of-a-solvent-change-when-a-solute-is-dissolved-in-it-give-an-example---aHR0cHM6Ly93d3cuZHVtbWllcy5jb20vd3AtY29udGVudC91cGxvYWRzLzQ3NjY2OC5pbWFnZTEuanBn.webp\" alt=\"image1.jpg\" width=\"680\" height=\"65\" />\r\n\r\nYou can now calculate the molality of the solution, taking care to convert grams of acetic acid to kilograms:\r\n\r\n<img src=\"//sg.cdnki.com/how-does-the-boiling-point-of-a-solvent-change-when-a-solute-is-dissolved-in-it-give-an-example---aHR0cHM6Ly93d3cuZHVtbWllcy5jb20vd3AtY29udGVudC91cGxvYWRzLzQ3NjY2OS5pbWFnZTIuanBn.webp\" alt=\"image2.jpg\" width=\"391\" height=\"54\" />\r\n\r\nNow that you have molality, you can plug it and your <i>K</i>_b value into the formula to find the change in boiling point:\r\n\r\n<img src=\"//sg.cdnki.com/how-does-the-boiling-point-of-a-solvent-change-when-a-solute-is-dissolved-in-it-give-an-example---aHR0cHM6Ly93d3cuZHVtbWllcy5jb20vd3AtY29udGVudC91cGxvYWRzLzQ3NjY3MC5pbWFnZTMuanBn.webp\" alt=\"image3.jpg\" width=\"373\" height=\"49\" />\r\n\r\nYou're not quite done, because the problem asks for the boiling point of the solution, not the change in the boiling point. Luckily, the last step is just simple arithmetic. You must add your\r\n\r\n<img src=\"//sg.cdnki.com/how-does-the-boiling-point-of-a-solvent-change-when-a-solute-is-dissolved-in-it-give-an-example---aHR0cHM6Ly93d3cuZHVtbWllcy5jb20vd3AtY29udGVudC91cGxvYWRzLzQ3NjY3MS5pbWFnZTQucG5n.webp\" alt=\"image4.png\" width=\"31\" height=\"24\" />\r\n\r\nto the boiling point of pure acetic acid, which, according to the table, is 118.1 degrees Celsius. This gives you a final boiling point of\r\n\r\n<img src=\"//sg.cdnki.com/how-does-the-boiling-point-of-a-solvent-change-when-a-solute-is-dissolved-in-it-give-an-example---aHR0cHM6Ly93d3cuZHVtbWllcy5jb20vd3AtY29udGVudC91cGxvYWRzLzQ3NjY3Mi5pbWFnZTUuanBn.webp\" alt=\"image5.jpg\" width=\"285\" height=\"21\" />\r\n\r\nfor the solution.","description":"<i>Boiling point elevation</i> refers to the tendency of a solvent's boiling point to increase when an impurity (a solute) is added to it. In fact, the more solute that is added, the greater the change in the boiling point.\r\n\r\nBoiling point elevations are directly proportional to the molality of a solution, but chemists have found that some solvents are more susceptible to this change than others. The formula for the change in the boiling point of a solution, therefore, contains a proportionality constant, abbreviated <i>K</i>_b, which is a property determined experimentally and must be read from a table such as the one below.\r\n<table><caption>Common <i>K</i>_b Values</caption>\r\n<tbody>\r\n<tr>\r\n<th>Solvent</th>\r\n<th><i>K</i>_b in Degrees C/<i>m</i></th>\r\n<th>Boiling Point in Degrees C</th>\r\n</tr>\r\n<tr>\r\n<td>Acetic acid</td>\r\n<td>3.07</td>\r\n<td>118.1</td>\r\n</tr>\r\n<tr>\r\n<td>Benzene</td>\r\n<td>2.53</td>\r\n<td>80.1</td>\r\n</tr>\r\n<tr>\r\n<td>Camphor</td>\r\n<td>5.95</td>\r\n<td>204.0</td>\r\n</tr>\r\n<tr>\r\n<td>Carbon tetrachloride</td>\r\n<td>4.95</td>\r\n<td>76.7</td>\r\n</tr>\r\n<tr>\r\n<td>Cyclohexane</td>\r\n<td>2.79</td>\r\n<td>80.7</td>\r\n</tr>\r\n<tr>\r\n<td>Ethanol</td>\r\n<td>1.19</td>\r\n<td>78.4</td>\r\n</tr>\r\n<tr>\r\n<td>Phenol</td>\r\n<td>3.56</td>\r\n<td>181.7</td>\r\n</tr>\r\n<tr>\r\n<td>Water</td>\r\n<td>0.512</td>\r\n<td>100.0</td>\r\n</tr>\r\n</tbody>\r\n</table>\r\n<h2 id=\"tab1\" >Here's the formula</h2>\r\nThe formula for the boiling point elevation is\r\n\r\n<img src=\"//www.dummies.com/wp-content/uploads/476667.image0.jpg\" alt=\"image0.jpg\" width=\"120\" height=\"27\" />\r\n\r\nwhere <i>m</i> is molality. Note the use of the Greek letter delta in the formula to indicate that you're calculating a <i>change in</i> the boiling point, not the boiling point itself. You need to add this number to the boiling point of the pure solvent to get the boiling point of the solution. The units of <i>K</i>_b are typically given in degrees Celsius per molality.\r\n<h2 id=\"tab2\" >What causes boiling points to rise?</h2>\r\nBoiling point elevations are a result of the attraction between solvent and solute particles in a solution. Colligative properties such as boiling point elevation depend on only the number of particles <i>in solution.</i> Adding solute particles increases these intermolecular attractions because more particles are around to attract one another. To boil, solvent particles must therefore achieve a greater kinetic energy to overcome this extra attractive force, which translates into a higher boiling point.\r\n<h2 id=\"tab3\" >Here's a sample problem</h2>\r\n<b>Try this example: </b>What is the boiling point of a solution containing 45.2 g of menthol (C₁₀H₂₀O) dissolved in 350 g of acetic acid?\r\n\r\nThe problem asks for the boiling point of the solution, so you know that first you have to calculate the boiling point elevation. This means you need to know the molality of the solution and the <i>K</i>_b value of the solvent (acetic acid). The table tells you that the <i>K</i>_b of acetic acid is 3.07 degrees C/<i>m</i>. To calculate the molality, you must convert 45.2 g of menthol to moles:\r\n\r\n<img src=\"//www.dummies.com/wp-content/uploads/476668.image1.jpg\" alt=\"image1.jpg\" width=\"680\" height=\"65\" />\r\n\r\nYou can now calculate the molality of the solution, taking care to convert grams of acetic acid to kilograms:\r\n\r\n<img src=\"//www.dummies.com/wp-content/uploads/476669.image2.jpg\" alt=\"image2.jpg\" width=\"391\" height=\"54\" />\r\n\r\nNow that you have molality, you can plug it and your <i>K</i>_b value into the formula to find the change in boiling point:\r\n\r\n<img src=\"//www.dummies.com/wp-content/uploads/476670.image3.jpg\" alt=\"image3.jpg\" width=\"373\" height=\"49\" />\r\n\r\nYou're not quite done, because the problem asks for the boiling point of the solution, not the change in the boiling point. Luckily, the last step is just simple arithmetic. You must add your\r\n\r\n<img src=\"//www.dummies.com/wp-content/uploads/476671.image4.png\" alt=\"image4.png\" width=\"31\" height=\"24\" />\r\n\r\nto the boiling point of pure acetic acid, which, according to the table, is 118.1 degrees Celsius. This gives you a final boiling point of\r\n\r\n<img src=\"//www.dummies.com/wp-content/uploads/476672.image5.jpg\" alt=\"image5.jpg\" width=\"285\" height=\"21\" />\r\n\r\nfor the solution.","blurb":"","authors":[{"authorId":9161,"name":"Peter J. Mikulecky","slug":"peter-j-mikulecky","description":"Peter J. Mikulecky, PhD, is a writer, technical writer, and educator.","_links":{"self":"//dummies-api.dummies.com/v2/authors/9161"}},{"authorId":9160,"name":"Chris Hren","slug":"chris-hren","description":" <p><b>Christopher Hren</b> is a high school chemistry teacher and former track and football coach. <b>Peter J. Mikulecky, PhD,</b> teaches biology and chemistry at Fusion Learning Center and Fusion Academy. ","_links":{"self":"//dummies-api.dummies.com/v2/authors/9160"}}],"primaryCategoryTaxonomy":{"categoryId":33762,"title":"Chemistry","slug":"chemistry","_links":{"self":"//dummies-api.dummies.com/v2/categories/33762"}},"secondaryCategoryTaxonomy":{"categoryId":0,"title":null,"slug":null,"_links":null},"tertiaryCategoryTaxonomy":{"categoryId":0,"title":null,"slug":null,"_links":null},"trendingArticles":null,"inThisArticle":[{"label":"Here's the formula","target":"#tab1"},{"label":"What causes boiling points to rise?","target":"#tab2"},{"label":"Here's a sample problem","target":"#tab3"}],"relatedArticles":{"fromBook":[{"articleId":253707,"title":"How to Make Unit Conversions","slug":"make-unit-conversions","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/253707"}},{"articleId":251836,"title":"How to Convert between Units Using Conversion Factors","slug":"convert-units-using-conversion-factors","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/251836"}},{"articleId":251010,"title":"How to Build Derived Units from Base Units","slug":"build-derived-units-base-units","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/251010"}},{"articleId":251005,"title":"How to Do Arithmetic with Significant Figures","slug":"arithmetic-significant-figures","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/251005"}},{"articleId":250992,"title":"How to Add and Subtract with Exponential Notation","slug":"add-subtract-exponential-notation","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/250992"}}],"fromCategory":[{"articleId":253707,"title":"How to Make Unit Conversions","slug":"make-unit-conversions","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/253707"}},{"articleId":251836,"title":"How to Convert between Units Using Conversion Factors","slug":"convert-units-using-conversion-factors","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/251836"}},{"articleId":251010,"title":"How to Build Derived Units from Base Units","slug":"build-derived-units-base-units","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/251010"}},{"articleId":251005,"title":"How to Do Arithmetic with Significant Figures","slug":"arithmetic-significant-figures","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/251005"}},{"articleId":250992,"title":"How to Add and Subtract with Exponential Notation","slug":"add-subtract-exponential-notation","categoryList":["academics-the-arts","science","chemistry"],"_links":{"self":"//dummies-api.dummies.com/v2/articles/250992"}}]},"hasRelatedBookFromSearch":false,"relatedBook":{"bookId":282070,"slug":"chemistry-workbook-for-dummies-with-online-practice-3rd-edition","isbn":"9781119357452","categoryList":["academics-the-arts","science","chemistry"],"amazon":{"default":"//www.amazon.com/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20","ca":"//www.amazon.ca/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20","indigo_ca":"//www.tkqlhce.com/click-9208661-13710633?url=//www.chapters.indigo.ca/en-ca/books/product/1119357454-item.html&cjsku=978111945484","gb":"//www.amazon.co.uk/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20","de":"//www.amazon.de/gp/product/1119357454/ref=as_li_tl?ie=UTF8&tag=wiley01-20"},"image":{"src":"//www.dummies.com/wp-content/uploads/chemistry-workbook-for-dummies-3rd-edition-cover-9781119357452-204x255.jpg","width":204,"height":255},"title":"Chemistry Workbook For Dummies with Online Practice","testBankPinActivationLink":"","bookOutOfPrint":false,"authorsInfo":"<p><b data-author-id=\"9160\">Christopher Hren</b> is a high school chemistry teacher and former track and football coach. <b data-author-id=\"34803\">Peter J. 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