{"id":5790,"date":"2023-08-24T19:14:20","date_gmt":"2023-08-25T00:14:20","guid":{"rendered":"https:\/\/staging.advancedrenaleducation.com\/wparep\/?post_type=article&#038;p=5790"},"modified":"2025-05-09T12:05:26","modified_gmt":"2025-05-09T17:05:26","slug":"concentracion-peso-atomico-y-molaridad-y-ley-de-avogadro-sp","status":"publish","type":"article","link":"https:\/\/staging.advancedrenaleducation.com\/wparep\/article\/concentracion-peso-atomico-y-molaridad-y-ley-de-avogadro-sp\/","title":{"rendered":"Concentraci\u00f3n, peso at\u00f3mico y molaridad y ley de Avogadro"},"content":{"rendered":"<h3><strong>Concentraci\u00f3n<\/strong><\/h3>\n<p>Las unidades de medida de una cantidad de sustancia se informan convenientemente como concentraci\u00f3n, que es masa por unidad de volumen. La unidad de volumen elegida suele ser una apropiada para la concentraci\u00f3n esperada de la sustancia o para un volumen que tenga sentido fisiol\u00f3gico: gramo\/litro (g\/l), milimol\/litro (mmol\/l), miligramo\/mililitro (mg\/ml).<\/p>\n<p>Si conocemos la concentraci\u00f3n de una sustancia (masa \/ volumen) y conocemos el volumen total de disolvente en el que se disuelve la sustancia (soluto) (volumen), se deduce que la masa total de soluto est\u00e1 dada por<br \/>\n<strong>concentraci\u00f3n (masa\/volumen) x volumen total = masa total<\/strong><\/p>\n<p>De manera similar, conocer la masa total y la concentraci\u00f3n da el volumen total de solvente como<br \/>\n<strong>masa total \uf0a4 concentraci\u00f3n (masa\/volumen) = volumen total<\/strong><\/p>\n<p>Y, dada la masa total y el volumen total, se obtiene un resultado para la concentraci\u00f3n como<br \/>\n<strong>masa total \uf0a4 volumen total = concentraci\u00f3n<\/strong><\/p>\n<h3>Peso at\u00f3mico y molaridad<\/h3>\n<p>El peso at\u00f3mico de una sustancia es un n\u00famero asignado que permite comparar las masas relativas (pesos) de los diferentes elementos. Por definici\u00f3n, a un \u00e1tomo de ox\u00edgeno se le asigna un &#8220;peso&#8221; de 16, y los pesos at\u00f3micos de los otros elementos se determinan en relaci\u00f3n con el del ox\u00edgeno. En una mol\u00e9cula, es decir, una sustancia que contiene dos o m\u00e1s \u00e1tomos diferentes, el peso molecular es igual a la suma de los pesos at\u00f3micos de los \u00e1tomos individuales. Por ejemplo, el peso molecular del agua (H2O) es 18 ([2 x 1] + 16).<\/p>\n<p>Un mol (mol) de cualquier sustancia se define como el peso molecular (o at\u00f3mico) de esa sustancia en gramos. De manera similar, un milimol (mmol) es igual a una mil\u00e9sima parte de un mol o el peso molecular (o at\u00f3mico) en miligramos.<\/p>\n<p>El peso at\u00f3mico del sodio (Na+) es 23. Por lo tanto, para Na+,<\/p>\n<p><strong>23 g = 1 mol<\/strong><\/p>\n<p><strong>23 mg =\u00a01 mmol <\/strong><\/p>\n<p><strong>23 mg de Na+ en 1 litro de agua = concentraci\u00f3n de Na+ ([Na+]) de 1 mmol\/l.<\/strong><\/p>\n<h3>Ley de Avogadro<\/h3>\n<p>La Ley de Avogadro establece que 1 mol de cualquier sustancia no disociable (una sustancia que no se puede reducir m\u00e1s a unidades componentes) contiene el mismo n\u00famero de part\u00edculas (aproximadamente 6,02 x 1023 = n\u00famero de Avogadro).<\/p>\n<p>As\u00ed, 1 mmol de Na+ contiene el mismo n\u00famero de \u00e1tomos que 1 mmol de Cl<sup>&#8211;<\/sup> aunque el primero pesa 23 mg y el segundo pesa 35,5 mg. Sin embargo, 1 mmol de NaCl (58,5 mg) se disocia en gran medida en iones Na+ y C<sup>l-<\/sup> y, por lo tanto, contiene casi el doble de part\u00edculas.<\/p>\n<p>La concentraci\u00f3n de mol\u00e9culas no cargadas, por ejemplo, glucosa y urea, tambi\u00e9n se puede medir en milimoles por litro y este es com\u00fanmente el caso cuando se usa el Systeme International (unidades SI). Sin embargo, en otros lugares, se miden m\u00e1s com\u00fanmente en el laboratorio cl\u00ednico como miligramos por decilitro (mg \/ dl o mg%). El peso molecular (peso molecular) de la glucosa es 180. En consecuencia, una concentraci\u00f3n de glucosa de 180 mg \/ l (o 18 mg \/ dl) es igual a 1 mmol\/l. Para convertir de miligramos por decilitro a milimoles por litro, se puede utilizar la siguiente f\u00f3rmula:<\/p>\n<p><strong>mmol\/l = (mg\/dl x 10) \u00f7 peso mol)<\/strong><\/p>\n<p>&nbsp;<\/p>\n<p class=\"ArEPheader2\" style=\"text-align: left;\" align=\"left\"><span style=\"font-weight: normal;\">P\/N 101820-01S Rev B 02\/2023<\/span><\/p>\n<div class=\"vcex-spacing\" style=\"height:30px\"><\/div>\n","protected":false},"featured_media":0,"template":"","format":"standard","meta":{"_acf_changed":false},"categories":[274],"tags":[222],"language":[42],"articles":[231],"class_list":["post-5790","article","type-article","status-publish","format-standard","hentry","category-articulos","tag-numbers-sp","language-spanish","articles-erc-ert","entry","no-media"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v26.2 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Concentraci\u00f3n, peso at\u00f3mico y molaridad y ley de Avogadro - Advanced Renal Education Program<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/staging.advancedrenaleducation.com\/wparep\/article\/concentracion-peso-atomico-y-molaridad-y-ley-de-avogadro-sp\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Concentraci\u00f3n, peso at\u00f3mico y molaridad y ley de Avogadro - Advanced Renal Education Program\" \/>\n<meta property=\"og:description\" content=\"Concentraci\u00f3n Las unidades de medida de una cantidad de sustancia se informan convenientemente como concentraci\u00f3n, que es masa por unidad de volumen. 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