{"id":188424,"date":"2025-02-07T03:23:38","date_gmt":"2025-02-07T03:23:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=188424"},"modified":"2025-02-07T03:23:41","modified_gmt":"2025-02-07T03:23:41","slug":"potassium-phosphate-k_3po_4-is-a-solid-at-room-temperature-and-is-soluble-in-water","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/07\/potassium-phosphate-k_3po_4-is-a-solid-at-room-temperature-and-is-soluble-in-water\/","title":{"rendered":"Potassium phosphate, K_{3}PO_{4} is a solid at room temperature and is soluble in water"},"content":{"rendered":"\n

Potassium phosphate, K_{3}P<\/em>O_{4} is a solid at room temperature and is soluble in water. Which of the following statements is correct?
Select one:
a. K_{3}P<\/em>O_{4} is an electrolyte.
b. K ^ + and P O 4 ^ 3- ions are solvated by water.
c. The solubility of K_{3}P<\/em>O_{4} will increase with increasing temperature.
d. All of the above are correct.
13 Saline solutions (NaCl in water) used to deliver intravenous drugs are 0.89% * (w \/ v) . What mass of NaCl would be needed to prepare 500.0 mL of such a solution?
Select one:
Oa. 0.45 g
b. 0.89 g
Oc. 4.5 g
d. 8.9 g<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

Question 1: Potassium phosphate solubility and properties<\/h3>\n\n\n\n

The correct answer is:<\/p>\n\n\n\n

d. All of the above are correct.<\/strong><\/p>\n\n\n\n

Explanation:<\/p>\n\n\n\n

    \n
  • a. K\u2083PO\u2084 is an electrolyte<\/strong>: K\u2083PO\u2084 is an electrolyte because it dissociates into ions when it dissolves in water. In this case, it dissociates into K\u207a (potassium) ions and PO\u2084\u00b3\u207b (phosphate) ions. These ions conduct electricity in solution, which is the defining characteristic of an electrolyte.<\/li>\n\n\n\n
  • b. K\u207a and PO\u2084\u00b3\u207b ions are solvated by water<\/strong>: When K\u2083PO\u2084 dissolves in water, the K\u207a and PO\u2084\u00b3\u207b ions become surrounded by water molecules, a process known as solvation. The positively charged K\u207a ions are solvated by the partial negative charge of the oxygen atoms in water, while the negatively charged PO\u2084\u00b3\u207b ions are solvated by the partial positive charges of the hydrogen atoms in water.<\/li>\n\n\n\n
  • c. The solubility of K\u2083PO\u2084 will increase with increasing temperature<\/strong>: Like most solid solutes, the solubility of K\u2083PO\u2084 increases with temperature. As temperature rises, the kinetic energy of the molecules increases, which makes it easier for the solute (K\u2083PO\u2084) to dissolve in the solvent (water).<\/li>\n<\/ul>\n\n\n\n

    Therefore, all of the statements are correct, and the answer is d<\/strong>.<\/p>\n\n\n\n

    \n\n\n\n

    Question 2: Saline solution mass calculation<\/h3>\n\n\n\n

    The correct answer is:<\/p>\n\n\n\n

    c. 4.5 g<\/strong><\/p>\n\n\n\n

    Explanation:
    We are asked to prepare a 0.89% (w\/v) NaCl solution, which means 0.89 grams of NaCl per 100 milliliters of solution.<\/p>\n\n\n\n

    To find the mass of NaCl needed to prepare 500.0 mL of solution, we can set up a simple calculation based on the percentage concentration:<\/p>\n\n\n\n

      \n
    1. Step 1: Convert the volume of solution to liters<\/strong>
      500.0 mL = 0.500 L.<\/li>\n\n\n\n
    2. Step 2: Use the formula for weight\/volume percent<\/strong>:
      [
      \\text{Mass of NaCl} = \\text{Concentration} \\times \\text{Volume of solution}
      ]
      The concentration is 0.89% w\/v, which means 0.89 grams of NaCl per 100 mL of solution. For 500.0 mL:
      [
      \\text{Mass of NaCl} = 0.89 \\, \\text{g\/100 mL} \\times 500.0 \\, \\text{mL} = 4.45 \\, \\text{g}
      ]
      This rounds to 4.5 g.<\/li>\n<\/ol>\n\n\n\n

      Thus, the correct answer is c. 4.5 g<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"

      Potassium phosphate, K_{3}PO_{4} is a solid at room temperature and is soluble in water. Which of the following statements is correct?Select one:a. K_{3}PO_{4} is an electrolyte.b. K ^ + and P O 4 ^ 3- ions are solvated by water.c. The solubility of K_{3}PO_{4} will increase with increasing temperature.d. All of the above are correct.13 […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-188424","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188424","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=188424"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188424\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=188424"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=188424"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=188424"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}