{"id":4735,"date":"2024-10-06T13:01:41","date_gmt":"2024-10-06T13:01:41","guid":{"rendered":"https:\/\/workhouse.sweetdishy.com\/?p=4735"},"modified":"2024-10-06T13:01:42","modified_gmt":"2024-10-06T13:01:42","slug":"heats-of-solution-dissolution-and-mixing","status":"publish","type":"post","link":"https:\/\/workhouse.sweetdishy.com\/index.php\/2024\/10\/06\/heats-of-solution-dissolution-and-mixing\/","title":{"rendered":"Heats of Solution, Dissolution, and Mixing"},"content":{"rendered":"\n

Up to this chapter we have assumed that when a stream consists of several components, the total properties of the stream are the appropriately weighted sum of the properties of the individual components. For such ideal solutions,<\/strong> we could write down for the heat capacity of an ideal mixture, for example,Cpmixture=xACpA+xBCpB+xCCpC+…<\/p>\n\n\n\n

or, for the enthalpy,\u0394H^mixture =xA\u0394H^A+xB\u0394H^B+xC\u0394H^C+\u22ef<\/p>\n\n\n\n

In particular, mixtures of gases have been treated as ideal solutions.<\/p>\n\n\n\n

However, you must take into consideration other types of mixtures. You can prepare various kinds of binary solutions or mixtures:<\/p>\n\n\n\n

    \n
  1. a.<\/strong> gas-gas<\/li>\n\n\n\n
  2. b.<\/strong> gas-liquid<\/li>\n\n\n\n
  3. c.<\/strong> gas-solid<\/li>\n\n\n\n
  4. d.<\/strong> liquid-liquid<\/li>\n\n\n\n
  5. e.<\/strong> liquid-solid<\/li>\n\n\n\n
  6. f.<\/strong> solid-solid<\/li>\n<\/ol>\n\n\n\n

    You can ignore the energy changes that occur on mixing for cases a, c, and f. They are negligible. The other mixtures constitute\u00a0real solutions.<\/strong>When a gaseous or solid\u00a0solute<\/strong>(the compound to be dissolved) is mixed with a liquid\u00a0solvent<\/strong>(the compound in which the solute is dissolved), the energy effect that occurs is referred to as the\u00a0heat<\/strong>(really\u00a0enthalpy<\/strong>)\u00a0of solution.<\/strong>When a liquid is mixed with a liquid, the energy effect is called the\u00a0heat (enthalpy) of mixing.<\/strong>The negative of the heat of solution or mixing is the\u00a0heat (enthalpy) of dissolution.<\/strong><\/p>\n\n\n\n

    The heat of solution can be positive (endothermic) or negative (exothermic). Examine\u00a0Figure 12.1, which shows the relative enthalpy values of a mixture of a fluorocarbon (C6<\/sub>F6<\/sub>) in benzene (C6<\/sub>H6<\/sub>).<\/p>\n\n\n\n

    You can treat heats of solution\/mixing in the same way you treat chemical reactions. In the energy balance, you can (a) merge the heats of solution\/mixing of the compounds in the system with the heats of formation, or (b) consolidate the effects of the heats of solution\/mixing in one lumped term analogous to a heat of reaction term. For example, let us represent the solution of 1 g mol of HCl(g) into 5 g mol of by the following chemical equation:<\/p>\n\n\n\n

    HCl(g) +5H2<\/sub>O(l) \u2192HCl[5H2<\/sub>O]<\/p>\n\n\n\n

    \"A
    Figure 12.1<\/strong> Relative enthalpy change on mixing C6<\/sub>F6<\/sub> in C6<\/sub>H6<\/sub> at 25\u00b0C<\/figcaption><\/figure>\n\n\n\n

    If you carry out experiments to measure the heat transfer from an apparatus at a constant 25\u00b0C and 1 atm by successively adding water to HCl, and arrange the experiments so that the energy balance reduces to\u00a0Q<\/em>\u00a0= \u0394H,<\/em>\u00a0then the values of \u0394H<\/em>\u00a0would be the tabulation in the third column of\u00a0Table 12.1. (The values incorporate a slight adjustment in the measured values of\u00a0Q<\/em>\u00a0at the vapor pressure of the solution to adjust them to 1 atm, the standard state.) If you cumulate each incremental change in \u0394H<\/em>, you would obtain the fourth column in\u00a0Table 12.1.\u00a0Appendix I\u00a0on the CD that accompanies this book contains other tables listing the heats of solution for common compounds.\u00a0Table 12.1\u00a0shows that there are actually two concepts that incorporate the name \u201cheat of solution\u201d:<\/p>\n\n\n\n

      \n
    1. a.<\/strong> The incremental (differential) heat of solution,<\/strong> column 3<\/li>\n\n\n\n
    2. b.<\/strong> The integral heat of solution,<\/strong> column 4\u2014the heat of solution for the combination of 1 mole of HCl(g) with n<\/em> moles of H2<\/sub>O(I)<\/li>\n<\/ol>\n\n\n\n

      Usually \u201cheat of solution\u201d refers to concept b, and the enthalpy change is stated per mole of solute.<\/strong><\/p>\n\n\n\n

      Figure 12.2\u00a0is a plot of the values listed in column 4 of\u00a0Table 12.1. The asymptotic value of the heat of solution of HCl dissolved in an infinite amount of water is known as the\u00a0heat of solution at infinite dilution<\/strong>\u00a0(\u221275, 144 J\/g mol HCl).<\/p>\n\n\n\n

      If you want to calculate the heat of formation of any of the solutions of HCl(g) in all you have to do is add the heat of solution to the heat of formation of HCl(g), as shown in column 5 in\u00a0Table 12.1\u0394H^f,\u00a0solution\u00a0o=\u0394H^f,solute\u00a0o+\u0394H^solution\u00a0o<\/p>\n\n\n\n

      (12.1)<\/p>\n\n\n\n

      where\u00a0\u0394H^solution\u00a0o\u00a0is the integral heat of solution at standard conditions per mole of HCl, and\u00a0\u0394H^f,\u00a0solution\u00a0o\u00a0is the heat of formation of the solution itself per\u00a0mole of HCl. It is important to remember that\u00a0the heat of formation of the H2<\/sub>O does not enter into the calculation<\/strong>\u00a0in Equation (12.1); it is defined as zero for the process of solution. Tables in reference books usually list data for the heats of formation of solutions in the standard state rather than the heats of solution themselves. In the following processes and examples, we assume that the systems are open, steady-state, or, if closed, that the accumulation term in the energy balance is \u0394U<\/em>\u00a0= \u0394H<\/em>\u00a0so that we discuss only enthalpies.<\/p>\n\n\n\n

      Table 12.1 Heat of Solution Data at 25\u00b0C and 1 atm<\/strong><\/p>\n\n\n\n

      Composition<\/th>Total Moles H2<\/sub>O Added to 1 mole HCl<\/th>\u0394\u0124<\/em>o<\/sup> for Each Incremental Step (J\/g mol HCl)<\/th>Integral Heat of Solution (Cumulative \u0394\u0124<\/em>o<\/sup>) (J\/g mol HCI)<\/th>Heat of Formation \u0394H^fo (J\/g mol HCI)<\/th><\/tr><\/thead>
      HCl(g)<\/td>0<\/td><\/td><\/td>\u221292,311<\/td><\/tr>
      HCl[1H2<\/sub>O(aq)]<\/td>1<\/td>\u221226,225<\/td>\u221226,225<\/td>\u2212118,536<\/td><\/tr>
      HCl[2H2<\/sub>O(aq)]<\/td>2<\/td>\u221222,593<\/td>\u221248,818<\/td>\u2212141,129<\/td><\/tr>
      HCl[3H2<\/sub>O(aq)]<\/td>3<\/td>\u22128033<\/td>\u221256,851<\/td>\u2212149,161<\/td><\/tr>
      HCl[4H2<\/sub>O(aq)]<\/td>4<\/td>\u22124351<\/td>\u221261,202<\/td>\u2212153,513<\/td><\/tr>
      HCl[5H2<\/sub>O(aq)]<\/td>5<\/td>\u22122845<\/td>\u221264,047<\/td>\u2212156,358<\/td><\/tr>
      HCl[8H2<\/sub>O(aq)]<\/td>8<\/td>\u22124184<\/td>\u221268,231<\/td>\u2212160,542<\/td><\/tr>
      HCl[10H2<\/sub>O(aq)]<\/td>10<\/td>\u22121255<\/td>\u221269,486<\/td>\u2212161,797<\/td><\/tr>
      HCl[15H2<\/sub>O(aq)]<\/td>15<\/td>\u22121503<\/td>\u221270,989<\/td>\u2212163,300<\/td><\/tr>
      HCl[25H2<\/sub>O(aq)]<\/td>25<\/td>\u22121276<\/td>\u221272,265<\/td>\u2212164,576<\/td><\/tr>
      HCl[50H2<\/sub>O(aq)]<\/td>50<\/td>\u22121013<\/td>\u221273,278<\/td>\u2212165,589<\/td><\/tr>
      HCl[100H2<\/sub>O(aq)]<\/td>100<\/td>\u2212569<\/td>\u221273,847<\/td>\u2212166,158<\/td><\/tr>
      HCl[200H2<\/sub>O(aq)]<\/td>200<\/td>\u2212356<\/td>\u221274,203<\/td>\u2212166,514<\/td><\/tr>
      HCl[500H2<\/sub>O(aq)]<\/td>500<\/td>\u2212318<\/td>\u221274,521<\/td>\u2212166,832<\/td><\/tr>
      HCl[1000H2<\/sub>O(aq)]<\/td>1000<\/td>\u2212163<\/td>\u221274,684<\/td>\u2212166,995<\/td><\/tr>
      HCl[50,000H2<\/sub>O(aq)]<\/td>50,000<\/td>\u2212146<\/td>\u221275,077<\/td>\u2212167,388<\/td><\/tr>
      HCl[\u221eH2<\/sub>O]<\/td><\/td>\u221267<\/td>\u221275,144<\/td>\u2212167,455<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

      SOURCE: National Bureau of Standards Circular 500,<\/em> U.S. Government Printing Office, Washington, DC (1952).<\/p>\n\n\n\n

      You can treat a solution as a single compound in making calculations in an energy balance by using the property that enthalpies of solutions are state variables. One convenient procedure is to merge the heats of solution of a compound with the heats of formation, as indicated in column 5 of\u00a0Table 12.1\u00a0and by Equation (12.1). Then the specific enthalpy of a solution relative to S.C. would beH^solution\u200b(T)=\u0394H^f,\u00a0solution\u00a0o\u200b+[H^(T)\u2212H^(\u00a0S.C.\u00a0)]solution\u00a0<\/p>\n\n\n\n

      (12.2)<\/p>\n\n\n\n

      \"A
      Figure 12.2<\/strong> Integral heat of solution of HCl in water<\/figcaption><\/figure>\n\n\n\n

      where the term in the brackets represents the sensible heat of the solution itself (any phase change is unlikely).<\/p>\n\n\n\n

      For example, suppose you want to find the\u00a0\u0394H^solution\u00a0o\u00a0that occurs at S.C. when a solution of 1 g mol of HCl dissolved in 1 g mol of H2<\/sub>O is placed in an infinite amount of water. Use the data listed in column 5 of\u00a0Table 12.1, and subtract the enthalpy of the initial state from the enthalpy of the final state as follows:<\/p>\n\n\n\n

      (\u2212167,455) \u2212(\u2212118,536) =\u221248,911 J\/g mol HCl<\/p>\n\n\n\n

      As another example, consider a process in which a dilute solution of HCl is to be concentrated. Because enthalpy changes for heats of solution are state variables, you can easily look up the heats of formation of HCl solutions at their respective concentrations. Then you can calculate the enthalpy change between the final and initial states for a closed process, or the enthalpy change between the output and the input for a flow process. Thus, if you mix 1 mole of HCl[15H2<\/sub>O] and 1 mole of HCl[5H2<\/sub>O], you obtain 2 moles of HCl[10H2<\/sub>O], and the total enthalpy change at 25\u00b0C and 1 atm is<\/p>\n\n\n\n

      \u0394H<\/em>o<\/sup>=[2(\u221269,486)] \u2212[1(\u221270,989) +1(\u221264,047)]<\/p>\n\n\n\n

      =\u22123936 J<\/p>\n\n\n\n

      You would have to remove 3936 J to keep the temperature of the final mixture at 25\u00b0C.<\/p>\n\n\n\n

      We should mention that the solution of a hydrated salt such as CaCl2<\/sub>\u00b7 6H2<\/sub>O requires a little care in the calculations. If you mix the hydrated salt with water or a CaCl2<\/sub> solution, the procedure to calculate the enthalpy change is as follows: You first have to decompose (melt) the hydrated salt into a solid and water. Then you dissolve the total salt available into the total water available after the melting and solution. For example, from the data in problem 12.3, if 1 g mol of Na2<\/sub>CO3<\/sub>\u00b7 7H2<\/sub>O is dissolved in 8 g mol of the resulting solution contains 1 g mol of Na2<\/sub>CO3<\/sub> and 15 g mol of H2<\/sub>O. The melting step involves the following enthalpy change:Na2CO3\u22c57H2O(s)\u2003\u2009\u2192\u2003\u2009Na2CO3(s)\u2009\u2003+\u2003\u20097H2O(l)\u0394H^fo(kJ\/gmol):\u2003\u2009\u22123201.18\u2009\u22121130.92\u2009\u2212285.840<\/p>\n\n\n\n

      \u0394H<\/em>o<\/sup>=[7(\u2212285.840) +1(\u22121130.92)] \u2212[1(\u22123201.18)] = +69.38 kJ<\/p>\n\n\n\n

      The solution step isNa2CO3(s)\u2009 \u2003\u2009+ \u2003\u200915H2O(l) \u2003\u2192 \u2009\u2003Na2CO3[15H2O]\u0394H^fo(kJ\/gmol):\u22121130.92\u2003  \u2003\u2009\u20090   \u22121163.70<\/p>\n\n\n\n

      \u0394H<\/em>o<\/sup> = (\u22121163.70) \u2212 (\u22121130.92) = \u2212 32.78 kJ<\/p>\n\n\n\n

      The overall enthalpy change is 69.38 \u221232.78 =36.60 kJ.<\/p>\n\n\n\n

      Example 12.1 Application of Heat of Solution Data<\/strong><\/p>\n\n\n\n

      You are asked to prepare an ammonium hydroxide solution at 77\u00b0F by dissolving gaseous NH3<\/sub> in water. Calculate (a) the amount of cooling needed in British thermal units to prepare a 3.0% solution containing 1 lb mol of NH3<\/sub>, and (b) the amount of cooling needed in British thermal units to prepare 100 gal of a solution of 32.0% NH3<\/sub>.<\/p>\n\n\n\n

      Data: The following heat of solution data have been taken from NBS circular 500<\/em>.<\/p>\n\n\n\n

      Composition<\/strong><\/th>State<\/strong><\/th>\u2212\u0394H^fo (Btu\/lb mol)<\/strong><\/th>\u2212\u0394H^solno (Btu\/lb mol)<\/strong><\/th><\/tr><\/thead>
      <\/td>g<\/td>19,900<\/td>0<\/td><\/tr>
      1H2<\/sub>O<\/td>aq<\/td>32,600<\/td>12,700<\/td><\/tr>
      2H2<\/sub>O<\/td>aq<\/td>33,600<\/td>13,700<\/td><\/tr>
      3H2<\/sub>O<\/td>aq<\/td>34,000<\/td>14,100<\/td><\/tr>
      4H2<\/sub>O<\/td>aq<\/td>34,200<\/td>14,300<\/td><\/tr>
      5H2<\/sub>O<\/td>aq<\/td>34,350<\/td>14,450<\/td><\/tr>
      10H2<\/sub>O<\/td>aq<\/td>34,600<\/td>14,700<\/td><\/tr>
      20H2<\/sub>O<\/td>aq<\/td>34,700<\/td>14,800<\/td><\/tr>
      30H2<\/sub>O<\/td>aq<\/td>34,700<\/td>14,800<\/td><\/tr>
      40H2<\/sub>O<\/td>aq<\/td>34,700<\/td>14,800<\/td><\/tr>
      50H2<\/sub>O<\/td>aq<\/td>34,750<\/td>14,850<\/td><\/tr>
      100H2<\/sub>O<\/td>aq<\/td>34,750<\/td>14,850<\/td><\/tr>
      200H2<\/sub>O<\/td>aq<\/td>34,800<\/td>14,900<\/td><\/tr>
      \u221eH2<\/sub>O<\/td>aq<\/td>34,800<\/td>14,900<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

      Solution<\/strong><\/p>\n\n\n\n

      The solution will be presented in abbreviated form.<\/p>\n\n\n\n

      Reference temperature: 77\u00b0F<\/p>\n\n\n\n

        \n
      1. a.<\/strong>\u00a0Basis: 1 lb mol NH3<\/sub>\u00a0\u2261 17 lb NH3<\/sub>wt\u00a0%\u00a0NH3\u2009\u2009=\u2009lb\u00a0NH3lb\u2009H2O\u00a0+\u00a0lb\u00a0NH3(100)3=17(100)17+mH2O\u2003mH2O=550\u00a0lb or about 30 lb mol H2<\/sub>OFrom the table above, the\u00a0\u0394H^solno=\u221214,800\u00a0Btu\/lb mol NH3<\/sub>, which is equal to 14,800 Btu removed from the system.<\/li>\n\n\n\n
      2. b.<\/strong>\u00a0Basis: 100 gal solutionFrom Lange\u2019s\u00a0Handbook of Chemistry<\/em>, a 32.0% solution of NH3<\/sub>\u00a0has the following properties:Sp.gr.: \u00a0\u00a0NH30.889\u2062\u2009\u2009\u2009\u2009H2O1.003The density of the 32.0% solution in pounds per 100 gal is(0.889)(62.4)(1.003)(100)7.48=744lb\/100gal744(0.32)17=14.0\u00a0lb mol NH3<\/sub>\/100 gal solutionBasis: 1 lb mol NH3<\/sub>32.0=170017+mH2O\u2003mH2O=36\u2009lb\u00a0and\u00a0nH2O=2\u2009lb\u2009molCooling req’dBtu\/100\u2009gal}=(lbmolNH3100gal)(\u2212\u0394HsolnoBtulbmolNH3)Cooling req’dfor 100 gal32.0%NH3\u2062\u2009soln}=(14.0)(\u221213,700)=\u2212191,000Btu\/100\u2009galsoln(heat removed)<\/li>\n<\/ol>\n\n\n\n

        Self-Assessment Test<\/h3>\n\n\n\n

        Questions<\/h4>\n\n\n\n

        1<\/a>.<\/strong> Define and show on a sketch (a) the integral heat of solution, and (b) the differential heat of solution.<\/p>\n\n\n\n

        2<\/a>.<\/strong> Indicate whether the following statements are true or false:<\/p>\n\n\n\n

          \n
        1. a. Heats of reaction and heats of solution represent the same physical phenomena.<\/li>\n\n\n\n
        2. b. All mixtures have significant heats of solution.<\/li>\n\n\n\n
        3. c. The heat of mixing at infinite dilution involves an infinite amount of solvent.<\/li>\n\n\n\n
        4. d. Heats of solution can be positive and negative.<\/li>\n\n\n\n
        5. e. A gas mixture is usually an ideal solution.<\/li>\n<\/ol>\n\n\n\n

          3<\/a>.<\/strong> a. What is the reference state for H2<\/sub>O in the table for the heat of solution of HCl?<\/p>\n\n\n\n

            \n
          1. b. What is the value of the enthalpy of the H2<\/sub>O in the reference state?<\/li>\n<\/ol>\n\n\n\n

            4.<\/strong> Repeat question 3 for HCl.<\/p>\n\n\n\n

            Problems<\/h4>\n\n\n\n

            1.<\/strong>\u00a0Calculate the heat of solution at standard conditions when 1 mol of a solution of 20 mol % HCl is mixed with 1 mol of a solution of 25 mol % HCl.<\/p>\n\n\n\n

            2.<\/strong>\u00a0How much heat has to be added to a solution of 1 g mol of HCl in 10 g mol of H2<\/sub>O to concentrate the solution to 1 g mol of HCl in 4 g mol of H2<\/sub>O?<\/p>\n\n\n\n

            3.<\/strong>\u00a0The heat of formation of H2<\/sub>SO4<\/sub>\u00a0is \u2212811.319 kJ\/g mol H2<\/sub>SO4<\/sub>. What is the heat of formation per gram mole of H2<\/sub>SO4<\/sub>\u00a0of a solution of 20% sulfuric acid?<\/p>\n\n\n\n

            Thought Problems<\/h4>\n\n\n\n

            1.<\/strong> A tanker truck of hydrochloric acid was inadvertently unloaded into a large storage tank used for sulfuric acid. After about one-half of the 3000 gal load had been discharged, a violent explosion occurred, breaking the inlet and outlet lines and buckling the tank. What might be the cause of the explosion?<\/p>\n\n\n\n

            2.<\/strong>\u00a0A concentrated solution (73%) of sodium hydroxide was stored in a vessel. Under normal operations, the solution was forced out by air pressure as needed. When application of air pressure did not work, apparently due to solidification of the caustic solution, water was poured through a manhole to dilute the caustic and free up the pressure line. An explosion took place and splashed caustic out of the manhole 15 ft into the air. What caused the incident?<\/p>\n\n\n\n

            Discussion Problem<\/h4>\n\n\n\n

            A significant amount of energy is liberated when freshwater and saltwater are mixed. It has been calculated that the dilution of a cubic meter of freshwater per second in a large volume of seawater dissipates roughly 2.3 MW of power. If this energy could be put to use rather than heating the ocean, it is estimated that the potential of the flow of the Columbia River would yield 15,000 MW. The technology to collect such potential has been proposed, namely, to use a selective membrane that lets certain molecules through but holds others back. Instead of separating water from saltwater by imposing an electric potential on the membrane as in desalinization, the idea is to reverse the process and mix freshwater with saltwater to generate an electric current. The membranes are arranged so that positive ions flow in one direction and negative ions in the other direction. What do you think of the proposal?<\/p>\n","protected":false},"excerpt":{"rendered":"

            Up to this chapter we have assumed that when a stream consists of several components, the total properties of the stream are the appropriately weighted sum of the properties of the individual components. For such ideal solutions, we could write down for the heat capacity of an ideal mixture, for example,Cpmixture=xACpA+xBCpB+xCCpC+… or, for the enthalpy,\u0394H^mixture =xA\u0394H^A+xB\u0394H^B+xC\u0394H^C+\u22ef In particular, […]<\/p>\n","protected":false},"author":1,"featured_media":4607,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[569],"tags":[],"class_list":["post-4735","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-heats-of-solution-and-mixing"],"jetpack_featured_media_url":"https:\/\/workhouse.sweetdishy.com\/wp-content\/uploads\/2024\/09\/heat.png","_links":{"self":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/4735","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/comments?post=4735"}],"version-history":[{"count":1,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/4735\/revisions"}],"predecessor-version":[{"id":4736,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/4735\/revisions\/4736"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/media\/4607"}],"wp:attachment":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/media?parent=4735"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/categories?post=4735"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/tags?post=4735"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}