Merge pull request #10 from virtual-labs/testing

Testing

experiment/simulation/index.html

@@ -228,7 +228,7 @@ <h1 id="1-1" style="position:absolute; left:90px; top:250px; color:grey; display
 <input id="check1" type="button" name="Formula" value="Check" />&nbsp;&nbsp;&nbsp;<input id="result1" type="button" name="Formula" value="Result"  style="visibility:hidden;"/></br>
 </br></br>
 
-<img id="eqn1"  style="position:absolute; left:0px; top:340px; border:2px solid black; padding:5px; visibility:hidden;" src="images/eqn1.png" />
+<img id="eqn1"  style="position:absolute; left:0px; top:325px; border:2px solid black; padding:5px; visibility:hidden;" src="images/eqn1.png" />
 
 <p id="r1" style="position:absolute; left:280px; top:268px; color:#32CD32;  visibility:hidden; font-size:22px;" >&#10004;</p><p id="w1" style="position:absolute; left:517px; top:266px; color:red;  visibility:hidden; font-size:22px;" >&#10008;</p>
 
@@ -386,7 +386,7 @@ <h1 id="7-1" style="position:absolute; left:250px; top:250px; color:grey; displa
 <input id="check12-2" type="button" name="check" value="Check" />&nbsp;&nbsp;&nbsp;<input id="result12-2" type="button" name="Formula" value="Result"  style="visibility:hidden;" /></br>
 </br></br>
 
-<img id="eqn12-3"  style="position:absolute; left:10px; top:340px; border:2px solid black; padding:5px; visibility:hidden; " src="images/eqn3.png" />
+<img id="eqn12-3"  style="position:absolute; left:10px; top:310px; border:2px solid black; padding:5px; visibility:hidden; " src="images/eqn3.png" />
 <p id="r12-2" style="position:absolute; left:257px; top:237px; color:#32CD32;  visibility:hidden; font-size:22px;" >&#10004;</p><p id="w12-2" style="position:absolute; left:485px; top:240px; color:red;  visibility:hidden; font-size:22px;" >&#10008;</p>
 <p id="display12-3" style="position:absolute; left:0px; top:330px; font-size:14px; visibility:hidden;" >P as alkalinity of CaCO<sub>3</sub> =</p>
 </div>
@@ -483,7 +483,7 @@ <h1 id="7-1" style="position:absolute; left:250px; top:250px; color:grey; displa
 <input id="check2" type="button" name="check" value="Check" />&nbsp;&nbsp;&nbsp;<input id="result2" type="button" name="Formula" value="Result"  style="visibility:hidden;" /></br>
 </br></br>
 
-<img id="eqn3"  style="position:absolute; left:10px; top:340px; border:2px solid black; padding:5px; visibility:hidden; " src="images/eqn3.png" />
+<img id="eqn3"  style="position:absolute; left:10px; top:310px; border:2px solid black; padding:5px; visibility:hidden; " src="images/eqn3.png" />
 
 <p id="r2" style="position:absolute; left:257px; top:245px; color:#32CD32;  visibility:hidden; font-size:22px;" >&#10004;</p><p id="w2" style="position:absolute; left:485px; top:245px; color:red;  visibility:hidden; font-size:22px;" >&#10008;</p>
 

experiment/theory.md

@@ -8,5 +8,27 @@
 
 <p style="text-indent:50px; text-align:justify;">Alkalinity of water is the capacity of water to neutralize acid. It is usually expressed as Total Alkalinity or Caustic Alkalinity in water. It is significant in many uses and treatments of natural waters and wastewaters. Alkalinity is measured titrimetrically by titrating against Dilute Sulphuric Acid. Phenolphthalein and Methyl Orange are used as indicator to indicate pH 8.3 and pH 4.3. Phenolphthalein process a pink colour when pH is above 8.3 and colourless when pH is below 8.3.</p>
 
+<p style="text-indent:50px; text-align:justify;">Natural water alkalinity is caused primarily by the presence of weak acid salts, though strong bases (i.e. OH- ) may also contribute in extreme environments. Bicarbonates are the most common type of alkalinity found in natural waters, and they are formed by the partitioning of CO2 from the atmosphere and the weathering of carbonate minerals in rocks and soil. Other salts of weak acids, such as borate, silicates, ammonia, phosphates, and organic bases from natural organic matter, may be present in small amounts. Alkalinity is frequently identified as mg/L CaCO3 because the majority of alkalinity is derived from the weathering of carbonate minerals.</p>
+
+<p style="text-indent:50px; text-align:justify;">Titration with standardized acid determines the total amount of hydroxyl ions in a solution. This is a well-known water-analysis procedure for estimating the concentrations of hydroxyl, carbonate ion, and bicarbonate ions. This titration has two pH endpoints, P and M, which correspond to the phenolphthalein and methyl orange indicators.</p>
+
+<p style="text-indent:50px; text-align:justify;">As previously stated, alkalinity in natural waters is primarily caused by carbonate species, and the following chemical equilibria are established in waters.
+</p>
+
+<p align="center">CO<sub>2</sub> + H<sub>2</sub>O <=> H<sub>2</sub>CO<sub>3</sub><sup>*</sup></p>
+<p align="center">H<sub>2</sub>CO<sub>3</sub> <=> HCO<sub>3</sub><sup>-</sup> + H<sup>+</sup></p>
+<p align="center">HCO<sub>3</sub><sup>-</sup> <=> CO<sub>3</sub><sup>2-</sup> + H<sup>+</sup></p>
+
+<p style="text-indent:50px; text-align:justify;">where H<sub>2</sub>CO<sub>3</sub><sup>*</sup> represents the total concentration of dissolved CO<sub>2</sub> and H<sub>2</sub>CO<sub>3</sub>. The first chemical equation represents the equilibrium of CO<sub>2</sub> in the atmosphere with dissolved CO<sub>2</sub> in the water. The equilibrium constant, Henry’s Law, for this reaction is </p>
+
+<center><a href="https://www.codecogs.com/eqnedit.php?latex=\fn_jvn&space;K_{CO_{2}}&space;=&space;\frac{\left&space;[&space;H_{2}CO_{3}\right&space;]}{P_{CO_{2}}}&space;=&space;10^{-1.47}" target="_blank"><img src="https://latex.codecogs.com/gif.latex?\fn_jvn&space;K_{CO_{2}}&space;=&space;\frac{\left&space;[&space;H_{2}CO_{3}\right&space;]}{P_{CO_{2}}}&space;=&space;10^{-1.47}" title="K_{CO_{2}} = \frac{\left [ H_{2}CO_{3}\right ]}{P_{CO_{2}}} = 10^{-1.47}" /></a></center><br>
+
+<p style="text-indent:50px; text-align:justify;">The equilibrium relationships for the last two reactions may be expressed as</p>
+
+<center><a href="https://www.codecogs.com/eqnedit.php?latex=\fn_jvn&space;K_{1}&space;=&space;\frac{\left&space;[&space;H^{&plus;}&space;\right&space;]\left&space;[HCO_{3}\;^{-}\right]}{H_{2}CO_{3}}&space;=&space;10^{-6.35}" target="_blank"><img src="https://latex.codecogs.com/gif.latex?\fn_jvn&space;K_{1}&space;=&space;\frac{\left&space;[&space;H^{&plus;}&space;\right&space;]\left&space;[HCO_{3}\;^{-}\right]}{H_{2}CO_{3}}&space;=&space;10^{-6.35}" title="K_{1} = \frac{\left [ H^{+} \right ]\left [HCO_{3}\;^{-}\right]}{H_{2}CO_{3}} = 10^{-6.35}" /></a></center></br>
+
+<center>
+<a href="https://www.codecogs.com/eqnedit.php?latex=\fn_jvn&space;K_{2}&space;=&space;\frac{\left&space;[&space;H^{&plus;}&space;\right&space;]\left&space;[CO_{3}\;^{2-}\right]}{\left&space;[&space;HCO_{3}\;^{-}&space;\right&space;]}&space;=&space;10^{-10.33}" target="_blank"><img src="https://latex.codecogs.com/gif.latex?\fn_jvn&space;K_{2}&space;=&space;\frac{\left&space;[&space;H^{&plus;}&space;\right&space;]\left&space;[CO_{3}\;^{2-}\right]}{\left&space;[&space;HCO_{3}\;^{-}&space;\right&space;]}&space;=&space;10^{-10.33}" title="K_{2} = \frac{\left [ H^{+} \right ]\left [CO_{3}\;^{2-}\right]}{\left [ HCO_{3}\;^{-} \right ]} = 10^{-10.33}" /></a></center>
+
 #### Relevant Indian Standard for Alkalinity Test :
 1. IS 3025-23 (Part 23) - 1986: Methods of Sampling and Test (physical and chemical) for Water and Wastewater, Alkalinity, First Revision.