Umm. Seriously, i am grateful during the tutoral, i have learn more things and have increased my knowledge. In the tutoral, i have get understand some basic keys which had enable me  to be couragous. It also inspired me when i do not conprehend ,despite the facts that i know some and losed some. During this, i understand more on  ionization, precipitation, etc. All my wish is to inspire others to learn more for futre boost.

<h2>Factors that affect the conductivity of electrolytes</h2>
<p>The conductivity of an electrolyte is therefore affected by the following factors:</p>
<ul>
<li>
<p>The <strong>concentration of ions</strong> in solution. The higher the <a data-lesson="equilibrium-calculations" data-subject="chemistry" data-tutorial="basic-equilibrium-concepts" href="https://app.ulearngo.com/chemistry/basic-equilibrium-concepts/equilibrium-calculations">concentration</a> of ions in solution, the higher its conductivity will be.</p>
</li>
<li>
<p>The <strong>type of substance</strong> that dissolves in water. Whether a material is a strong electrolyte (e.g. potassium nitrate, \(\text{KNO}_{3}\)), a weak electrolyte (e.g. acetic acid, \(\text{CH}_{3}\text{COOH}\)) or a non-electrolyte (e.g. sugar, alcohol, oil) will affect the conductivity of <a data-lesson="unique-properties-of-water" data-subject="chemistry" data-tutorial="states-of-matter" href="https://app.ulearngo.com/chemistry/states-of-matter/unique-properties-of-water">water</a> because the concentration of ions in solution will be different in each case. Strong electrolytes form ions easily, weak electrolytes do not form ions easily and non-electrolytes do not form ions in solution.</p>
</li>
<li>
<p><strong>Temperature.</strong> The warmer the solution, the higher the <a data-lesson="summarizing-solubility" data-subject="chemistry" data-tutorial="solutions-and-colloids" href="https://app.ulearngo.com/chemistry/solutions-and-colloids/summarizing-solubility">solubility</a> of the material being dissolved and therefore the higher the conductivity as well.</p>
</li>
</ul>
<div class="ns-school-emp">
<h2>Optional Experiment: Electrical conductivity</h2>
<div class="ns-school-defn">
<section class="activity">
<h3>Aim</h3>
<p>To investigate the electrical conductivities of different substances and solutions.</p>
</section>
<section class="activity">
<h3>Apparatus</h3>
<ul>
<li>
<p>Solid <a data-lesson="acid-base-reactions-continued-2" data-subject="chemistry" data-tutorial="acid-base-redox-reactions" href="https://app.ulearngo.com/chemistry/acid-base-redox-reactions/acid-base-reactions-continued-2">salt</a> (\(\text{NaCl}\)) crystals</p>
</li>
<li>
<p>different liquids such as distilled water, tap water, seawater, sugar, oil and alcohol</p>
</li>
<li>
<p>solutions of salts e.g. \(\text{NaCl}\), \(\text{KBr}\), \(\text{CaCl}_{2}\), \(\text{NH}_{4}\text{Cl}\)</p>
</li>
<li>
<p>a solution of an acid (e.g. \(\text{HCl}\)) and a solution of a base (e.g. \(\text{NaOH}\))</p>
</li>
<li>
<p>torch cells</p>
</li>
<li>
<p>ammeter</p>
</li>
<li>
<p>conducting wire, crocodile clips and 2 <a data-lesson="carbon" data-subject="chemistry" data-tutorial="metals-metalloids-nonmetals" href="https://app.ulearngo.com/chemistry/metals-metalloids-nonmetals/carbon">carbon</a> rods.</p>
</li>
</ul>
</section>
<section class="activity">
<h3>Method</h3>
<ol>
<li>
<p>Set up the experiment by connecting the circuit as shown in the diagram below. In the diagram, X represents the substance or solution that you will be testing.</p>
</li>
<li>
<p>When you are using the solid crystals, the crocodile clips can be attached directly to each end of the crystal. When you are using solutions, two carbon rods are placed into the <a data-lesson="summarizing-properties-of-liquids" data-subject="chemistry" data-tutorial="liquids-and-solids" href="https://app.ulearngo.com/chemistry/liquids-and-solids/summarizing-properties-of-liquids">liquid</a> and the clips are attached to each of the rods.</p>
</li>
<li>
<p>In each case, complete the circuit and allow the current to flow for about 30 seconds.</p>
</li>
<li>
<p>Observe whether the ammeter shows a reading.</p>
</li>
</ol>
<img alt="d37e96278493c3530750c4f4dfae385f.png" src="https://data.ulearngo.com/assets/224ebac0-d8f0-4d45-9211-08095b44a759"/><img alt="6b462d07ee1d02b51260a3329bbad964.png" src="https://data.ulearngo.com/assets/312c340a-8e6c-4e3d-b672-a9072802bb9b"/></section>
<section class="activity">
<h3>Results</h3>
<p>Record your observations in a table similar to the one below:</p>
<div>
<table>
<tbody>
<tr>
<td>
<p>Test substance</p>
</td>
<td>
<p>Ammeter reading</p>
</td>
</tr>
<tr>
<td> </td>
<td> </td>
</tr>
<tr>
<td> </td>
<td> </td>
</tr>
<tr>
<td> </td>
<td> </td>
</tr>
<tr>
<td> </td>
<td> </td>
</tr>
<tr>
<td> </td>
<td> </td>
</tr>
</tbody>
</table>
</div>
<p>What do you notice? Can you explain these observations?</p>
</section>
<section class="activity">
<h3>Conclusions</h3>
<p>Solutions that contain free-moving ions are able to conduct electricity because of the movement of charged particles. Solutions that do not contain free-moving ions do not conduct electricity.</p>
</section>
</div>
</div>
<p>Remember that for electricity to flow, there needs to be a movement of charged <a data-lesson="the-kinetic-theory-of-gases" data-subject="chemistry" data-tutorial="states-of-matter" href="https://app.ulearngo.com/chemistry/states-of-matter/the-kinetic-theory-of-gases">particles</a> e.g. ions. With the solid \(\text{NaCl}\) crystals, there was no flow of electricity recorded on the ammeter. Although the solid is made up of ions, they are held together very tightly within the <a data-lesson="crystal-lattice-structure" data-subject="chemistry" data-tutorial="bonding-atomic-combinations" href="https://app.ulearngo.com/chemistry/bonding-atomic-combinations/crystal-lattice-structure">crystal lattice</a> and therefore no current will flow. Distilled water, oil and alcohol also don't conduct a current because they are <em>covalent compounds</em> and therefore do not contain ions.</p>
<p>The ammeter should have recorded a current when the salt solutions and the acid and base solutions were connected in the circuit. In solution, salts <em>dissociate</em> into their ions, so that these are free to move in the solution. Look at the following examples:</p>
<p>Dissociation of potassium bromide:</p>
<p>\[\text{KBr (s)} \rightarrow \text{K}^{+}\text{(aq)} + \text{Br}^{-}\text{(aq)}\]</p>
<p>Dissociation of table salt:</p>
<p>\[\text{NaCl (s)} \rightarrow \text{Na}^{+}\text{(aq)} + \text{Cl}^{-}\text{(aq)}\]</p>
<p>Ionisation of hydrochloric acid:</p>
<p>\[\text{HCl (l)} + \text{H}_{2}\text{O (l)} \rightarrow \text{H}_{3}\text{O}^{+}\text{(aq)} + \text{Cl}^{-}\text{(aq)}\]</p>
<p>Dissociation of <a data-lesson="redox-reactions" data-subject="chemistry" data-tutorial="reactions-in-aqueous-solution" href="https://app.ulearngo.com/chemistry/reactions-in-aqueous-solution/redox-reactions">sodium</a> hydroxide:</p>
<p>\[\text{NaOH (s)} \rightarrow \text{Na}^{+}\text{(aq)} + \text{OH}^{-}\text{(aq)}\]</p>

1da7dde6-444c-4cfc-9055-98f781c809ca

Factors Affecting Electrolyte Conductivity

Chemistry generally explores the substances of which matter is composed, the investigation of their properties and reactions, and the use of such reactions to form new substances. 

Chemistry

Explore how different substances dissolve and react with each other in water, including ionization and conductivity, precipitation reactions, tests for anions, and various types of reactions such as redox and ion exchange.


Factors Affecting Electrolyte Conductivity

Track Your Learning Progress

Earlier discussion