Nacl Strong Or Weak Electrolyte

At the finish of my get-go postal service on SECTION 4 - Types of Chemical Reactions and Solution Stoichiometry, we introduced Potent Electrolytes, Weak Electrolytes, and Nonelectrolytes.

Let's elaborate on each of these 3 types of substances...

i. Strong Electrolytes.

Strong Electrolytes = substances (solutes) that are completely ionized (hydrated) when dissolved in h2o.

ex: very soluble salts (i.e. NaCl)
ex: strong acids ( i.eastward. HCl, HNO₃, HClO₄, H₂SO₄)
ex: strong bases ( i.e. NaOH, KOH)

➞ when the in a higher place compounds are dissolved in water, they are 100% ionized. In other words, they ionize (dissociate into cation and anion) completely:

Strong Electrolytes Conduct Electricity

So, the easier it is for a substance (solute) to form ions in solution, the better it is at conducting electricity because ions act equally charge carriers in aqueous solutions.

=====

2. Weak Electrolytes.

Weak Electrolytes = substances that ionize (dissolve) but slightly in water.

➞ two most common are: NH_three (ammonia) and HC₂H₃O_two (acetic acid).

➞ they produce relatively few ions (charge carriers) when dissolved...

Weak Electrolytes Dissociate to a Slight Extent

See the reaction arrow above? It shows us that mainly only HC_twoH_threeO₂ is nowadays and it'southward non an ion.

Considering acetic acid (HC₂H₃O₂) is a weak electrolyte, it's called a weak acid.

weak acrid = any acid that dissociates (ionizes) but to a slight extent in aqueous solution.

-----

ex: The most common weak base is ammonia (NH_three). It's a weak electrolyte:

Ammonia is a Weak Electrolyte

The solution is basic considering OH^- ions are produced. Simply because very few OH^- ions are formed, NH₃ is a weak electrolyte, and thus a weak base of operations.

=====

3. Nonelectrolytes.

Nonelectrolytes = substances that exercise deliquesce in water to make an aqueous solution, but do not produce any ions.

ex: C₂H₅OH (ethanol)
ex: C₁₂H₂₂O₁₁ (sucrose) -- table saccharide. Here'due south what happens:

Sucrose is a Nonelectrolyte

=====

Molarity and Concentration in Chemical science.

The extent to which a solute dissolves in a solution is expressed past the solution's concentration.

➞ Concentration is almost often expressed every bit molarity (K).

➞ Molarity (G) = number of moles of solute (mol) / liters of solution (Fifty).

So, 1M = i mol/50 .

Here it is once again, but easier to follow:

The Molarity Formula

Molarity Calculations.

ex: Calculate the molarity of a solution made by dissolving 11.5g of solid NaOH in enough h2o to make one.50L of solution.

- well, we know that molarity = moles of NaOH / liters of solution.

- we already have the "liters of solution" = 1.50L

- so the first thing nosotros need to do, is summate the "moles of NaOH"...

Molarity Calculation Example

=====

In my next video web log post from this series: Section 4 - Types of Chemical Reactions and Solution Stoichiometry, we'll cover more than Molarity Calculations.