Think Pink

https://drive.google.com/open?id=0B6biT3nsiazTdy1xQzNaWGFVS0E



This is an image of the titrated solution when too much base is added. There is a fine line from the time you add the perfect amount of solution to one drop extra that makes a bright pink color. In order to get the perfect amount it takes trial and error.

Acid

Must See Video of Titration Lab
Above is a link of our titration lab. You can see the acid solution change colors as the base is added.it took careful concentration to avoid getting the solution too pink so the slower the better.

Titration

The word titration rhymes with tight nation. The medical use of this word is a little different, but in chemistry titration refers to a commonly used method of finding the concentration of an unknown liquid, by comparing it with a known liquid. An acid-base titration is good to consider when learning the method, but there are more uses for the technique. The measure of oxalate ion using potassium permanganate in a warm acid environment is a good example of a redox titration. The Mohr titration is a determination of chloride concentration using known silver nitrate solution and sodium dichromate an indicator.

Acid or Base Buffers

A buffer is a solution that resists changes in pH. A buffer is made with a weak acid and a soluble salt containing the conjugate base of the weak acid or a weak base and a soluble salt containing the conjugate acid of the weak base. Some examples of buffer material pairs are:

acetic acid and sodium acetate, H(C₂H₃O₂) and Na(C₂H₃O₂)
hydrofluoric acid and potassium fluoride, HF and KF
carbonic acid and sodium bicarbonate, H₂CO₃ and NaHCO₃
ammonium hydroxide and ammonium nitrate, NH₄OH and NH₄NO₃
nitrous acid and lithium nitrite, HNO₂ and LiNO₂

Weak Acid and Bases

Weak acids and bases do not ionize very much, so the [H⁺] or [(OH)^-] must be calculated by the equilibrium expression.

This would be easy to know exactly, except that the [HA] is not always equal to the concentration of solute that actually went into the solution. The more accurate way to express the equilibrium expression would be to include in the denominator the idea that the [HA] is really the concentration of solute originally put into solution minus the amount of that solute that ionized. We could represent the amount that ionized by either the [A^-] or the [H⁺], so the denominator should be either [HA] - [A^-] or [HA] - [H⁺]. Let's use the second option for alternative denominator because we want to solve for the hydrogen ion concentration. By the 5% rule, [HA] = [HA] - [H⁺] only if the hydrogen ion concentration is less than five percent of the total solute concentration. This is the case for most weak acids. The only exceptions are when the strongest of the weak acids are in the most dilute solutions.

Acid/Bases

 An acid is a material that can release a proton or hydrogen ion. Hydrogen chloride in water solution ionizes and becomes hydrogen ions and chloride ions. a base, or alkali, is a material that can donate a hydroxide ion. Sodium hydroxide in water solution becomes sodium ions and hydroxide ions. Every ion dissociation that involves a hydrogen or hydroxide ion could be considered an acid- base reaction. Acids are electron pair acceptors and bases are electron pair donors.  Each ionizable pair has a proton donor and a proton acceptor. Acids are paired with bases. One can accept a proton and the other can donate a proton. Each acid has a proton available and another part, called the conjugate base. When the acid ionizes, the hydrogen ion is the acid and the rest of the original acid is the conjugate base.