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2. Benzoic acid - Wikipedia

   en.wikipedia.org/wiki/Benzoic_acid

   Benzoic acid is cheap and readily available, so the laboratory synthesis of benzoic acid is mainly practiced for its pedagogical value. It is a common undergraduate preparation. Benzoic acid can be purified by recrystallization from water because of its high solubility in hot water and poor solubility in cold water.

3. Primary standard - Wikipedia

   en.wikipedia.org/wiki/Primary_standard

   Zinc powder, after being dissolved in sulfuric or hydrochloric acid, for standardization of EDTA solutions Such standards are often used to make standard solutions . These primary standards are used in titration and are essential for determining unknown concentrations [ 1 ] or preparing working standards.

4. Benzalkonium chloride - Wikipedia

   en.wikipedia.org/wiki/Benzalkonium_chloride

   Aqueous solutions should be neutral to slightly alkaline. Solutions foam when shaken. Concentrated solutions have a bitter taste and a faint almond-like odour. [citation needed] Standard concentrates are manufactured as 50% and 80% w/w solutions, and sold under trade names such as BC50, BC80, BAC50, BAC80, etc.

5. Neutralization (chemistry) - Wikipedia

   en.wikipedia.org/wiki/Neutralization_(chemistry)

   With a dilute solution of the weak acid, the term 1 + ⁠ T A / K a ⁠ is equal to ⁠ T A / K a ⁠ to a good approximation. If pK w = 14, pH = 7 + (pK a + log T A)/2. This equation explains the following facts: The pH at the end-point depends mainly on the strength of the acid, pK a. The pH at the end-point is greater than 7 and increases ...

6. Henderson–Hasselbalch equation - Wikipedia

   en.wikipedia.org/wiki/Henderson–Hasselbalch...

   A simple buffer solution consists of a solution of an acid and a salt of the conjugate base of the acid. For example, the acid may be acetic acid and the salt may be sodium acetate . The Henderson–Hasselbalch equation relates the pH of a solution containing a mixture of the two components to the acid dissociation constant , K a of the acid ...

7. pH indicator - Wikipedia

   en.wikipedia.org/wiki/PH_indicator

   For example, if the concentration of the conjugate base is 10 times greater than the concentration of the acid, their ratio is 10:1, and consequently the pH is pK a + 1 or pK b + 1. Conversely, if a 10-fold excess of the acid occurs with respect to the base, the ratio is 1:10 and the pH is p K a − 1 or p K b − 1.