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2. pH - Wikipedia

   en.wikipedia.org/wiki/PH

   When calculating the pH of a solution containing acids and/or bases, a chemical speciation calculation is used to determine the concentration of all chemical species present in the solution. The complexity of the procedure depends on the nature of the solution.

3. Henderson–Hasselbalch equation - Wikipedia

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

   The Henderson–Hasselbalch equation relates the pH of a solution containing a mixture of the two components to the acid dissociation constant, Ka of the acid, and the concentrations of the species in solution. [2] Simulated titration of an acidified solution of a weak acid (pKa = 4.7) with alkali. To derive the equation a number of simplifying ...

4. Buffer solution - Wikipedia

   en.wikipedia.org/wiki/Buffer_solution

   In the case of citric acid, the overlap is extensive and solutions of citric acid are buffered over the whole range of pH 2.5 to 7.5. Calculation of the pH with a polyprotic acid requires a speciation calculation to be performed. In the case of citric acid, this entails the solution of the two equations of mass balance:

5. Ion speciation - Wikipedia

   en.wikipedia.org/wiki/Ion_speciation

   Speciation of ions refers to the changing concentration of varying forms of an ion as the pH of the solution changes. [1] The ratio of acid, AH and conjugate base, A −, concentrations varies as the difference between the pH and the p Ka varies, in accordance with the Henderson-Hasselbalch equation. The pH of a solution of a monoprotic weak ...

6. Weak base - Wikipedia

   en.wikipedia.org/wiki/Weak_base

   Weak. v. t. e. A weak base is a base that, upon dissolution in water, does not dissociate completely, so that the resulting aqueous solution contains only a small proportion of hydroxide ions and the concerned basic radical, and a large proportion of undissociated molecules of the base.

7. Charlot equation - Wikipedia

   en.wikipedia.org/wiki/Charlot_equation

   Equation used to calculate the pH of a weak acid or base solution. The Charlot equation, named after Gaston Charlot, is used in analytical chemistry to relate the hydrogen ion concentration, and therefore the pH, with the formal analytical concentration of an acid and its conjugate base. It can be used for computing the pH of buffer solutions ...

8. Acid–base titration - Wikipedia

   en.wikipedia.org/wiki/Acid–base_titration

   An acid–base titration is a method of quantitative analysis for determining the concentration of Brønsted-Lowry acid or base (titrate) by neutralizing it using a solution of known concentration (titrant). [1] A pH indicator is used to monitor the progress of the acid–base reaction and a titration curve can be constructed.

9. Ammonia solution - Wikipedia

   en.wikipedia.org/wiki/Ammonia_solution

   Ammonia solution, also known as ammonia water, ammonium hydroxide, ammoniacal liquor, ammonia liquor, aqua ammonia, aqueous ammonia, or (inaccurately) ammonia, is a solution of ammonia in water. It can be denoted by the symbols NH 3 (aq). Although the name ammonium hydroxide suggests a salt with the composition [NH+. 4] [OH−.