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  • pH - Wikipedia
    The pH of a solution is defined as the negative logarithm of the concentration of H +, and the pOH is defined as the negative logarithm of the concentration of OH − For example, the pH of a 0 01 M solution of hydrochloric acid (HCl) is equal to 2 (pH = −log 10 (0 01)), while the pOH of a 0 01 M solution of sodium hydroxide (NaOH) is equal
  • pH indicator - Wikipedia
    The ratio of concentration of conjugate acid base to concentration of the acidic basic indicator determines the pH (or pOH) of the solution and connects the color to the pH (or pOH) value For pH indicators that are weak electrolytes, the Henderson–Hasselbalch equation can be written as: pH = pK a + log 10 ⁠ [Ind −] [HInd] ⁠
  • Bjerrum plot - Wikipedia
    A Bjerrum plot is obtained by using these three equations to plot these three species against pH = −log 10 [H +] eq, for given K 1, K 2 and DIC The fractions in these equations give the three species' relative proportions, and so if DIC is unknown, or the actual concentrations are unimportant, these proportions may be plotted instead
  • Bicarbonate buffer system - Wikipedia
    The pH of tears shift throughout a waking day, rising "about 0 013 pH units hour" until a prolonged closed-eye period causes the pH to fall again [15] Most healthy individuals have tear pH in the range of 7 0 to 7 7, where bicarbonate buffering is the most significant, but proteins and other buffering components are also present that are
  • Acidity function - Wikipedia
    In this case H 0 and H − are equivalent to pH values determined by the buffer equation or Henderson-Hasselbalch equation However, an H 0 value of −21 (a 25% solution of SbF 5 in HSO 3 F) [5] does not imply a hydrogen ion concentration of 10 21 mol dm 3: such a "solution" would have a density more than a hundred times greater than a neutron
  • Charlot equation - Wikipedia
    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 when the approximations of the Henderson–Hasselbalch equation
  • Isoionic point - Wikipedia
    The equation can be further simplified to calculate the pH by taking the negative logarithm of both sides to yield p H = p K 1 + p K 2 2 {\displaystyle pH={{pK_{1}+pK_{2}} \over {2}}} which shows that under certain conditions, the isoionic and isoelectric point are similar


















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