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1) The Henderson-Hasselbalch Equation relates pH and pKa to [A-] and [HA].
2) Ka is known as the acid formation constant.
3)When titrating, the analyte is the standardized (known concentration) solution, and the titrant is the solution being analyzed.
4)Volumetric titrations can only ever be performed using a monoprotic weak acid and a strong base.
5) For monoprotic weak acids, the titration curve (pH on y-axis, volume of base added on x-axis) takes on an S-shape.
6)Volumetric titrations involve a
7)In titrations, an indicator (dye) solution is often used to signal the endpoint with a color change.
8) NaOH is the chemical formula for sodium hydroxide.
9) For the chemical reaction between an acid (H+) and base (OH-), there is a 1:1 molar ratio between H+ and OH-.
10) In the reaction of a weak acid HA with base NaOH, the product NaA is the conjugate acid salt.
11) In the reaction of a weak acid HA with base NaOH, sodium ion Na+ is a spectator ion.
12) Water is a product formed in the reaction of a weak acid HA with base NaOH.
13) As more titrant is added to the analyte solution and the solution becomes more basic, the pH increases.
14 The half-equivalence point of the titration occurs on the titration curve at the exact center/inflection point of the S-shape.
15) The equivalence point has been reached when the moles of weak acid present in the analyte solution is equal to the moles of base that have been added to the solution.
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