2. A convenient way of converting hydroxide concentration to pH is -log 10-14 pH+ pOH -log 10-14 = pH + log [OH-] 14 = pH - log [H30] 14 = -log [OH] + log [H3O*] 3. Titration of strong acid with strong base (titrant), beyond the equivalence point, we first calculate and then [ pOH and pH; pH and pOH; mmol of acid left and pH; mmol of base added and pOH ] 4. At the equivalence point of the titration of strong acid and base, the solution is [ pH > pOH; pOH > pH; pH = pOH; pH>7] 5. Colorless in moderately acidic solutions and exhibit a variety of colors in alkaline media but fade slowly in strong alkaline solutions. [ thymol blue; phenolphthalein indicator; azo indicator; alizarin ] 6. Titrating a strong base with a strong acid, the hydroxide ion is numerically related to the analytical concentration of the base at [ initial point; pre-equivalence point; equivalence point; post equivalence point ] 7. If Ka increases the strength of an acid [ increases; decreases; no effect ]

2. A convenient way of converting hydroxide concentration to pH is -log 10-14 pH+ pOH -log 10-14 = pH + log [OH-] 14 = pH - log [H30] 14 = -log [OH] + log [H3O*] 3. Titration of strong acid with strong base (titrant), beyond the equivalence point, we first calculate and then [ pOH and pH; pH and pOH; mmol of acid left and pH; mmol of base added and pOH ] 4. At the equivalence point of the titration of strong acid and base, the solution is [ pH > pOH; pOH > pH; pH = pOH; pH>7] 5. Colorless in moderately acidic solutions and exhibit a variety of colors in alkaline media but fade slowly in strong alkaline solutions. [ thymol blue; phenolphthalein indicator; azo indicator; alizarin ] 6. Titrating a strong base with a strong acid, the hydroxide ion is numerically related to the analytical concentration of the base at [ initial point; pre-equivalence point; equivalence point; post equivalence point ] 7. If Ka increases the strength of an acid [ increases; decreases; no effect ]

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 111QRT: Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong...

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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