Of the substances (as pure substances, in aqueous solutions, or of mixtures) tested on video, categorize them into either molecular or ionic substances. molecular ionic No Answers Chosen No Answers Chosen Possible answers | HCI (in toluene) | 0.1 M C12H22O11 (aq) - this is sucrose | CH3COOH (glacial acetic acid) | saturated Ca(OH)2 (aq) | 0.1 M NH4CI (aq) | KCIO3 (s) | C7H8 (toluene) 0.1 МСНЗСH2ОH (аq) СНЗСН20Н (pure) | KCIO3 (I) | 0.1 M NaCl (aq) 0.1 МКСIО3 (аq) | saturated Ca3(PO4)2 (aq) | 0.1 M NH3 (aq) | 0.1 M HCI (aq) | H2O (distilled) 0.1МСНЗСООН (аq) | 0.1 M NAOH (aq)

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section20.7: Green Chemistry And Sustainability

Problem 2.1ACP: Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the...

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A hydrochloric acid solution is standardized by titrating 0.5008 g of primary standard tris(hydroxymethyl) aminomethane, C4H11NO3, with 99.9780% purity. If 39.68 mL isrequired for the titration, what is the molarity of the acid?
The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. 1. what is the pH when the volume of base added equals half the volume of the equivalence point? 2. what is the pH of the titration when 20.00 mL of base have been added? 3. what is the pH of the titration when 30.00 mL of base have been added?
Benzoic acid, C6H5COOH, is much more soluble in NaOH(aq) than it is in pure water. Can you suggest a reason for this? of HO,
The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. A. What is the pH at the beginning of the titration, Vbase = 0.00 mL? B. What is the pH at the equivalence point? C. What is the pH of the titration when 5.00 mL of base have been added? D. What is the pH when the volume of base added equals half the volume of the equivalence point? E. What is the pH of the titration when 20.00 mL of base have been added? F. What is the pH of the titration when 30.00 mL of base have been added?
The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. a) Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of base horizontally. Label your axes with correct pH and volumes. (Attach more space, if needed) b) what is the pH at the beginning of the titration, Vbase = 0.00 mL ? c) what is the volume of the base needed to reach the equivalence point ? (label the equiv. point) d) what is the pH at the equivalence point?e) what is the pH of the titration when 5.00 mL of base have been added ? f) what is the pH when the volume of base added equals half the volume of the equivalence point? g) what is the pH of the titration when 20.00 mL of base have been added? h) what is the pH of the titration…
Titrations are acid-base reactions in which the amount of acid and base in solution are known quite precisely. The specific case where the acid and base have been added in equivalent molar amounts, is called the equivalence point. At this point, mol acid = mol base %3D At all other points in a titration, either the base is the limiting reactant (and there is excess acid) or the acid is the limiting reactant (and there is excess base). So, except at the equivalence point, titration problems are limiting reactant problems, which means we can do them- a lot of them! One additional point: when there is left over strong acid (acid in excess), 100% of that excess acid is ionized to become H* ions: [strong acid] = [H*] and pH = -log[H"] Something similar happens for strong bases. 1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200 M HCI. Show all your work for each calculation (including the volumes for which the pH is given).…
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A saturated aqueous solution of silver perchlorate (AgClO4) contains 84.8% by mass AgClO4, but a saturated solution of AgClO4 in 60% aqueous perchloric acid contains only 5.63% by mass AgClO4. Explain this large difference using chemical equations.
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