Researchers working with glasses often think of acid-basereactions in terms of oxide donors and oxide acceptors.The oxide ion is O2-.(a) In this system, is the base the oxide donor or the oxideассeptor?(b) Identify the acid and base in each of these reactions:2 CaO + SiO2Ca,SiO4Сa, SiO, + SiOz —2 СaSiO,|Сa, SiO, + Ca0 — СазSiO;

According to Bronsted acid-base theory, Lewis acid is an electrophile, which gains a pair of…

Answered: Researchers working with glasses often…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 7P

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When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
Iodometry is a standard method for redox titration. In many indirect methods one lets the analyte (the substance whose concentration is to be determined) react with iodide ions as then forms triiodide ions, I3- . The amount of triiodide ions is then determined by titration with thiosulphate ions, S2O32- which then form tetrathionate ions, S4O62- whereby the triiodide ions change into iodide ions. Determine the mass of triiodide ions in a solution from the following data. The sample containing triiodide ions was titrated with a 0.01002 M sodium thiosulfate solution of which 18.38 mL were required.
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
Express the concentration in % w/v that is equivalent to 0.5 M NaOHsolution.
Calculate the ph of a solution prepared by dissolving 1.00g of sodium acetate,CH^3COONa, in 50.0ml of 0.15 M acetate acid, CH^3COOH(aq)
A buffer solution of volume 100 cm3 consists of 0.10 M CH3COOH(aq) and 0.10 MNaCH3CO2(aq). (a) What is its pH? (b) What is the pH after the addition of 3.3 mmol NaOH to the buffer solution? (c) What is the pH after the addition of 6.0 mmol HNO3 to the initial buffer solution?
The pH of an aqueous solution of 0.176 M tellurous acid, H2TeO3 (aq), is
A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=4.9×10−7M? B. What is the hydroxide ion concentration, [OH−][OH−], in an aqueous solution with a hydrogen ion concentration of [H+]=4.9×10−7M? C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq)↽−−⇀H+(aq)+A−(aq) The equilibrium concentrations of the reactants and products are [HA]=0.270 M, [H+]=2.00×10−4 M, and [A−]=2.00 ×10−4 M. Calculate the ?a value for the acid HA.
If the equilibrium constant for A + B C is 0.180, what is the equilibrium constant for 2C 2A + 2B ?
The pH of an aqueous solution of 0.1690 M hydrosulfuric acid, H₂S (aq), is
Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?
Assuming the base completely dissociates in water, what is the pH of a 5.70 g/L solution of Ba(OH) 2 (aq) ?

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