Oxoacids can be formed that involve several central atomsof the same chemical element. An example is H;P3O9,which can be written P;O6(OH)3. (Sodium salts of thesepolyphosphoric acids are used as “builders" in detergentsto improve their cleaning power.) In such a case, we wouldexpect acid strength to correlate approximately with theratio of the number of lone oxygen atoms to the numberof central atoms (this ratio is 6:3 for H;P3O9, for exam-ple). Rank the following in order of increasing acidstrength: H,PO, H,P,О9, Н,Р,06, H.P,0-, H;Р,О 10-Assume that no hydrogen atoms are directly bonded tophosphorus in these compounds.

The acidity of each oxoacid can be measured by calculating the ratio of the number of double bonded…

Answered: Oxoacids can be formed that involve…

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 84AP

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Leucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion form of leucine.
The elements sodium, aluminum, and chlorine are in the same period.. (a) Which has the greatest electronegativity?. (b) Which of the atoms is smallest?. (c) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine. (d) Will the oxide of each element be acidic, basic, or amphoteric?
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
(a) Draw the Lewis structures for at least four species thathave the general formula where X and Y may be the same or different, and n mayhave a value from +1 to -2. (b) Which of the compoundsis likely to be the strongest Brønsted base?
Indicate whether each of the following statements is true orfalse. For each statement that is false, correct the statementto make it true. (a) In general, the acidity of binary acids increasesfrom left to right in a given row of the periodic table.(b) In a series of acids that have the same central atom,acid strength increases with the number of hydrogen atomsbonded to the central atom. (c) Hydrotelluric acid (H2Te) isa stronger acid than H2S because Te is more electronegativethan S.
What is the basis for referring to the hydrogen ion as a proton? (a) The Arrhenius definition of an acid. (b) The Brønsted-Lowry definition of an acid x (c) The Lewis definition of an acid. (d) H* exists as a bare proton. (e) None of these.
Arrange the oxides B2O3, Al2O3, BaO, CO2, Cl2O7, SO3 in order from the most acidic through amphoteric to the most basic (use arrows to indicate the order).
The reaction of ammonia with copper(II) ions is an example of a Lewis Acid–Lewis Base reaction. Which species is the acid and which is the base? How do you know?
The hypochlorite ion, ClO-, acts as a weak base. (a) Is ClO-stronger or weaker base than hydroxylamine? (b) WhenClO- acts as a base, which atom, Cl or O, acts as the protonacceptor? (c) Can you use formal charges to rationalize youranswer to part (b)?
Which of the following species can be Brønsted–Lowry acids: (a) HI; (b) SO 4 2 −; (c) H 2PO 4 −; (d) Cl −?
2. Barbituric acid, HC,H,N,O, a weak organic acid used to manufacture hypnotic drugs and some plastic, has a Ka of 9.8 x 10 An industrial process requires a 0.25 mol/L solution of Barbituric acid. (a) Calculate the H° and pH of the solution. (b) What is the percent ionization of the acid?

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