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…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 106 mo mo-when about a tenth of a mole of the acid is L dissolved in a liter of water. The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10-6 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid strong or weak? species present at 10-6 mol/L or greater when dissolved in water ICIO weak H₂SO, weak IICI strong HCIO, strong ☐ x DO....
A solution is made by dissolving 44.1 g of Ba(NO₂)₂ in 500.0 mL of water. (a) Does Ba²⁺ have any acidic or basic properties? (b) Does NO₂⁻ have any acidic or basic properties? (c) As NO₂⁻ is a base, write the basic equilibrium equation that exists in solution (d) What is the value of Kb for NO₂⁻? The Ka of HNO₂ is 4.5 × 10⁻⁴. (e) Determine the pH of the solution
Over the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, This makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ion. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ion?
Aluminum has been implicated as a neurotoxic agent for Alzheimer’s patients and is known as harmful for renal failure patients. In 1985, the medical community recommended that no more than 10 mg/L Al3+ be present in drinking water used for dialysis patients. At what pH is the maximum Al3+ concentration equal to 10 mg/L, assuming that the only source of Al3+ is Al(OH)3? How does this compare with the allowable pH of drinking water of 7.8; would we expect to observe this concentration in drinking water?
Rank the following acids in order of increasing strength: ClCH2SH, CH3SH, H2S.
Consider the following data on some weak acIas and weak bases: acid base K, Kb name formula name formula 8. acetic acid HCH;CO2|1.8 × 10 hydroxylamine HONH, |1.1 × 10° HNO2 ethylamine C,H,NH2 6.4 x 10 nitrous acid 4.5 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М КCН3СО2 choose one 0.1 M C2H5NH3BR choose one 0.1 M NaNO3 choose one 0.1 M NaNO2 choose one
At pH = 3.9, a weak acid has a concentration of 0.75 M. If the pKa = 4.5, what is the concentration of the conjugate base?
Over the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ions. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ions?
Why did you times the trmp by Avogadro's?
Which of the following species can be Brønsted–Lowry acids: (a) HF; (b) HSO 3 −; (c) Cl 2?
What concentration of acetic acid would produce an aqueous solution with a pH = 3.275? (Ka for HC2H3O2 = 1.76 x 105)
Which of the following species can be Brønsted–Lowry bases: (a) LiOH; (b) Cl −; (c) CH 4?

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