c6 6. Arrange the following 0.01 M substances in order of increasing pH.HNO3: pKa = -1.38HNO2: pkg = 3.14%3DHCIO: pk, = 3.18%3!NH3: pK, = 4.74CH3NH3: pKb = 3.36%3DNH3 < CH3NH3 < HNO3 < HNO2 < HCIONH3 < CH3NH3 < HCIO < HNO2 < HNO3HNO3 < HNO2 < HCIO < CH3NH3 < NH3HNO3 < HNO2 < HCIO < NH3 < CH3NH3

Answered: Image /qna-images/answer/96f1f1bc-c090-452c-a921-0c0cfe92bc6f.jpg

6. Arrange the following 0.01 M substances in order of increasing pH. HNO3: pk, = -1.38 HNO2: pka = 3.14 %3D HCIO: pk, = 3.18 %3! NH3: pK, = 4.74 %3D CH3NH3: pKp = 3.36 %3D NH3 < CH3NH3 < HNO3 < HNO2 < HCIO NH3 < CH3NH3 < HCIO < HNO2 < HNO3 HNO3 < HNO2 < HCIO < CH3NH3 < NH3 HNO3 < HNO2 < HCIO < NH3 < CH3NH3

6. Arrange the following 0.01 M substances in order of increasing pH. HNO3: pk, = -1.38 HNO2: pka = 3.14 %3D HCIO: pk, = 3.18 %3! NH3: pK, = 4.74 %3D CH3NH3: pKp = 3.36 %3D NH3 < CH3NH3 < HNO3 < HNO2 < HCIO NH3 < CH3NH3 < HCIO < HNO2 < HNO3 HNO3 < HNO2 < HCIO < CH3NH3 < NH3 HNO3 < HNO2 < HCIO < NH3 < CH3NH3

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 21Q

See similar textbooks

Similar questions

Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
. Strong buses are bases that completely ionize in water to produce hydroxide ion, OH-. The strong bases include the hydroxides of the Group I elements. For example, if 1.0 mole of NaOH is dissolved per liter, the concentration of OH ion is 1.0 M. Calculate the [OH-], pOH, and pH for each of the following strong base solutions. a. 1.10 M NaOH b. 2.0104M KOH c. 6.2103M CsOH d. 0.0001 M NaOH
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Calculate the ionization constant for each of the following acids or bases form the ionization constant of its conjugate base or conjugate acid: (a) F- (b) NH4+ (c) AsO43- (d) (CH3)2 NH2+ (e) NO2- (f) HC2O4- (as a base)
The pH of a 0.10-M solution of caffeine is 11.16. Determine Kb for caffeine from these data: C8H10N4O2(aq)+H2O(l)C8H10N4O2H+(aq)+OH(aq)