Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula hydrocyanic acid HCN 4.9 x 10 -10 NH3 ammonia 1.8 x 10-5 HCH3CO2 1.8 x 10¯³ -4 acetic acid methylamine CH3NH, 4.4 × 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' 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 M NH4BR choose one 0.1 М КСN choose one 0.1 M NACH3CO2 choose one 0.1 M KBr choose one

Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula hydrocyanic acid HCN 4.9 x 10 -10 NH3 ammonia 1.8 x 10-5 HCH3CO2 1.8 x 10¯³ -4 acetic acid methylamine CH3NH, 4.4 × 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' 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 M NH4BR choose one 0.1 М КСN choose one 0.1 M NACH3CO2 choose one 0.1 M KBr choose one

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.114QE

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Similar questions

Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
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
A solution of formic acid (HCOOH, Ka = 1.8 104) has a pH of 2.70. Calculate the initial concentration of formic acid in this solution.
Ethanol (ethyl alcohol), CH3CH2OH, can act as a BrnstedLowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a BrnstedLowry base. Write the chemical equation for the reaction of ethanol as a base with hydronium ion, H3O+. Explain how you arrived at these chemical equations. Both of these reactions can also be considered Lewis acid base reactions. Explain this.