Please rank from 1(lowest) to 4(highest) O ACIDS AND BASESPredicting the qualitative acid-base properties of saltsConsider the following data on some weak acids and weak bases:acidbaseK.K,nameformulanameformulaHNO, 4.5 x 10aniline C,H,NH, 4.3× 10¬10-4nitrous acidhydrofluoric acidHF-46.8 x 10pyridine C3H,N |1.7×10-9Use 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 tothe solution that will have the next lowest pH, and so on.solutionpH0.1 M CGH5NH3B.choose onev0.1 М KFchoose onev0.1 M NaNO2choose onev0.1 М КBrchoose one v

more PH , lesser the acidic value

Consider the following data on some weak acids and weak bases: acid base K, name formula name formula HNO, 4.5 x 10 aniline C,H5NH,|4.3× 10¯ - 10 -4 nitrous acid hydrofluoric acid HF 6.8 × 10 pyridine C3H,N |1.7×10¬9 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 CgHgNH3Br choose one v 0.1 M KF choose onev 0.1 M NaNO2 choose one v 0.1 M KBr choose onev ?

Consider the following data on some weak acids and weak bases: acid base K, name formula name formula HNO, 4.5 x 10 aniline C,H5NH,|4.3× 10¯ - 10 -4 nitrous acid hydrofluoric acid HF 6.8 × 10 pyridine C3H,N |1.7×10¬9 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 CgHgNH3Br choose one v 0.1 M KF choose onev 0.1 M NaNO2 choose one v 0.1 M KBr choose onev ?

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

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.87QE

See similar textbooks

Similar questions

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?
State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species. (a) NH3. (b) HPO4-. (c) Br-. (d) NH4+. (e) ASO43-
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.
The hydroxide ion concentration, [OH-], of an aqueous solution of 0.558 M triethylamine (a weak base with the formula (C2H5)3N) , Kb = 5.2×10-4, is: [OH-] = M
Many moderately large organic molecules containing basicnitrogen atoms are not very soluble in water as neutral molecules,but they are frequently much more soluble as theiracid salts. Assuming that pH in the stomach is 2.5, indicatewhether each of the following compounds would be presentin the stomach as the neutral base or in the protonatedform: nicotine, Kb = 7 x 10-7; caffeine, Kb = 4 x10-14;strychnine, Kb = 1 x 10-6; quinine, Kb = 1.1 x 10-6.
The hydroxide ion concentration, [OH-], of an aqueous solution of 0.421 M diethylamine (a weak base with the formula (C2H5)2NH) , Kb = 6.9×10-4, is:
The hydroxide ion concentration of an aqueous solution of 0.429 N acetylsalicylic acid (aspirin), HC9H7O4, is [OH-] = ________ M.
What is the pH of an aqueous solution of 0.005 M C6H5O- at 298 K of the Ka for phenol at the given T is 1.0 x 10⎯10?
The hydroxide ion concentration, [OH-], of an aqueous solution of 0.441 M triethanolamine (a weak base with the formula C6H15O3N) , Kb = 5.8×10-7, is: [OH-] = __________ M.
Oxalic acid (H2C2O4) is a diprotic acid with Ka1=5.6×10-1 and Ka2=1.5×10-4. Oxalate ion (C2O42-) also has two base dissociation constants, Kb(1) =6.5×10-11 and Kb2=1.8×10-14. Based on these values, deduce the formula to compute the base dissociation constants of oxalate ion in terms of Kw and Ka1 or Ka2.
Carry out the phosphoric acid dissociation and write the expression of all the species of said dissociation