Question

Values for Ka for three weak acids are given below, at T = 25 C, along...

Values for Ka for three weak acids are given below, at T = 25 C, along with their conjugate bases

formic acid (HCOOH)   Ka = 1.7 x 10-4 conjugate base = HCOO-

hypoiodic acid (HIO)   Ka = 2.3 x 10-11 conjugate base = IO-

phenol (C6H5OH) Ka = 1.3 x 10-10 conjugate base = C6H5O-

Based on this information, we can say

a) HCOO- is a stronger base than IO-

b) HCOO- is a stronger base that C6H5O-

c) IO- is a stronger base than C6H5O-

d) Both a and b

e) All three conjugate bases are the same strength

Homework Answers

Answer #1

According to Bronsted -Lowry concept

if the acid were stronger its conjugate base is weak. The higher the Ka value the stronger is the acid.

Thus let us arrange the acids in decreasing order of strength using their Ka values.

formic acid > phenol > HIO

Thus the conjugate bases have the strength in reverse order

HCOO- < C6H5O- < IO-

Thus only option C is correct ( IO- is stronger base than both C6H5O- and HCOO-) as it is the conjugate base of weakest acid HIO

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the pH of a 0.334 M aqueous solution of phenol (a weak acid) (C6H5OH, Ka...
Calculate the pH of a 0.334 M aqueous solution of phenol (a weak acid) (C6H5OH, Ka = 1.0×10-10) and the equilibrium concentrations of the weak acid and its conjugate base. pH =    [C6H5OH ]equilibrium =    M [C6H5O- ]equilibrium =    M
From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for...
From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases. a) CH3CO2H: [H3O+]= 1.34 x 10^-3 [CH3CO2H]= 9.866 x 10^-2 [CH3CO2-]= 1.34 x 10^-3 b) ClO- [OH-]= 4.0 x 10^-4 [HClO]= 2.38 x 10^-5 [ClO-]= 0.273 M
For the following questions refer to the table below. Acids Ka HNO2 4.0 x 10-4 HCl...
For the following questions refer to the table below. Acids Ka HNO2 4.0 x 10-4 HCl 3.1 x 106 HCN 6.2 x 10-10 HClO4 > 1.0 x 1010 H2SO4 1.0 x 103 HBrO 2.0 x 10-9 HIO3 1.6 x 10-1 Rank the following bases from strongest to weakest base. NO2-, Cl-, CN-, ClO4-, BrO- What are the following Kb values at 25 ᵒC? CN- BrO- NO2- HSO4- Which acid from the table would be the weakest acid?
Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms...
Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized as NX3(aq)+H2O(l)⇌HNX3+(aq)+OH−(aq) where NX3 is the base and HNX3+ is the conjugate acid. The equilibrium-constant expression for this reaction is Kb=[HNX3+][OH−]/[NX3] where Kb is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of Kb increases. Ka and Kb are related through...
1. Organize the following acids form strongest to weakest. aqua acid among these three: [Fe(H2O)6]3+, [Zn(H2O)6]2+...
1. Organize the following acids form strongest to weakest. aqua acid among these three: [Fe(H2O)6]3+, [Zn(H2O)6]2+ and [Mg(H2O)6]2+. Explain you answer. 2. If you replace one -OH group in H2SO4 with –CCl3, a. the resulting acid, H(CCl3)SO3 is weaker than H2SO4. b. the resulting acid, H(CCl3)SO3 is stronger than H2SO4 c. we cannot say anything about the acidity of the new compound relative to H2SO4. 3. Consider a solvent AB that undergoes autoionization to produce AB2– and A+ ions. Then...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...