a. Please show how the weak base OCl- (aq), hypochlorite, will react with strong acid, H3O+ (aq), in a neutralization reaction. To answer this, please create two equilibria (one for the weak base dissociation, the other for the reaction of hydronium ion with dissociated hydroxide to form water; please assign values ofKc to each). Add the two equilibria to yield the net reaction; now, find the value of Kc for the net reaction. Please propose whether or not the net reaction will proceed 100% from (l --> r); please explain your proposed answer.
b. Using your net reaction from above, please determine the pH of the solution formed when 20.00 mmol of OCl- is neutralized by 20.00 mmol of HCl (aq) in a solution of volume 50.00 mL. Please rewrite your net equation and create an ICE chart to determine the mmol of products. The value of Ka for HOCl can be found in Table 14.2.
a. Please show how the weak base OCl- (aq), hypochlorite, will react with strong acid, H3O+ (aq), in a neutralization reaction. To answer this, please create two equilibria (one for the weak base dissociation, the other for the reaction of hydronium ion with dissociated hydroxide to form water; please assign values ofKc to each). Add the two equilibria to yield the net reaction; now, find the value of Kc for the net reaction. Please propose whether or not the net reaction will proceed 100% from (l --> r); please explain your proposed answer.
b. Using your net reaction from above, please determine the pH of the solution formed when 20.00 mmol of OCl- is neutralized by 20.00 mmol of HCl (aq) in a solution of volume 50.00 mL. Please rewrite your net equation and create an ICE chart to determine the mmol of products. The value of Ka for HOCl can be found in Table 14.2.
For unlimited access to Homework Help, a Homework+ subscription is required.
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Principles of Chemistry Molecular Approach
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
Chemistry: The Central Science
Related questions
For the dissociation reaction of a weak acid in water,
HA(aq)+H2O(l)âH3O+(aq)+Aâ(aq)
the equilibrium constant is the acid-dissociation constant, Ka, and takes the form
Ka=[H3O+][Aâ][HA]
Weak bases accept a proton from water to give the conjugate acid and OHâ ions:
B(aq)+H2O(l)âBH+(aq)+OHâ(aq)
The equilibrium constant Kb is called the base-dissociation constant and can be found by the formula
Kb=[BH+][OHâ][B]
When solving equilibrium-based expression, it is often helpful to keep track of changing concentrations is through what is often called an I.C.E table, where I. stands for Initial Concentration, C. stands for Change, and E. stands for Equilibrium Concentration. To create such a table, write the reaction across the top creating the columns, and the rows I.C.E on the left-hand side.
Initial (M)Change (M)Equilibrium (M)A+ BâAB
Part A
Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH. What was the Ka value calculated by the student if the pH of the solution was 2.60?
Express your answer numerically using two significant figures.
Hints
| |||||||
Ka = |
SubmitMy AnswersGive Up
Incorrect; Try Again; 3 attempts remaining
You used the initial concentration of aspirin in the Ka expression. Instead, you need to use the equilibrium concentration. Consider that the amount of aspirin that reacted is equal to the amount of H3O+ produced. How much is left over?
Part B
A 0.100 M solution of ethylamine (C2H5NH2) has a pH of 11.87. Calculate the Kb for ethylamine.
Express your answer numerically using two significant figures.
Hints
| |||
Kb = |