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Science Chemistry CHEMISTRY 1111 LAB MANUAL >C<

The given statement that is should be proved. Concept Introduction: Acid ionization constant K a : The equilibrium expression for the reaction HA ( a q ) ⇌ H + ( a q ) + A - ( a q ) is given below. K a = [ H + ][A - ] [ HA] Where K a is acid ionization constant, [ H + ] is concentration of hydrogen ion, [ A - ] is concentration of acid anion, [ HA] is concentration of the acid Base ionization constant K b The equilibrium expression for the ionization of weak base B will be, B ( a q ) + H 2 O ( l ) ⇌ HB + ( a q ) + OH - ( a q ) K b = [ HB + ] [ OH - ] [ B ] Where K b is base ionization constant, [ OH − ] is concentration of hydroxide ion, [ HB + ] is concentration of conjugate acid, [ B] is concentration of the base Relationship between K a and K b K a × K b =K w

The given statement that is should be proved. Concept Introduction: Acid ionization constant K a : The equilibrium expression for the reaction HA ( a q ) ⇌ H + ( a q ) + A - ( a q ) is given below. K a = [ H + ][A - ] [ HA] Where K a is acid ionization constant, [ H + ] is concentration of hydrogen ion, [ A - ] is concentration of acid anion, [ HA] is concentration of the acid Base ionization constant K b The equilibrium expression for the ionization of weak base B will be, B ( a q ) + H 2 O ( l ) ⇌ HB + ( a q ) + OH - ( a q ) K b = [ HB + ] [ OH - ] [ B ] Where K b is base ionization constant, [ OH − ] is concentration of hydroxide ion, [ HB + ] is concentration of conjugate acid, [ B] is concentration of the base Relationship between K a and K b K a × K b =K w

Solution Summary: The author explains the equilibrium expression for the ionization of weak base B.

CHEMISTRY 1111 LAB MANUAL >C<

CHEMISTRY 1111 LAB MANUAL >C<

1st Edition

ISBN: 9781307092097

Author: Chang

Publisher: MCG/CREATE

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Question

Chapter 15, Problem 15.151QP

Interpretation Introduction

Interpretation:

The given statement that is should be proved.

Concept Introduction:

Acid ionization constant $Ka$ :

The equilibrium expression for the reaction $HA(aq)⇌H+(aq)+A-(aq)$ is given below.

$Ka = [H+][A-][HA]$

Where $Ka$ is acid ionization constant, $[H+]$ is concentration of hydrogen ion, $[A-]$ is concentration of acid anion, $[HA]$ is concentration of the acid

Base ionization constant $Kb$

The equilibrium expression for the ionization of weak base $B$ will be,

$B(aq)+H2O(l) ⇌ HB+(aq)+OH-(aq)$

$Kb=[HB+][OH-][B]$

Where $Kb$ is base ionization constant, $[OH−]$ is concentration of hydroxide ion, $[HB+]$ is concentration of conjugate acid, $[B]$ is concentration of the base

Relationship between $Ka$ and $Kb$

$Ka×Kb=Kw$

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Chapter 15, Problem 15.150QP

Chapter 15, Problem 15.152QP

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Chapter 15 Solutions

CHEMISTRY 1111 LAB MANUAL >C<

Ch. 15.1 - Identify the conjugate acid-base pairs for the...Ch. 15.1 - Which of the following does not constitute a...Ch. 15.2 - Prob. 2PE Ch. 15.2 - Prob. 1RC Ch. 15.3 - Nitric acid (HNO3) is used in the production of...Ch. 15.3 - The pH of a certain orange juice is 3.33....Ch. 15.3 - Prob. 5PE Ch. 15.3 - Which is more acidic: a solution where [H+] =2.5 ...Ch. 15.4 - Prob. 6PE Ch. 15.4 - Predict whether the equilibrium constant for the...

Ch. 15.4 - Prob. 1RC Ch. 15.5 - What is the pH of a 0.122 M monoprotic acid whose...Ch. 15.5 - The pH of a 0.060 M weak monoprotic acid is 3.44....Ch. 15.5 - The concentration of water is 55.5 M. Calculate...Ch. 15.6 - Calculate the pH of a 0.26 M methylamine solution...Ch. 15.6 - Consider the following three solutions of equal...Ch. 15.7 - Consider the following two acids and their...Ch. 15.8 - Calculate the concentrations of H2C2O4, HC2O4,...Ch. 15.8 - Which of the diagrams (a)(c) represents a solution...Ch. 15.9 - Which of the following acids is weaker: HClO2 or...Ch. 15.10 - Calculate the pH of a 0.24 M sodium formate...Ch. 15.10 - Prob. 14PE Ch. 15.10 - The diagrams shown here represent solutions of...Ch. 15.11 - Prob. 1RC Ch. 15.12 - Identify the Lewis acid and Lewis base in the...Ch. 15.12 - Prob. 1RC Ch. 15 - Define Brnsted acids and bases. Give an example of...Ch. 15 - Prob. 15.2QP Ch. 15 - Classify each of the following species as a...Ch. 15 - Write the formulas of the conjugate bases of the...Ch. 15 - Identify the acid-base conjugate pairs in each of...Ch. 15 - Write the formula for the conjugate acid of each...Ch. 15 - Prob. 15.7QP Ch. 15 - Write the formula for the conjugate base of each...Ch. 15 - What is the ion-product constant for water?Ch. 15 - Write an equation relating [H+] and [OH] in...Ch. 15 - Prob. 15.12QP Ch. 15 - The pH of a solution is 6.7. From this statement...Ch. 15 - Define pOH. Write the equation relating pH and...Ch. 15 - Calculate the concentration of OH ions in a 1.4 ...Ch. 15 - Calculate the concentration of H+ ions in a 0.62 M...Ch. 15 - Calculate the pH of each of the following...Ch. 15 - Calculate the pH of each of the following...Ch. 15 - Calculate the hydrogen ion concentration in mol/L...Ch. 15 - Calculate the hydrogen ion concentration in mol/L...Ch. 15 - Complete the following table for a solution: pH...Ch. 15 - Fill in the word acidic, basic, or neutral for the...Ch. 15 - The pOH of a strong base solution is 1.88 at 25C....Ch. 15 - Calculate the number of moles of KOH in 5.50 mL of...Ch. 15 - How much NaOH (in grams) is needed to prepare 546...Ch. 15 - A solution is made by dissolving 18.4 g of HCl in...Ch. 15 - Prob. 15.27QP Ch. 15 - Prob. 15.28QP Ch. 15 - Prob. 15.29QP Ch. 15 - Prob. 15.30QP Ch. 15 - Which of the following diagrams best represents a...Ch. 15 - (1) Which of the following diagrams represents a...Ch. 15 - Classify each of the following species as a weak...Ch. 15 - Classify each of the following species as a weak...Ch. 15 - Which of the following statements is/are true for...Ch. 15 - Which of the following statements is/are true...Ch. 15 - Predict the direction that predominates in this...Ch. 15 - Predict whether the following reaction will...Ch. 15 - What does the ionization constant tell us about...Ch. 15 - List the factors on which the Ka of a weak acid...Ch. 15 - Prob. 15.41QP Ch. 15 - Which of the following solutions has the highest...Ch. 15 - The Ka for benzoic acid is 6.5 105. Calculate the...Ch. 15 - A 0.0560-g quantity of acetic acid is dissolved in...Ch. 15 - The pH of an acid solution is 6.20. Calculate the...Ch. 15 - What is the original molarity of a solution of...Ch. 15 - Calculate the percent ionization of benzoic acid...Ch. 15 - Calculate the percent ionization of hydrofluoric...Ch. 15 - A 0.040 M solution of a monoprotic acid is 14...Ch. 15 - (a) Calculate the percent ionization of a 0.20 M...Ch. 15 - Use NH3 to illustrate what we mean by the strength...Ch. 15 - Which of the following has a higher pH: (a) 0.20 M...Ch. 15 - Calculate the pH of a 0.24 M solution of a weak...Ch. 15 - The diagrams here represent three different weak...Ch. 15 - Calculate the pH for each of the following...Ch. 15 - The pH of a 0.30 M solution of a weak base is...Ch. 15 - What is the original molarity of a solution of...Ch. 15 - In a 0.080 M NH3 solution, what percent of the NH3...Ch. 15 - Write the equation relating Ka for a weak acid and...Ch. 15 - From the relationship KaKb = Kw, what can you...Ch. 15 - Prob. 15.61QP Ch. 15 - Write all the species (except water) that are...Ch. 15 - The first and second ionization constants of a...Ch. 15 - Compare the pH of a 0.040 M HCl solution with that...Ch. 15 - What are the concentrations of HSO4, SO42 and H+...Ch. 15 - Calculate the concentrations of H+, HCO3, and CO32...Ch. 15 - Prob. 15.67QP Ch. 15 - Prob. 15.68QP Ch. 15 - Predict the acid strengths of the following...Ch. 15 - Compare the strengths of the following pairs of...Ch. 15 - Which of the following is the stronger acid:...Ch. 15 - Prob. 15.72QP Ch. 15 - Define salt hydrolysis. Categorize salts according...Ch. 15 - Explain why small, highly charged metal ions are...Ch. 15 - Al3+ is not a Brnsted acid but is Al(H2O)63+....Ch. 15 - Specify which of the following salts will undergo...Ch. 15 - Predict the pH ( 7, 7, or 7) of aqueous...Ch. 15 - Predict whether the following solutions are...Ch. 15 - A certain salt, MX (containing the M+ and X ions),...Ch. 15 - In a certain experiment a student finds that the...Ch. 15 - Calculate the pH of a 0.36 M CH3COONa solution.Ch. 15 - Calculate the pH of a 0.42 M NH4Cl solution.Ch. 15 - Prob. 15.83QP Ch. 15 - Predict whether a solution containing the salt...Ch. 15 - Classify the following oxides as acidic, basic,...Ch. 15 - Write equations for the reactions between (a) CO2...Ch. 15 - Explain why metal oxides tend to be basic if the...Ch. 15 - Prob. 15.88QP Ch. 15 - Zn(OH)2 is an amphoteric hydroxide. Write balanced...Ch. 15 - Al(OH)3 is an insoluble compound. It dissolves in...Ch. 15 - Prob. 15.91QP Ch. 15 - In terms of orbitals and electron arrangements,...Ch. 15 - Classify each of the following species as a Lewis...Ch. 15 - Describe the following reaction in terms of the...Ch. 15 - Which would be considered a stronger Lewis acid:...Ch. 15 - All Brnsted acids are Lewis acids, but the reverse...Ch. 15 - Determine the concentration of a NaNO2 solution...Ch. 15 - Determine the concentration of a NH4Cl solution...Ch. 15 - Prob. 15.99QP Ch. 15 - A typical reaction between an antacid and the...Ch. 15 - Prob. 15.101QP Ch. 15 - The pH of a 0.0642 M solution of a monoprotic acid...Ch. 15 - Like water, liquid ammonia undergoes...Ch. 15 - HA and HB are both weak acids although HB is the...Ch. 15 - A solution contains a weak monoprotic acid HA and...Ch. 15 - The three common chromium oxides are CrO, Cr2O3,...Ch. 15 - Prob. 15.107QP Ch. 15 - Use the data in Table 15.3 to calculate the...Ch. 15 - Prob. 15.109QP Ch. 15 - Calculate the pH of a 0.20 M ammonium acetate...Ch. 15 - Novocaine, used as a local anesthetic by dentists,...Ch. 15 - Prob. 15.112QP Ch. 15 - Prob. 15.113QP Ch. 15 - The ion product of D2O is 1.35 1015 at 25C. (a)...Ch. 15 - Give an example of the following: (a) a weak acid...Ch. 15 - Prob. 15.116QP Ch. 15 - Prob. 15.117QP Ch. 15 - Prob. 15.118QP Ch. 15 - When chlorine reacts with water, the resulting...Ch. 15 - When the concentration of a strong acid is not...Ch. 15 - Calculate the pH of a 2.00 M NH4CN solution.Ch. 15 - Calculate the concentrations of all species in a...Ch. 15 - Identify the Lewis acid and Lewis base that lead...Ch. 15 - Very concentrated NaOH solutions should not be...Ch. 15 - In the vapor phase, acetic acid molecules...Ch. 15 - Calculate the concentrations of all the species in...Ch. 15 - Prob. 15.127QP Ch. 15 - Prob. 15.128QP Ch. 15 - How many grams of NaCN would you need to dissolve...Ch. 15 - A solution of formic acid (HCOOH) has a pH of...Ch. 15 - Prob. 15.131QP Ch. 15 - A 1.87-g sample of Mg reacts with 80.0 mL of a HCl...Ch. 15 - Prob. 15.133QP Ch. 15 - Prob. 15.134QP Ch. 15 - Prob. 15.135QP Ch. 15 - Prob. 15.136QP Ch. 15 - Prob. 15.137QP Ch. 15 - Prob. 15.138QP Ch. 15 - Prob. 15.139QP Ch. 15 - The atmospheric sulfur dioxide (SO2) concentration...Ch. 15 - Calcium hypochlorite [Ca(OCl)2] is used as a...Ch. 15 - Prob. 15.142QP Ch. 15 - About half of the hydrochloric acid produced...Ch. 15 - Prob. 15.144QP Ch. 15 - Prob. 15.145QP Ch. 15 - How many milliliters of a strong monoprotic acid...Ch. 15 - Prob. 15.147QP Ch. 15 - Prob. 15.148QP Ch. 15 - Prob. 15.149QP Ch. 15 - A 1.294-g sample of a metal carbonate (MCO3) is...Ch. 15 - Prob. 15.151QP Ch. 15 - Calculate the pH of a solution that is 1.00 M HCN...Ch. 15 - Prob. 15.153QP Ch. 15 - Use the vant Hoff equation (see Problem 14.119.)...Ch. 15 - At 28C and 0.982 atm, gaseous compound HA has a...Ch. 15 - Prob. 15.156QP Ch. 15 - Calculate the pH of a 0.20 M NaHCO3...Ch. 15 - Prob. 15.158QP Ch. 15 - In this chapter, HCl, HBr, and HI are all listed...Ch. 15 - Use the data in Appendix 2 to calculate the for...Ch. 15 - Malonic acid [CH2(COOH)2] is a diprotic acid....Ch. 15 - Look up the contents of a Tums tablet. How many...Ch. 15 - Phosphorous acid, H3PO3(aq), is a diprotic acid...Ch. 15 - Chicken egg shells are composed primarily of...

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