Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
9th Edition
ISBN: 9781260477467
Author: Martin Silberberg
Publisher: Mcgraw-hill Higher Education (us)
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Chapter 19.2, Problem 19.4AFP

(a)

Interpretation Introduction

Interpretation:

For the titration of 30.00 mL and 0.2000MHBrO of Ka=6.3×105 with 0.1000 M NaOH solution before the addition of pH has to be calculated.

Concept introduction:

pH: pH is the logarithm of the reciprocal of the concentration of H3O+ in a solution. The pH of a solution is a measure of concentration of hydrogen ion in a solution. Lower pH due to more hydrogen ions and higher pH due to less concentration of hydrogen ions.

  pH=pKa+log[conjugate base][acid]

It is a Henderson-Hasselbalch equation.

  pKa=pH+log[HA][A-]

Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid. For a dissociation of acid (HA) in aqueous solution,

  HA+H2OH3O++A

  pKa=pH+log[HA][A]

During a dissociation of acid in aqueous solution,

  • If pH=pKa, the concentration of compound in its acidic and basic form is equal.
  • If pH<pKa, the compound exist in its acidic form.
  • If pH>pKa, the compound exist in its basic form.

(b)

Interpretation Introduction

Interpretation:

For the titration of 30.00 mL and 0.2000MHBrO of Ka=6.3×105 with 0.1000 M NaOH the solution equilibrium and solution pH has to be calculated.

Concept introduction:

pH: pH is the logarithm of the reciprocal of the concentration of H3O+ in a solution. The pH of a solution is a measure of concentration of hydrogen ion in a solution. Lower pH due to more hydrogen ions and higher pH due to less concentration of hydrogen ions.

  pH=pKa+log[conjugate base][acid]

Henderson-Hasselbalch equation

  pKa=pH+log[HA][A-]

Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid. For a dissociation of acid (HA) in aqueous solution,

  HA+H2OH3O++A

  pKa=pH+log[HA][A]

During a dissociation of acid in aqueous solution,

  • If pH=pKa, the concentration of compound in its acidic and basic form is equal.
  • If pH<pKa, the compound exist in its acidic form.
  • If pH>pKa, the compound exist in its basic form.

(c)

Interpretation Introduction

Interpretation:

For the titration of 30.00 mL and 0.2000MHBrO of Ka=6.3×105 with 0.1000 M NaOH the solution equilibrium and solution pH has to be calculated.

Concept introduction:

pH: pH is the logarithm of the reciprocal of the concentration of H3O+ in a solution. The pH of a solution is a measure of concentration of hydrogen ion in a solution. Lower pH due to more hydrogen ions and higher pH due to less concentration of hydrogen ions.

  pH=pKa+log[conjugate base][acid]

It is a Henderson-Hasselbalch equation.

Henderson-Hasselbalch equation

  pKa=pH+log[HA][A-]

Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid. For a dissociation of acid (HA) in aqueous solution,

  HA+H2OH3O++A

  pKa=pH+log[HA][A]

During a dissociation of acid in aqueous solution,

  • If pH=pKa, the concentration of compound in its acidic and basic form is equal.
  • If pH<pKa, the compound exist in its acidic form.
  • If pH>pKa, the compound exist in its basic form.

(d)

Interpretation Introduction

Interpretation:

For the titration of 30.00 mL and 0.2000MHBrO of Ka=6.3×105 with 0.1000 M NaOH the amount of OH added is twice the amount of HBrO initially present should be calculated.

Concept introduction:

pH: pH is the logarithm of the reciprocal of the concentration of H3O+ in a solution. The pH of a solution is a measure of concentration of hydrogen ion in a solution. Lower pH due to more hydrogen ions and higher pH due to less concentration of hydrogen ions.

  pH=pKa+log[conjugate base][acid]

It is a Henderson-Hasselbalch equation.

Henderson-Hasselbalch equation

  pKa=pH+log[HA][A-]

Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid. For a dissociation of acid (HA) in aqueous solution,

  HA+H2OH3O++A

  pKa=pH+log[HA][A]

During a dissociation of acid in aqueous solution,

  • If pH=pKa, the concentration of compound in its acidic and basic form is equal.
  • If pH<pKa, the compound exist in its acidic form.
  • If pH>pKa, the compound exist in its basic form.

(e)

Interpretation Introduction

Interpretation:

The titration curve and label the pKa value and equivalent point of given titration point has to sketch.

Concept introduction:

pH: pH is the logarithm of the reciprocal of the concentration of H3O+ in a solution. The pH of a solution is a measure of concentration of hydrogen ion in a solution. Lower pH due to more hydrogen ions and higher pH due to less concentration of hydrogen ions.

  pH=pKa+log[conjugate base][acid]

It is a Henderson-Hasselbalch equation.

Henderson-Hasselbalch equation

  pKa=pH+log[HA][A-]

Henderson-Hasselbalch equation explains the relationship between pH of solution and pKa of acid. For a dissociation of acid (HA) in aqueous solution,

  HA+H2OH3O++A

  pKa=pH+log[HA][A]

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Chapter 19 Solutions

Chemistry: The Molecular Nature of Matter and Change

Ch. 19.3 - Prob. 19.6AFPCh. 19.3 - Prob. 19.6BFPCh. 19.3 - Prob. 19.7AFPCh. 19.3 - Prob. 19.7BFPCh. 19.3 - Prob. 19.8AFPCh. 19.3 - Prob. 19.8BFPCh. 19.3 - Prob. 19.9AFPCh. 19.3 - Prob. 19.9BFPCh. 19.3 - Prob. 19.10AFPCh. 19.3 - Prob. 19.10BFPCh. 19.3 - Prob. 19.11AFPCh. 19.3 - Prob. 19.11BFPCh. 19.3 - Prob. 19.12AFPCh. 19.3 - Prob. 19.12BFPCh. 19.4 - Cyanide ion is toxic because it forms stable...Ch. 19.4 - Prob. 19.13BFPCh. 19.4 - Prob. 19.14AFPCh. 19.4 - Calculate the solubility of PbCl2 in 0.75 M NaOH....Ch. 19 - Prob. 19.1PCh. 19 - Prob. 19.2PCh. 19 - Prob. 19.3PCh. 19 - Prob. 19.4PCh. 19 - Prob. 19.5PCh. 19 - Prob. 19.6PCh. 19 - Prob. 19.7PCh. 19 - Prob. 19.8PCh. 19 - Does the pH increase or decrease with each of the...Ch. 19 - The scenes below depict solutions of the same...Ch. 19 - The scenes below show three samples of a buffer...Ch. 19 - What are the [H3O+] and the pH of a propanoic...Ch. 19 - What are the [H3O+] and the pH of a benzoic...Ch. 19 - Prob. 19.14PCh. 19 - Prob. 19.15PCh. 19 - Prob. 19.16PCh. 19 - Find the pH of a buffer that consists of 0.95 M...Ch. 19 - Prob. 19.18PCh. 19 - Prob. 19.19PCh. 19 - Prob. 19.20PCh. 19 - Find the pH of a buffer that consists of 0.50 M...Ch. 19 - A buffer consists of 0.22 M KHCO3 and 0.37 M...Ch. 19 - A buffer consists of 0.50 M NaH2PO4 and 0.40 M...Ch. 19 - What is the component concentration ratio,...Ch. 19 - Prob. 19.25PCh. 19 - Prob. 19.26PCh. 19 - Prob. 19.27PCh. 19 - Prob. 19.28PCh. 19 - A buffer that contains 0.40 M of a base, B, and...Ch. 19 - A buffer that contains 0.110 M HY and 0.220 M Y−...Ch. 19 - A buffer that contains 1.05 M B and 0.750 M BH+...Ch. 19 - A buffer is prepared by mixing 204 mL of 0.452 M...Ch. 19 - A buffer is prepared by mixing 50.0 mL of 0.050 M...Ch. 19 - Prob. 19.34PCh. 19 - Prob. 19.35PCh. 19 - Prob. 19.36PCh. 19 - Choose specific acid-base conjugate pairs to make...Ch. 19 - An industrial chemist studying bleaching and...Ch. 19 - Oxoanions of phosphorus are buffer components in...Ch. 19 - The scenes below depict the relative...Ch. 19 - Prob. 19.41PCh. 19 - What species are in the buffer region of a weak...Ch. 19 - Prob. 19.43PCh. 19 - Prob. 19.44PCh. 19 - Prob. 19.45PCh. 19 - Prob. 19.46PCh. 19 - Prob. 19.47PCh. 19 - Prob. 19.48PCh. 19 - Prob. 19.49PCh. 19 - Prob. 19.50PCh. 19 - Prob. 19.51PCh. 19 - Prob. 19.52PCh. 19 - Prob. 19.53PCh. 19 - Prob. 19.54PCh. 19 - Prob. 19.55PCh. 19 - Prob. 19.56PCh. 19 - Prob. 19.57PCh. 19 - Prob. 19.58PCh. 19 - Prob. 19.59PCh. 19 - Prob. 19.60PCh. 19 - Prob. 19.61PCh. 19 - Use figure 19.9 to find an indicator for these...Ch. 19 - Prob. 19.63PCh. 19 - Prob. 19.64PCh. 19 - Prob. 19.65PCh. 19 - Prob. 19.66PCh. 19 - Write the ion-product expressions for (a) silver...Ch. 19 - Write the ion-product expressions for (a)...Ch. 19 - Write the ion-product expressions for (a) calcium...Ch. 19 - Prob. 19.70PCh. 19 - The solubility of silver carbonate is 0.032 M at...Ch. 19 - Prob. 19.72PCh. 19 - Prob. 19.73PCh. 19 - The solubility of calcium sulfate at 30°C is 0.209...Ch. 19 - Prob. 19.75PCh. 19 - Prob. 19.76PCh. 19 - Prob. 19.77PCh. 19 - Calculate the molar solubility of Ag2SO4 in (a)...Ch. 19 - Prob. 19.79PCh. 19 - Prob. 19.80PCh. 19 - Prob. 19.81PCh. 19 - Prob. 19.82PCh. 19 - Prob. 19.83PCh. 19 - Write equations to show whether the solubility of...Ch. 19 - Prob. 19.85PCh. 19 - Prob. 19.86PCh. 19 - Prob. 19.87PCh. 19 - Does any solid PbCl2 form when 3.5 mg of NaCl is...Ch. 19 - Prob. 19.89PCh. 19 - Prob. 19.90PCh. 19 - Prob. 19.91PCh. 19 - A 50.0-mL volume of 0.50 M Fe(NO3)3 is mixed with...Ch. 19 - Prob. 19.93PCh. 19 - Prob. 19.94PCh. 19 - Write a balanced equation for the reaction of in...Ch. 19 - Prob. 19.96PCh. 19 - Prob. 19.97PCh. 19 - Prob. 19.98PCh. 19 - What is [Ag+] when 25.0 mL each of 0.044 M AgNO3...Ch. 19 - Prob. 19.100PCh. 19 - Prob. 19.101PCh. 19 - Prob. 19.102PCh. 19 - When 0.84 g of ZnCl2 is dissolved in 245 mL of...Ch. 19 - When 2.4 g of Co(NO3)2 is dissolved in 0.350 L of...Ch. 19 - Prob. 19.105PCh. 19 - A microbiologist is preparing a medium on which to...Ch. 19 - As an FDA physiologist, you need 0.700 L of formic...Ch. 19 - Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2],...Ch. 19 - Water flowing through pipes of carbon steel must...Ch. 19 - Gout is caused by an error in metabolism that...Ch. 19 - In the process of cave formation (Section 19.3),...Ch. 19 - Phosphate systems form essential buffers in...Ch. 19 - The solubility of KCl is 3.7 M at 20°C. Two...Ch. 19 - It is possible to detect NH3 gas over 10−2 M NH3....Ch. 19 - Manganese(II) sulfide is one of the compounds...Ch. 19 - The normal pH of blood is 7.40 ± 0.05 and is...Ch. 19 - A bioengineer preparing cells for cloning bathes a...Ch. 19 - Sketch a qualitative curve for the titration of...Ch. 19 - Prob. 19.119PCh. 19 - The scene at right depicts a saturated solution of...Ch. 19 - Prob. 19.121PCh. 19 - The acid-base indicator ethyl orange turns from...Ch. 19 - Prob. 19.123PCh. 19 - Prob. 19.124PCh. 19 - Prob. 19.125PCh. 19 - Prob. 19.126PCh. 19 - Prob. 19.127PCh. 19 - Prob. 19.128PCh. 19 - Calcium ion present in water supplies is easily...Ch. 19 - Calculate the molar solubility of Hg2C2O4 (Ksp =...Ch. 19 - Environmental engineers use alkalinity as a...Ch. 19 - Human blood contains one buffer system based on...Ch. 19 - Quantitative analysis of Cl− ion is often...Ch. 19 - An ecobotanist separates the components of a...Ch. 19 - Some kidney stones form by the precipitation of...Ch. 19 - Prob. 19.136PCh. 19 - Prob. 19.137PCh. 19 - Because of the toxicity of mercury compounds,...Ch. 19 - A 35.0-mL solution of 0.075 M CaCl2 is mixed with...Ch. 19 - Rainwater is slightly acidic due to dissolved CO2....Ch. 19 - Prob. 19.141PCh. 19 - Ethylenediaminetetraacetic acid (abbreviated...Ch. 19 - Buffers that are based on...Ch. 19 - NaCl is purified by adding HCl to a saturated...Ch. 19 - Scenes A to D represent tiny portions of 0.10 M...Ch. 19 - Prob. 19.146PCh. 19 - Prob. 19.147PCh. 19 - Prob. 19.148P
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY