Concept explainers
(a)
Interpretation:
The equation for the equilibria is to be predicted. The
Concept introduction:
Dissociation constant
Where,
•
•
Answer to Problem 3.19P
The equation for the equilibria is
Explanation of Solution
The relation between
Where,
•
•
The base and acid is given as
The corresponding reaction is shown below.
The equation (1) for the reaction is written as shown below.
Where,
•
•
The
Substitute the value of
Therefore, the equilibrium constant for the reaction is
The equation for the equilibria is
(b)
Interpretation:
The equation for the equilibria is to be predicted. The
Concept introduction:
Dissociation constant
Where,
•
•
Answer to Problem 3.19P
The equation for the equilibria is
The equilibrium constant for the reaction is
Explanation of Solution
The relation between
Where,
•
•
The acid and base is given as
The corresponding reaction is shown below.
The equation (1) for the reaction is written as shown below.
Where,
•
•
The
Substitute the value of
Therefore, the equilibrium constant for the reaction is
The reaction in part (a) has the larger value of
The equation for the equilibria is
The reaction in part (a) has the larger value of
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Chapter 3 Solutions
Organic Chemistry Study Guide and Solutions
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- Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO,H, pK = 5.0]. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right? %3D The pKa values in Table 2.1 span a large range (-7 to 50). The pK, scale is logarithmic. small difference in pK, translates into a large numerical difference, For example, the diffe between the pK, of NH3 (38) and CH2=CH, (44) is six pKa units. This means that NH, is one million times more acidic than CH,=CH,.arrow_forwardWhy is (CH3)3Cl considered to be a Lewis Acid?arrow_forward(a) Find the equilibrium constant for following acid dissociation reaction at 25°C. Start your answer by writing the equation for Ka written with ΔG°. NH4+ ↔ NH3 + H+ Is your calculated equilibrium constant (Ka) consistent with the value given in the course handout? (b) Find Ka for the reaction at 10 and 40°C. Discuss how temperature affects fractionation between NH4+ and NH3. (c) NH3 is often called free ammonia as opposed to ammonium ion. While ammonia ions are relatively benign, free ammonia is known to be toxic for microbial growth at high concentration especially in high strength wastewater treatment. Briefly discuss about potential temperature effects on the toxicity in biological wastewater treatment.arrow_forward
- The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forwardThe ionization constant (Kb) of trimethylamine ((CH3);N) is 7.40 x 105. If 5.911 grams of trimethylamine is dissolved in 50.0 mL of water, what are the equilibrium concentration of all species present?arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning