Interpretation:
The validation corresponding to the fact that
Concept introduction:
The
This scale is defined from
Answer to Problem 20.35AP
The value of
Explanation of Solution
The given
So, the value of
The ionization table for acetic acid for initial and final concentration is given below.
The expression to calculate the value of
Substitute the values of respective concentrations and
The value of
Substitute the value of
Therefore, the value of
The given
So, the value of
The ionization table for phenol for initial and final concentration is given below.
The expression to calculate the value of
Substitute the values of respective concentrations and
Substitute the value of
Therefore, the value of
The
Want to see more full solutions like this?
Chapter 20 Solutions
Loose-leaf Version For Organic Chemistry
- Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30arrow_forwardWrite the products of these reactions. Use single or double arrows as appropriate. When you are done, label the acid and base on the left side and the conjugate acid (CA) and conjugate base (CB) on the right side. (a) PO43- + CH3NH3+ (b) H2O + H2SO4arrow_forward(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.arrow_forward
- Calculate the pH of a 0.315 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.arrow_forwardThe Ksp for In(OH)3 is 1.3 x 10-37. Find the concentration of In3+ in a buffered solution at pH 5 Find the concentration of In3+ in a buffered solution at pH 6 Find the concentration of In3+ in a buffered solution at pH 7arrow_forward1. The Ka of fluoroacetic acid is 2.5 x 10-3. Calculate the final [H+] if 1.250 molfluoroacetic acid partially dissociates in 1.00 L of water at 25 C.arrow_forward
- please help! Formic acid (Ka = 1.8 x 10-4) is used as a preservative on hay and animal feed. Hypobromous acid (Ka = 2.0 x 10-9) is used as a germicidal agent for pools and spas. An agricultural chemist wishes to test whether a mixture of the two would be more effective in preventing hay decay over the winter months. Calculate the pH of a solution that is 0.050 M in hypobromous acid and 0.025 M in formic acid.arrow_forwardThe acids are: isopropanol, ethyne, and phenol. Which acid will NOT be deprotanated by NaOH and which acid will deprotonate in the presence of NaHCO3. After an acid base reaction, which compound above has the weakest conjugate base?arrow_forward
- Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage LearningOrganic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning