Abuler coAirs the weak acia HA ad is conugate base A. The weak acid has a pK, of 4.36 and the buffler has a pH of 4.92. Part A Which statemeant is true of the relative concentrations of the wweak acid and coniugate base in the bufter? O [HA| = |A"| O [HA| < [A| O [HA| > LA | Submit Request Answor Part B Which buffer component wauld you acid to change the pH vi the butfer ta 4.72? O HA

Abuler coAirs the weak acia HA ad is conugate base A. The weak acid has a pK, of 4.36 and the buffler has a pH of 4.92. Part A Which statemeant is true of the relative concentrations of the wweak acid and coniugate base in the bufter? O [HA| = |A"| O [HA| < [A| O [HA| > LA | Submit Request Answor Part B Which buffer component wauld you acid to change the pH vi the butfer ta 4.72? O HA

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.17QAP

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For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At equilibrium after partial dissociation, its pH is found to be 5.05. What is the acid ionization constant, Ka, for hypobromous acid at this temperature?
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. Use 1.80105 as Ka for acetic acid. (a) What is the pH of the solution? (b) Is the solution acidic or basic? (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of the original buffer?
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?