Calculate the pH of a solution prepared by mixing 0.080 0 mol of chloroacetic acid plus 0.040 0 mol of sodium chloroacetate in 1.00 L of water. (Assume pKa = 2.866 and Kw = 1.01 ✕ 10−14).
(a) First do the calculation by assuming that the concentrations of [HA] and [A-] equal their formal concentrations.
(b) Then do the calculation, using the real values of [HA] and [A-] in the solution.
(c) Using f rst your head, and then the Henderson-Hasselbalch equation, f nd the pH of a solution prepared by dissolving all the all the following compounds in one beaker containing a total volume of 1.00 L: 0.174 mol ClCH2CO2H, 0.026 mol ClCH2CO2Na, 0.074 mol HNO3, and 0.074 mol Ca(OH)2. Assume that Ca(OH)2 dissociates completely.
Answers: 1
Another question on Chemistry
Chemistry, 21.06.2019 18:30
For each of the following mixtures decide if filtering would be suitable to separate the substances. explain your answers. oil in water sugar in water sand in water chalk in water tea leaves in a cup of tea
Answers: 2
Chemistry, 21.06.2019 23:00
Why are the trends and exceptions to the trends in ionization energy observed?
Answers: 1
Chemistry, 22.06.2019 02:30
When svante arrhenius first proposed his acid-base theory, he was a doctoral candidate. his professors thought his ideas were unfounded. within a decade, the arrhenius theory of acid-base was widely accepted and praised within the scientific world. arrhenius defined acids as compounds having ionizable hydrogen and bases as compounds with ionizable a) barium. b) hydronium. c) hydroxide. d) oxygen.
Answers: 3
Chemistry, 22.06.2019 05:00
Choose all the answers that apply. ionic compounds dissolve easily in water do not dissolve in water have low melting points have high melting points conduct electricity when melted
Answers: 1
You know the right answer?
Calculate the pH of a solution prepared by mixing 0.080 0 mol of chloroacetic acid plus 0.040 0 mol...
Questions
