source : yahoo.com
A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution? ?
Let’s give this a try. The equation for the dissociation is
HA = H^+ + A-
If you start out with 1.25 M, and it dissociates 9.2%, then 9.2% of the starting acid is now in the form of H+ and A-. Further, the concentrations of H+ and A- are equal, both equal to 9.2% of 1.25 M: 1.25M * 0.092 = 0.115 M.
Since pH = -log[H+], that means pH = -log(0.115) = 0.94
Hope that helped!
Unit 8 Homework Answers | Ph | Acid – OH- releaser What is the definition of a Bronsted acid? Weak acids dissociate <5% What is the general equation for Ka? Acid = (25/50)(0.25 M) = 0.125 M Base = (25/50)(0.25 M) = 0.125 M Equal amounts of strong acid/weak base so should be acidic Shortcut hint- Equivalence point of a strong…A 1.25 M solution of the weak acid HA is 9.2% dissociated. Which, if any, of the following is an example of the leveling effect? In water, no acid stronger than H3O+ can exist. A solution is prepared by adding 0.10 mol of sodium sulfide, Na2S, to 1.00 L of water.The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation ?
Chemistry Exam III Flashcards | Quizlet – Know the answer? Add Answer of: 65. A 0.15 M solution of a weak acid is 3.0% dissociated. If a weak acid, HA, is 3% dissociated in a 0.25 M solution, calculate the Ka and pH of the solution. 1 attempts left Check my work Be sure to answer all parts.What is the ph of the solution? 1. See answer. The equilibrium reaction for dissociation of (weak acid) is, initially conc. c 0 0. At eqm. Concentration (c) = 1.25 M. Degree of dissociation = = 9.2% = 0.092.First, we must write the equation of the acid dissociation in water. Let's use a generic acid that we'll call 'HA.' When it dissociates, it will form H+ and A- (A- is called the the solution is a very strong acidic solution because the closer to 0 the pH value is the stronger the pH of the solution/substance.
HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the d – Regardless of the identity of the acid, a monophonic acid will undergo the following equilibrium in Further, it says that the acid (HA) is 0.01265 % dissociated, forming H+ and A-. So this would The pKa of an acid is determined by its relative strength or its degree of dissociation in water to produce…· 0.2 (M) solution of monobasic acid is dissociated to 0.95% The dissociation constant of an acid HA is 1×10−5, the pH ofThe other assumes the weak acid barely dissociates in water and approximates the pH. Which one you choose depends on how accurate you Let x represent the concentration of H+ that dissociates from HB, then [HB] = C – x where C is the initial concentration. Enter these values into the Ka equation