Ka of acetic acid is 1.77 x10$? Problem: A buffer is prepared containing 1.00 molar acetic acid and 0.800 molar sodium acetate. What is its pH if the Problem: A buffer is prepared containing 1.00 molar acetic acid and 0.800 molar sodium acetate. What is its pH if the Ka of acetic acid is 1.77 x105?
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Step by step
Solved in 2 steps with 2 images
- The answer choice for first blank is decrese or increase The answer choice for second blank is base, acid, or buffer The answer choice for third blank is shown in pictureAnswer briefly. How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?Explain please. Draw Fisher of both
- please help? make the answer clearplease help!! In the previous step, you determined there is 0.091 M excess hydroxide in the solution. What is the pH of the solution?I was under the impression that in acid + base interactions, the conjugates were the opposite of what we listed as either the acid or base. For example in the second image, the conjugate to the parent base is conjugate acid. But I was reviewing practice problems and the conjugates don't coincide with my interpretation. How then do I assign conjugates?
- Solve the second part only It’s experiment: Determination of the dissociation constant and concentration of a weak acidCan you explain why the attached set of work is incorrect. The problem is the following: Determine the pH of a .25 M CH3NH3Cl solution (Ka for CH3NH3+ = 2.3*10^-11)(Show the dissociation equation for salt. Show the reaction of CH3NH3 ion in H2O)For the column relative strength you must rank from strongest to weakest. 1 is the strongest , 2 in the middle and 3 is the weakest