Question 3 1 pts Consider a 0.1 M solution of the weak acid CH3COOH with a...
Consider a buffer composed of the weak acid acetic acid (CH3COOH) and the conjugate base sodium acetate (NaCH3COO). Which pair of concentrations results in the most effective buffer (i.e. has the highest buffer capacity)? A. 0.10 M CH3COOH; 0.10 M NaCH3COO B. 0.90 M CH3COOH; 0.10 M NaCH3COO C. 0.10 M CH3COOH; 0.90 M NaCH3COO D. 0.50 M CH3COOH; 0.50 M NaCH3COO
Acetic acid (CH3COOH,CH3COOH, ?a=5.62×10−5)Ka=5.62×10−5) is a weak acid, so the salt sodium acetate (CH3COONa)CH3COONa) acts as a weak base. Calculate the pH of a 0.445 M0.445 M solution of sodium acetate.
1. Calculate pH of CH3COOH. The concentration of this species is O.33 M. Ka = 1.8x10^-5 (six decimal places) 2. Calculate pH of NH4OH. The concentration kf this species is 0.49 M. Ka= 1.8x10^-5 (six decimal places) 3. How do I figure out is an aqueous solution of a salt is acidic, basic, or neutral? Can you explain it by using this as an example; Sodium acetate, NaCH3COO?
Question 1 1 pts Consider a solution that is 0.1 M HF and 0.1 M NaF. This is a mixture of conjugates in equal proportions, which tells you that it is a buffer. What two reactions are relevant to the pH in this situation? NaF --> Nat + F F+H2O <--> HF + OH- HF + NaF --> H+ +Na+ + F2 HF <--> H+ +F Ht+F<--> Nat + F" Question 2 1 pts A buffer solution contains a mixture...
In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is the pH calculated before the titrant is added? The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is 14. The pH is 7. The pH is calculated using the H-H equation for a buffer solution, using the ratio of the concentrations of the base...
A solution is 0.031 M in acetic acid, CH3COOH, and has a pH of 3.97. What is the concentration of acetate ion? (Ka of acetic acid 1.8x10-5)
3. One liter of buffer solution was prepared by mixing 0.1 mole of acetic acid CH3COOH and 0.05 mole of sodium acetate CH3COONa. Calculate a. pH of that solution b. How much of a strong base, say NaOH, in mol/L needs to be added to that solution to change its pH to 6.0? Notes and useful data: For acetic acid pK4.75 For carbonic acid pKa 6.3 and pKa 10.3 Sodium acetate CH3COONa dissociates entirely to Na'CH3COO
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M HCl to 100 ml of the buffer in part a.
Please Help a) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. B) calculate the pH of the buffer if you add 10 ml of 0.1 M HCL to 100ml of the buffer in part a.
A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). Question options: a) pH= 7.00 b) pH= 5.28 c) pH = 4.56 d) pH= 4.74