What is the pH of a buffer solution in which the molar concentration of acetic acid is 0.15M and the molar mass concentration of the acetate ion is 0.55M? ka(acetic acid)=1.8 x 10-5 a. 5.30  b. 12.93  c. 5.01 d. 4.74

Ka of acetic acid equals 1.8*10^-5 The buffer solution is 50 mL of 0.2 M CH3CO2H and 50 mL of 0.2 M NaCH3CO2together in a beaker.  What is the theoretical pH of each soluton? a. 50 mL of boiled deionized water + 5 mL of 0.2 M HClb. 50 mL of boiled deionized water + 5 mL of 0.2 M NaOHc. 50 mL of buffer + 5 mL of 0.2 M HCld. 50 mL of buffer + 5 mL of 0.2 M NaOH

For a titration of HCl with NaOH, 3.0 mL of 0.4 M NaOH are needed to neutralize 4.0 mL of the HCI. What is the molarity of the HCI? O 960 M O 0.15 M O .3 M O .0096 M

You have 50.00 mL of a solution that is 0.100 M in aceticacid, and you neutralize it by adding 50.00 mL of a solution that is 0.100 M in sodium hydroxide. The pH of the resulting solution is not 7.00. Explain why. Is the pH of the solution greater than or less than 7?

7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?

Consider a buffer solution prepared by adding 0.45 mol of CH3COOK to 1.00 L of 2.00 M CH3COOH. (K₁ = 1.8 x 10-5). If 0.05 mol of HCI is added to this buffer solution the pH of the solution will drop slightly. The pH does not drastically decrease because the HCI reacts with present in the buffer solution. Select one: O a. H₂O O b. CH3COOH O C. CH3COO O d. H+

1.  all the aqueous solutions that are good buffer systems 2.  a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is the PH of this buffer solution. b. a buffer solution is 0.495 m in h2s and 0.354 m in khs, if Ka1 for H2s is 1.0 * 10^-7. what is the PH of this buffer solution. c. a buffer solution is 0.455 m in NaHSO and 0.299 m in Na2SO3, if Ka for HSO3 is 6.4 * 10^-8. what is the PH of this buffer solution.  3. A 28.9 ml sample of a 0.385 m aqueous hydrocyanic acid solution is titrated with a 0.372 m aqueous sodium hydroxide solution. what is the ph at the start of the titration, before any sodium hydroxide has been added. b. A 31.9 ml sample of a 0.599 m aqueous hydrofluoric acid solution is titrated with a 0.242 m aqueous barium hydroxide solution. what is the ph after 15.8ml of base has been added. c. when a 23.8 ml sample of a 0.357 m aqueous acetic acid solution is titrated with a 0.459 m aqueous barium hydroxide solution. what is the ph…

Calculate the expected pH of the buffer.

Could you solve this problem, question 36?

K Please don't provide the handwriting solution An analytical chemist is titrating 133.6mL of a .3400M solution of hydrazoic acid (HN3) with a .3500 M solution of KOH. The pKa of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 51.85mL of the KOH solution to it.