What is the pH of a solution prepared by mixing 10.0 ml of 0.100 M NaoH with 15.

Question

What is the pH of a solution prepared by mixing 10.0 ml of 0.100 M NaoH with 15.0 mL of 0.100 M HCl? Assume the volumes of additives Show how formic acid CHCOOH, dissociates in solution men of at M solution Ka for formic acid 3, show how methylamine, dissociates solution then alternative pH of an M solution of the base. Ks for methylamine i44 10 4 a calculate K. for the anilinium ion ion given that k for aniline (cat is 1.5 b) Calculate K for the cyanide ion given Ka for Show how the following ions are hydrolyzed in water and tell if the ion would give an acidic or basic solution: i) CH_3CO_2 ii) Nh_4 iii) F 6. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of025 M ammonia and 15.0 mL of 0.15 M in ammonium chloride. Assume the volumes are additive. Kb for ammonia is 1.8 x 10^-5.

Explanation / Answer

1)
moles of NaOH added = M*V = 0.100 M * 10 mL = 1 mmol
moles of HCl added = M*V = 0.100 M * 15 mL = 1.5 mmol

1 mmol of each will react to form neutral solution

remaining moles of HCl = 1.5 mmol - 1 mmol = 0.5 mmol

total volume = 10.0 mL + 15.0 mL = 25.0 mL

[H+] = number of mol/ volume
= 0.5 mmol / 25 mL
= 0.02 M

pH = -log [H+]
= - log (0.02)
= 1.70

Answer: 1.70

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