Determine the pH of a 1.0M solution of sodium acetate (NaC2H3O2). Ka = 1.8x10-5 for acetic acid.

What is the pH of a solution formed by mixing 135.0 mL of 0.0100 M HCl with 80.0 mL of 0.0450 M NaOH? Express your answer using three decimal places. VE ΑΣΦ pH = Submit Request Answer ?

Determine the quantities shown below for a solution that is 0.0780 M in ethylamine,CH₂CH₂NH₂. The K₂ for the CH3CH₂NH₂+ ion is 2.12×10 10. K= 1.000×10-14 A. Determine the K for ethylamine,CH₂CH₂NH₂ Kb = B. Find the hydroxide ion concentration. [OH^] = C. What is the pH of this solution? pH = M (3 decimal places)

8. You will perform some calculations to see the difference between a pH buffer solution and a weak acid solution of the same pH when a small amount of strong base is added. Chlorous acid, HC1O₂, is a moderately strong acid with a Ka = 1.110×10-². Please answer the following questions. A. B. What is the molarity of the HClO₂ solution whose pH is 2.21? Please provider your answer below. 미ㄷ → Please provider your answer below. f A $ To prepare a buffer solution of the same pH, what is the molarity of the NaClO₂ if the molarity of the HC1O₂ is 0.6771 M? M → M → $