How do you calculate the molar concentration of OH in a 0.075 M solution of ethylamine?

1 Answer
Apr 6, 2017

Answer:

#"Ethylamine"# acts as a Bronsted base in aqueous solution:

Explanation:

#EtNH_2(aq) + H_2O(l) rightleftharpoons EtNH_3^+ + HO^-#

#K_b=([EtNH_3^+][""^(-)OH])/([EtNH_2])#

We could solve this equation had we a value for #K_b# for #"ethylamine"#, or #K_a# for #"ethyl ammonium cation"#; such values are available, and it should have been supplied with the question.