A solution contains 0.159 M
C2H5NH3 and
0.177 M ethylamine,
C2H5NH2.
The pH of this solution is
.
A solution contains 0.159 M C2H5NH3 and 0.177 M ethylamine, C2H5NH2. The pH of this solution...
A. The compound ethylamine is a weak base like ammonia. A solution contains 0.268 M C2H5NH3+ and 0.151 M ethylamine, C2H5NH2. The pH of this solution is . B.A solution contains 0.335 M ammonium bromide and 0.338 M ammonia. The pH of this solution is .
The compound ethylamine is a weak base like ammonia. A solution contains 0.230 M C2H5NH3 and 0.151 M ethylamine, C2H5NH2 The pH of this solution is A solution contains 9.00x10-2 M ammonium bromide and 0.418 M ammonia. The pH of this solution is
A) The compound ethylamine is a weak base like ammonia. A solution contains 0.180 M C2H5NH3+ and 0.408 M ethylamine, C2H5NH2. The pH of this solution is .B) A solution contains 0.204 M ammonium chloride and 0.359 M ammonia. The pH of this solution is
Calculate the pH of a buffer solution that is 0.116 M in C2H5NH2 (ethylamine) and 0.403 M in C2H5NH3Cl.
Find the pH of the solution obtained when 32 mL of 0.087 M ethylamine, C2H5NH2, is titrated to the equivalence point with 0.15 M HCl. The value of Kb for ethylamine is 4.7 x 10-4. (in 3 s.f.)
Hi need help with all of these 6 questions, please!!! 1. A solution contains 0.143 M sodium fluoride and 0.189 M hydrofluoric acid. The pH of this solution is ___? 2. A solution contains 0.443 M potassium cyanide and 0.445 M hydrocyanic acid. The pH of this solution is ___? 3. The compound ethylamine is a weak base like ammonia. A solution contains 0.182 M C2H5NH3+ and 0.271 M ethylamine, C2H5NH2. The pH of this solution is ___? 4. A...
Find the [OH−] of a 0.44 M ethylamine (C2H5NH2) solution. (The value of Kb for ethylamine (C2H5NH2) is 5.6×10−4.) Express your answer to two significant figures and include the appropriate units.
A solution contains 0.250 M ammonium chloride and 0.168 M ammonia. The pH of this solution is The compound ethylamine is a weak base like ammonia. A solution contains 0.494 M CH3NH3 and 0.132 M ethylamine, C2H5NH2. The pH of this solution is
1.) An aqueous solution contains 0.431 M ethylamine (C2H5NH2). How many mL of 0.368 M hydrobromic acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.400? 2) A buffer solution contains 0.308 M ammonium bromide and 0.319 M ammonia. If 0.0500 moles of perchloric acid are added to 225 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not...
Calculate the pH at the equivalence point for the titration of 1.0 M ethylamine, C2H5NH2, by 1.0 M perchloric acid, HClO4. (pKb for C2H5NH2 = 3.25)