Given Kb=6.4x10-4 for C2H5NH2 (ethylamine), what is the pH value for 0.1 M C2H5NH3Br?
Given Kb=6.4x10-4 for C2H5NH2 (ethylamine), what is the pH value for 0.1 M C2H5NH3Br?
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.
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.)
1. A 23.6 mL sample of 0.391 M ethylamine, C2H5NH2, is titrated with 0.315 M nitric acid. At the equivalence point, the pH is . Ethylamine Kb = 4.3X10-4 Nitrous acid Ka1 = 4.5x10-4 2. A 29.1 mL sample of 0.336 M ethylamine, C2H5NH2, is titrated with 0.276 M hydrochloric acid. After adding 52.4 mL of hydrochloric acid, the pH is . hydrochloric acid Ka1 = 3.5x10-8 Ethylamine Kb = 4.3X10-4
250 mL of 0.200 M aqueous ethylamine (C2H5NH2(aq), Kb = 5.6 × 10–4) is titrated with 0.200 M HCl(aq). Which of the following indicators would be most appropriate for detecting the equivalence point of the above titration? The range of pH values for which each indicator undergoes a color change is given in parentheses. A. Crystal Violet (pH 0-1.8) B. 2,4-Dinitrophenol (pH 2.5-4.0) C. Eriochrome Black T (pH 5.0-6.5) D. m-Nitrophenol (pH 6.8-8.5) E. Alizarin yellow (pH 10.0-12.0)
6.) Determine the pH during the titration of 34.9 mL of 0.220 M ethylamine (C2H5NH2, Kb = 4.3×10-4) by 0.220 M HNO3 at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HNO3 (b) After the addition of 12.7 mL of HNO3 (c) At the titration midpoint (d) At the equivalence point (e) After adding 52.0 mL of HNO3
The following mixture represents a buffered solution (a buffer): 0.30 M ethylamine (C2H5NH2) + 0.15 M ethylammonium bromi de (C2H5NH3Br) True False QUESTION 9 The following mixture represents a buffered solution (a buffer): 0.20 M hydrochloric acid + 0.13 M potassium chloride True False QUESTION 10 A buffer solution is made that is 0.25 M in HNO2 and 0.75 M in NaNO2. If Ka for HNO2 is 4.5E-4, what is the pH of the buffer solution?
1.Determine the pH during the titration of 36.6 mL of 0.304 M ethylamine (C2H5NH2 , Kb = 4.3×10-4) by 0.304 M HI at the following points. (a) Before the addition of any HI (b) After the addition of 16.1 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 51.2 mL of HI b.Determine the pH during the titration of 61.4 mL of 0.450 M nitrous acid (Ka = 4.5×10-4) by 0.450 M NaOH...
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)
2. A 35.00-ml sample of a 0.0870 M solution of ethylamine, C2H5NH2 (Kb = 5.6 x 10), is titrated with 0.150 M HCI. (a) What is the equivalence volume of HCI? (b) Calculate the pH of the solution: (1) prior to the start of the titration. (ii) after addition of 10.15 mL of the 0.150 M HCI. (iii) after addition of 14.50 mL of the 0.150 M HCI. (iv) after addition of 6.00 mL of the HCl beyond the equivalence...
A solution contains 0.159 M C2H5NH3 and 0.177 M ethylamine, C2H5NH2. The pH of this solution is .