Find the pH of the solution obtained When 32 mL of o.oB7 M. Ethylamine (C, H, NH₂) is titrated ul 10 mL of o. is...
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
5a) 5a) Calculate the pH when 30.00 mL of 1.300 x 10'M NH. NH3(aq) is titrated is titrated with 30.00 mL of 1.000 x 10-'M HCI. (3 points) 5b) What is the best buffer pH for this titration? (1 point)
A 20.0 mL sample of 0.150 M ethylamine is titrated with 0.0878 M HCl. Part A What is the pH after the addition of 5.0 mL of HCl? For ethylamine, pKb = 3.25. 0 11.52 O 9.98 04.02 O 10.75 Submit Request Answer
A chemist titrates 140.0 ml of a 0.8665 Methylamine (C,H,NH,) solution with 0.5484 M HBr solution at 25 °C. Calculate the pH at equivalence. The pky of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added.
Be sure to answer all parts A 10.0-mL solution of 0.390 M NH, is titrated with a 0.130 M HCl solution. Calculate the pH after the following additions of the HCl solution: (a) 0.00 mL (b) 10.0 mL (c) 30.0 mL (d) 40.0 mL
4-l0.2 Solution 8 10.0 mL of solution 5 + find the limiting reager Calculated pH h Measure 4 (hint-calculate the number of moles o and log On 0006 200 fo.0000 C000s +0000 Should the pH of a buffer change when large quantity of base is added?e Why? Butter is o imitins feasant. ph Should to The Cicnse tue cecid MaRe tue 4. Calculate the pH of the following solutions. Compare these values with the experimental values obtained for Solutions 9...
A 26.6 mL sample of 0.363 M ethylamine, C2H5NH2, is titrated with 0.247 M hydrochloric acid. After adding 17.6 mL of hydrochloric acid, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Retry Entire Group 4 more group attempts remaining
A 25.0 mL sample of 0.203 M ethylamine, C2H^NH2, is titrated with 0.225 M nitric acid. Before the addition of any nitric acid, the pH is (2) After adding 8.62 mL of nitric acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 35.4 mL of nitric acid, the pH is Use the Tables link on the toolbar for any equilibrium constants that are required. Not submitted...
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)