- 2.80 Ethylamine, C2H5NH2, is a monoprotic base with pKb = 3.37 at 25 °C. For...
1) Ammonia, NH3, is a monoprotic base with pKb = 4.74 at 25 °C. For 0.121 mol L−1 NH3(aq) at 25 °C, calculate (a) the percent ionization of NH3; and (b) the pH of the solution. 2) Hydrazoic acid, HN3, is a monoprotic acid with pKa = 4.72 at 25 °C. For 0.121 mol L−1 HN3(aq) at 25 °C, calculate (a) the percent ionization of HN3; and (b) the pH of the solution.
Calculate the Ka (aq., 25 °C) of a 0.250 M weak acid whose pH is 3.86. The base-ionization constant of ethylamine (C2H5NH2) is 6.4 x 10-4 at 25.0 °C. The [H+) in a 1.6 x 10-2 M solution of ethylamine is M.
Part A) Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 205 mg/L. Express your answer to two decimal places. Part B) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.20. Express your answer to two decimal places. B2) Find the percent dissociation of this solution. Express your answer using two significant figures.
Hydroselenic acid, H2Se, is a diprotic acid with pKa,1 = 3.89 and pKa,2 = 11.01 at 25 °C. For 0.147 mol L−1 H2Se(aq) at 25 °C, calculate: (a) the fraction, α1, of H2Se that exists in the singly-ionized form, HSe− α1 = (Enter a number between 0 and 1, accurate to 2 significant figures.) (b) the equilibrium concentration of the doubly-ionized form, Se2− [Se2− ]eq = mol L−1 (Enter a number accurate to 2 significant figures.) (c)...
The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 ⋅ 10−4 at 25.0 °C. The [H+] in a 1.1 ⋅ 10-2 M solution of ethylamine is ________ M. a)2.7 ⋅ 10−3 b)3.8 ⋅ 10−12 c)11.37 d)4.3 ⋅ 10−12 e) 2.4 ⋅ 10−3
8) The base-ionization constant of ethylamine (C2H-NH2) is 6.4 x 10-4 at 25.0 °C. The [H*] in a 1.6 x 10-2 M solution of ethylamine is M. 9) Z is a weak base. An 0.350 M aqueous solution of NaZ is prepared. The pH of the solution was 8.93 at 25.0°C. The Ky of Z" is: 10) At 25 C, the pH of a 0.15 M aqueous solution of Csz (the cesium salt of HZ) is 10.70. What is the...
Question 6: (1 point) Selenous acid, H2SO3, is a diprotic acid with pKa,1 = 2.64 and pKa,2 = 8.26 at 25 °C. For 0.169 mol L-1 H2SeO3(aq) at 25 °C, calculate: (a) the fraction, at, of H2SeO3 that exists in the singly-ionized form, HSEO3- ay = (Enter a number between 0 and 1, accurate to 2 significant figures.) (b) the equilibrium concentration of the doubly-ionized form, Se032- [SeO32-leq = _ (Enter a number accurate to 2 significant figures.) mol L-1...
Calculate pH of a weak acid/conjugate base buffer solution. 1. a) Calculate the pH of 650. mL of a 0.211-M solution of acetic acid before and after the addition of 0.123 mol of potassium acetate. pH befor addition = pH after addition = 1 b) Calculate pH of a weak base/conjugate acid buffer solution. A 0.190-M aqueous solution of C2H5NH2 (ethylamine) has a pH of 11.9. Calculate the pH of a buffer solution that is 0.190 M in C2H5NH2 and...
Oxycodone (C18H21NO4), a narcotic analgesic, is a weak base with pKb=5.47. Part A Calculate the pH in a 0.00280 M oxycodone solution. Express your answer using three significant figures. Part B Calculate the concentrations of C18H21NO4 in a 0.00280 M oxycodone solution. Express your answer to two significant figures and include the appropriate units. Part C Calculate the concentrations of HC18H21NO+4 in a 0.00280 M oxycodone solution. Express your answer to two significant figures and include the appropriate units. Part...
Part A.) Consider that you are titrating a diprotic weak base "B" which has pKb1=4 and pKb2=8. The product of the first ionization of B is BH+ and the product of the second ionization is BH22+. A 0.00500-mol sample of the base is dissolved in enough water to produce 100.0 mL of solution and is titrated with 0.500 M HCl. What is the exact pH when 7.2 mL of HCl is added? Enter your answer to three significant figures. Part...