Explain the process of how to get the answer. The answer is highlighted.
Explain the process of how to get the answer. The answer is highlighted. Ch. 18 Values...
The correct answer is highlighted. I do not understand how the professor came up with this answer. Ch. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species K HF HNO2 CH3COOH HOCI HOB HOCN HCN H2SO4 Kn = 7.2 x 10-4 = 4.5 x 10-4 Ka = 1.8 x 10-5 K = 3.5 x 10-8 Ka = 2.5 x 10-9 K = 3.5 x 104 Ka = 4.0 x 10-10 Kai =...
The correct answers are highlighted. I do not understand how the answer came to be. Please explain in detail. We were unable to transcribe this imageCh. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species HF HNO2 CH3COOH НОСІ HOB HOCN HCN H2SO4 Kg = 7.2 x 104 KA = 4.5 x 10-4 K= 1.8 x 10-5 K = 3.5 10-8 Ka = 2.5 x 10-9 K = 3.5 x 104 K...
Acid Substance or Species HE HNO2 CH3COOH HOCI HOBI ka = 7.2 x 10-4 NH3 K = 4.5 x 10-4 (CH3)3N = 1.8 x 10-5 [Co(OH)]2+ Ka = 3.5 x 10-8 [Fe(OH2)2]2+ Ka = 2.5 x 10-9 [Fe(OH2)613+ Ka = 3.5 x 10-4 [Be(OH)412+ Ka = 4.0 x 10–10 [Cu(OH)212+ Ka1 = very large HBO2 Ka2 = 1.2 x 10-2 (COOH)2 HOCN HCN H2SO4 Kb = 1.8 x 10-5 Kb = 7.4 x 10-5 Ka = 5.0 x 10-10 Ka...
right answer is highlighted. what is the process of how to complete this answer? ID: A 15. Refer to Ch. 18 Values. The (OH) = 1.3 x 105 M for a 0.025 M solution of a weak base. Calculate the value of K, for this weak base. a. 5.2 x 10-5 b. 3.1 x 10-7 c. 7.7 x 10-4 d. 4.0 x 10- e. 6.8 x 10-11
correct answer is highlighted. what is the process of how to find the value of the ionization constant of the acid? this is my work so far... 12. Refer to Ch. 18 Values. The pH of a 0.10 M solution of a monoprotic acid is 2.85. What is the value of the ionization constant of the acid? a. 6.3 x 10-5 b. 3.8 x 10-6 c. 2.0 x 10-5 d. 4.0 x 10-8 e. 7.2 x 104 12. Refer to...
correct answer is highlighted in pink. how do i get the pH without it being 1.6? Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance H2CO3 Substance HCOH HNO2 НОСІ (COOH)2 Constant K = 1.8 x 10-4 Ka = 4.5 x 10-4 KA = 3.5 x 10-8 K = 7.2 x 10-4 KA = 4.0 x 10-10 Ki = very large K = 1.2 x 10-2 Ka=2.5 x 10-9 Constant Ki = 4.2 x...
please explain how you got your answer 18. Given the Ka values (in parentheses) for the following acids: HCI (Ka is very large) HNO2 (Ka = 4.0 x 10-): HF (Ka = 7.2 x 104) CH3COOH (Ks = 1.8 x 10-5) HCN (K. = 6.2 x 10-10) C6H3COOH (Ka = 6.3 x 10-5). Rank (or list) these acids in order of decreasing strength (strongest first). A. HCI > HF > HNO2 > C6H5COOH > CH3COOH > HCN B. HCI >...
please show all work for part III :) all the information needed is in the pictures III. Preparing HC,HO, Solutions and Determining pH only cal. One! theoretical pH 1.0 x 10-14 (181) concentration of HC,H,O, M measured pH ya ? 3.06 1.0 x 10-2 ka: 1. 8x10°3 ixio- 3.43 1.0 x 10-3 x = CH) -1,34% 103n 3.87 1.0 x 107 PM - 04 TH11 4.30 concentration of HC,H,O, M calculated K of HC H302 based on pH data literature...
3. Insoluble metal hydroxides can be used as a "buffer" to resist changes in pH. For example, consider the solution that would sul if 0.200 moles of MgCl2 are combined wih0.200 moles of NaOH in a total volume of 1.00 liter a) Determine the concentrations of all ionic species in this solution b) Calculate the pH of this solution c) You could add 0.040 moles of NaOH to the solution in part (a), causing additional Mg(OH)2 to precipitate. Calculate the...
If you need anymore values let me know! Thanks so much for your help! Use the References to access important values if needed for this question. How many grams of solid ammonium bromide should be added to 1.50 L of a 0.166 M ammonia solution to prepare a buffer with a pH of 8.560 ? grams ammonium bromide Use the References to access important values if needed for this question. How many grams of solid potassium cyanide should be added...