7. (5 pts) Determine the pOH of a 0.227 M solution of the WB pyridine, CsHsN;...
28) (8 pts) Calculate the pH of a 0.68 M NH&Br (aq) aqueous solution at 25 C. Kb (NH3) 1.8x105
9. Determine the (OH), pH, and pOH of a 0.15 M ammonia solution 10. Determine if each solute will form a solution that is acidic, basic, or pH-neutral. a. FeCl3 b. NaF C. CaBr2 d. NH4Br e. C6H5NH3NO2 Chapter 15
For the lonization of ammonia shown below, the mixture initially contains 0.500 M NH, (aq). Determine the equilibrium millimolar (mm) concentration of HO- if K. - 1.74 x 10-5. NH3 (aq) + H2O (liq) + NH4+ (aq) + OH- (aq) QUESTION 18 Calculate the concentration of sulfate (SO2-) in a 0.0500 M solution of Nasso, If K = 0.012 for the following reaction: HSO4- (aq) + H20 (lia) = H2O* (aq) + SO42- (aq)
Please help with 16 and 17
16. (10 pts) The pKb of NH, is 1.76×10-5. a) Determine the pH of a solution of 0.200 M NHs(aq) b) Calculate the pK, for NH.CI. c) Determine the pH of a solution of 0.200 M NH.C(aą). d) Determine the pH of a buffer solution made from 500.0 mL each of 0.200 M NH, and 0.200 M NH4CI 17. (pts) Determine the pH of a buffer made from 65.0 mL of 0.15 M HCHO,...
please explain how you got these answers!!
and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(I), [Cu(NH). If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.074 V at 298 K Constants Periodic Table Use the standard reduction potentials shown here to answer the questions Reduction half-reaction E (V) Cu2+ (aq) 2e Cu(s) 0.337 2H + (aq) + 2e →H, (g) | 0.000 ▼ Part A...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
Question 5 6 pts A student has three test tubes containing a metal (M) nitrate solution M(NO3)2 (aq) (where "M" represents a generic transition metal). The student adds aqueous ammonia (NH3) to one test tube, aqueous hydrochloric acid (HCI) to the second tube, and nothing more to the third tube, but forgets to label the tubes. After this, one test tube contains a red solution, one an orange solution, and one a yellow solution. Note: This metal, M, would follow...
1. Determine the Ka value for an acid that is 0.294 M in a solution that has a pH of 2.80. A 49 x 10-14 B. 23 x 109 C. 14 x 10-5 D. 20 x 10-5 OE 3.7x 10-7 2. When titrating 25.0 mL of 0.080 M HCIO with 0.060 M NaOH, calibrate the pH after adding 25.0 mL of 0.050 M NaOH (pKa = 7.55) A. 7.43 b.7.55 C.7.77 D.10.08 E 1248 3. The correct expression for the...
20) Determine the pH of a 0.188 M NH3 solution at 25°C. The K of NH3 is 1.76 x 10-5. 20) B) 12.656 A) 5.480 C) 8.520 D) 11.260 E) 2.740