Here, [Fe3+] = [Fe2+] = 0.004 M or 4*10-3 M
pOH = 1/2 (pKb - Log[NH3]) = 1/2 (4.74 - Log5) = 2.0205
i.e. [OH-] = 10-2.0205 = 9.54*10-3 M
Now, Kc = 1/[Fe2+][OH-] = 1/(4*10-3 * 9.54*10-3) = 2.621*104
If NH3 (ammonia, pKb=4.74) is added to a solution of Fe(NO3)3 such that right after the...
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.
An analytical chemist is titrating 227.4mL of a 0.5200M solution of ammonia NH3 with a 0.5400M solution of HNO3. The pKb of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 230.7mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3solution added. Round your answer to 2 decimal places. An analytical chemist is titrating 227.4...
One drop of 2.5 M KSCN solution is added to 0.5 mL of 0.10 M Fe(NO3)3. After the solution is mixed, 1.0 mL of 0.125 M EDTA solution is added. Enter the chemical formula of the major iron complex in solution after the addition of EDTA
40. Concentrated aqueous ammonia is added to a solution of copper(II) sulfate. A white precipitate forms. The precipitate dissolves as more ammonia is added, generating an intensely blue solution. Which combination of net ionic equations, in the appropriate order, describes this chemistry?! I Cu?* (aq) + 2OH(aq) Cu(OH)2 (19) II Cu?" (aq) + 2OH(aq) = Cu(OH)2 (8) III Cu(OH)(aq) + 4 NH, (aq) Cu(NH3),?* () + 2OH(aq) IV Cu(OH)2 (8) + 4NH, (aq) Cu(NH3)*(14) + 2OH(aq) V NH3(aq) + H20...
An analytical chemist is titrating 66.8 mL of a 0.7300 M solution of ammonia (NH3) with a 0.5100 M solution of HNO3. The p K, of ammonia is 4.74 Calculate the pH of the base solution after the chemist has added 109.2 mL of the HNO2 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO2 solution added. Round your answer to 2 decimal places....
An analytical chemist is titrating 149.5 mL of a 0.8000 M solution of ammonia (NH3) with a 0.7300 M solution of HNO3. The pK, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 52.0 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH...
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of 0.02454 M ammonium chloride solution (pKb of ammonia is 4.75) 5. If you added 1 mL of 0.2550 M NaOH to 103 mL of pure water, what would the pH be?
Taking into account the dissolution-precipitation equilibrium of Fe(OH)2: Fe(OH)2 (s) ---> Fe2+ (aq) + 2OH- (aq) (a) How much Fe2+ (expressed in mg/dm3) may be present in a water containing 0.001 M of NaOH without occurring precipitation of Fe(OH)2 ? (b) Determine the maximum amount of Fe2+ in solution (expressed in mg/dm3) by lowering the pH value of water by two units (possible by the addition of a strong acid). Kps (Fe(OH)2)= 2.0 x 10^-15 M^3
When ammonia is added to Zn(NO3)2 solution, a white precipitate forms, which dissolves on the addition of excess ammonia; but when ammonia is added to a mixture of Zn(NO3)2 and NH4NO3 no precipitate forms at any time. Suggest an explanation for this difference in behavior.
In step1, aqueous ammonia is added to a solution of the three ions. The equilibrium for the ammonia is EQ1: NH3(aq + H2O(l) ßà NH4+(aq) Kb=1.8x10-5 The bismuth(III) ion is precipitated out of the solution as Bi(OH)3. The equilibrium involved is related to the one provided below: EQ2: Bi(OH)3(s) ßà Bi3+(aq) +3OH(aq)- Ksp =3.2x10-40 Manipulate EQ 1 and 2 to solve for the net equation, EQ3: EQ3 (net): 3H2O+ Bi3+(aq) +3NH3(aq) ßàBi(OH)-(s) +3NH4+(aq) Write the mass law expression for the...