For all metal ion - EDTA complxes, what is the relationship between the conditional formation constant Kf' and the normal formation constant, Kf ? -The conditional formation constant is always less than or equal to Kf at all pHs.. -The conditional formation constant is usually less than Kf, but can sometimes be greater than Kf for some metal ions at high pHs. -The conditional formation constant is always less than Kf at all pHs.. -There are no restrictions. Depending on the metal ion and the pH, the conditional formation constant can be less than, equal to, or greater than Kf.

A 0.150 mol quantity of CoCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Co²+ ions at equilibrium? Assume the formation constant* of Co(NH,+ is 5.0 × 1031M-6. concentration:

Write the balanced chemical equation associated with the formation constant, Kf, for each complex ion. Include phase symbols. Ag(CN), : Ag2+ (aq) + 2CN (aq) Ag(CN), (aq) Incorrect BeF : Ве Incorrect Incorrect 1L 1L

Zn²+ and Mn²+ (starting concentration 102 mol/L) should be separated by fractionated precipitation using H₂S. Does a pH or pH range exist allowing to completely precipitate one metal (i.e. the remaining concentration of the precipitated ion has to be 105 mol/L or less) whereas the other stays in solution at its initial concentration? Please calculate this pH range!

A chemist wishes to prepare a standard aqueous solution that has a concentration of Fe3+ equal to 1.0x10-5 M. This solution is to be prepared by allowing water at a set pH to reach equilibrium with solid Fe(OH)3. Given the fact that pH = -log [H+], what pH should be used for the aqueous solution to give this desired concentration of [Fe3+].

Use the References to access important values if needed for this question. A buffer solution is 0.386 M in KHSO3 and 0.338 M in K2 SO3. If K, for HSO3- is 6.4 x 10-8, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining

A 50.00 mL of 0.0275 M HCl solution was titrated with 0.1500 M NaOH. Calculate the pH of the analyte solution in the specified volumes of the titrant added. At 5 mL of the titrant.   -1.26 -1.56 -1.86 -2.06 At 14 mL of the titrant. -10.23 -11.78 -12.23 -13.78 At 20 mL of the titrant. -10.23 -11.78 -12.23 -13.78

18a

Please provide detailed solution and give the explanation of the concept.....   A 1.42 L buffer solution consists of 0.176 M butanoic acid and 0.280 M sodium butanoate. Calculate the pH of the solution following the addition of 0.077 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5. Note: The buffer solution consists of the weak acid butanoic acid, C3H7COOH, and its conjugate base butanoate, C3H7COO–. The added NaOH, a strong base, will react with a stoichiometrically equivalent amount of butanoic acid to produce butanoate. Start by determining the initial amount, in moles, of butanoic acid and butanoate in the buffer solution before the addition of NaOH.

A 10.0 ml. solution of 0.300 M NH, is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCI solution: 0.00 ml., 10.0 ml., 30.0 ml., and 40.0 ml.. Round your answer to 3 decimal places. Note: Reference the K, of acids at 25 °C and K, of bases at 25 °C tables for additional information. Part 1 of 4 0.00 ml. Added, pH= Part 2 of 4 10.0 mL Added, pH = 0.. 0.8