If you start with 0.30 M mn2+ at what pH will the free Mn2+ concentration be...
In this example, we are going to focus on the chelation of free Mn2+ ions in a solution at pH = 7. (a) If there are 20.0 L of 0.00025 M Mn2+ in the solution before the addition of EDTA, how much EDTA is needed to complex all of the Mn2+ in moles? (b) You have a 0.050 M solution of EDTA, how many Liters of the solution is needed to reach the equivalence point for the solution of Mn2+...
A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at 0.010 M, was saturated with H2S(g) at room temperature. Assume that the pH of the solution remains constant and that the [H2S]sat = 0.10 M. The Ksp for MnS9S) is 2.5 x 10-13 , Ksp for CdS(s) is 8.0 x 10 -27 and Ksp for FeS(s) is 6.3 x10-18 . For H2S:Ka1=1.3 x 10-7. Ka2=8.5 x 10-14. Calculate the equilibrium concentrations of Mn2+(aq),Cd2+(aq), and...
QUESTION 21 What is the pH of a solution with a hydronium (H30+) concentration of 4.6 x 10-5 M. QUESTION 22 What is the hydronium (H30) concentration of a solution with a pH of 2.09?
READING pH from Diagrams If you have an oxalic acid concentration of 10-2 M, what is the pH of the system? If you have a sodium oxalate system of 10-2 M, what is the pH of the system? 7. 1.0E-01 1.0E-03 2 1.0E-05 1.0E-07 1.0E-09 1.0E-11 ?? OH -HA- HAA-2 H2A 2 3 4 5 6 7 8 9 10 11 12 13 14 pH
Suppose you have a solution that is 0.044 M in Mn2+and 0.31 M in Cr3+. What range of pH values will allow you to separate these ions? In other words, for what range of pH values will one of the hydroxides precipitate but not the other?
please explain how you got all your answers 10. Calculate the pH of a 0.30 M formic acid solution. (K-1.8 x 10") Weak monoprotic acid. 11. Calculate the K, for a 0.050 M solution of HA (weak acid) if the pH = 4.65. 12. What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25C? (K. of F = 1.4 x 10) 13. Which of...
Find the conditional formation constant for (MgEDTA)^2- at pH 9.00. Then find the concentration of free Mg^2+ in 0.050 M Na2[Mg(EDTA)] at pH 9.00. Please show all the steps because I don't know how to start it. If you do, I'll give it a thumbs up! Thank you!
What is the pH of a solution with a fluoride concentration of 0.16 M ? The Kb for F– is 1.47×10-11 .
QUESTION 21 What is the pH of a solution with a hydronium (H30+) concentration of 4.6 x 10-5 M.
QUESTION 21 What is the pH of a solution with a hydronium (H30+) concentration of 4.6 x 10-5 M.