A 50.0 mL of 0.0400 M EDTA was added to 20.0 mL of 0.0800 M Cu(NO3)2 at pH 5.00. The Kifor CuY- is 6.0x1018 and g4 at pH 5.00 is 3.7x107. Find the equilibrium concentration of Cu2+
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- Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the conditional formation constant for Zn at this pH?Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.02 M KMnO4 solution was used for the titration. gH * + MnO 4 + 5Fe 2+ -> SFe 3+ + Mn 2+ + 4H 20 (MM Fe = 56 a/moll mass of iron compound (g) 0.604 initial buret reading (mL) 0.94 Tinal buret reading (mL 16.21A 28.7 mL aliquot of hypochlorous acid that has a concentration of 0.516 M will be titrated with 0.345 M NaOH. Calculate the pH of the solution upon the addition of 8.14 mL of NaOH. The Ka of the acid at the temperature of the experiment is 3.34 x 10-8.
- Calculate the pSr value for 10 mL of EDTA in the titration of 50 mL of 0.02 M Sr2 + in an environment buffered at pH 11 with a titre of 0.02 M EDTA. A. 1.89B. 3.78C. 7.56D. 12.11Consider the titration of 25.0mL 0.020M of Co(NO3)2 with .0100M EDTA in a solution buffered to pH 10.00. Calculate pCo^2+ at the following volumes of added EDTA. a. 0.0 mL b. 20.0 mL c. 40.0 mL d. 49.0 mL e. 50.0 mL f. 50.1 mL g. 55.0 mL h. 60.0 mLA deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3.
- Find the pH during the titration of 20.00 mL of 0.1000 Mtri-ethylamine, (CH₃CH₂)₃N (K(b)=5.2X10⁻⁴), with 0.1000 M HCl solution after the following additions of titrant:(a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 19.00 mL(e) 19.95 mL(f ) 20.00 mL(g) 20.05 mL(h) 25.00 mLIn the titration of 50 mL 0.02 M Sr² with 0.02 M EDTA in a buffered medium at titrated pH 11, calculate the psr value for the addition of 10 mL EDTAIn order to adjust the EDTA solution, 10 mL of 0.01M Ca + 2 sample was taken and 10 mL of pH 10 buffer was added on it and it was completed to 100 mL. Then, two drops of EBT indicator were added and titrated with EDTA. Since the consumption is 13 mL, what is the concentration of EDTA solution in terms of molarity?
- Calculate the silver ion concentration in terms of pAg during the titration of 70.00 mL of 0.07000 M NaCl with 0.1000 M AgNO3 after the addition of the following volumes of reagent: (a) in the preequivalence point region at 20.00 mL, (b) at the equivalence point (25.00 mL), (c) after the equivalence point at 50.00 mL. For AgCl, Ksp = 1.82E10-10. Show your answer with three significant figures.A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. Ans in 3 sig figures. no need to write the unit.Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn at the equivalence point of the titration?