1. A solution was prepared with an Ni(EDTA)2- concentration of 0.0150M.
a) Calculate the concentration of Ni2+ in this solution if it was buffered to a pH of 3.0
b) Calculate the concentration of Ni2+ in this solution if it was buffered to a pH of 8.0
1. A solution was prepared with an Ni(EDTA)2- concentration of 0.0150M. a) Calculate the concentration of...
Calculate the conditional formation constant of the EDTA complex of Al3+ in a solution buffered to pH = 3.0 Answer to 3 significant digits.
Calculate the molar Y^4- concentration in a 0.0350 M EDTA solution buffered to pH of 11.00. At pH 11.00 alpha_4 is 0.85. 2.98 times 10^-2 7.23 times 10^-3 3. 10^-3 3.41 times 10^-8 4.27 times 10^-4
23.
A solution is prepared by adding 0.10 mole of Ni(NH3). Cl2 to 0.50 L of 3.2 M NH3. Calculate (Ni (NH3)&2+) and (Ni2+in this solution. Koveralt for Ni (NH3)22+ is 5.5 x 108. That is, 5.5 x 108 = Ni (NH3) 2+1 [Ni2+] [NH3] for the overall reaction Ni2+ (aq) + 6NH3(aq) = Ni (NH3). 2+ (aq) (Ni (NH3), 2+] = 0 [Ni2+] = C M
What is the maximum concentration of Ni2+ in a solution of pH 10.00? Ksp (NI(OH)2) = 2.0*10-15 M
Complex-Formation Titrations +2 10. Calculate the Ca concentration and pCa logCa D of a solution that results from the mixing of each of the following solutions (buffered at a pH of 10.0): +2 +2 +2 EDTA +10 The complexation reaction: Ca CaEDTA atapH of 10.0, has an Kefr r 5.0 s 10 +2 +10 Kerr-lCaEDTAI/(1 Ca.-11 EDTA I) = 5.0 x 10 a) Calculate the pCa of a solution of 50.0 ml of 0.0102 MCa with 50.0 ml of 0.0100...
22. What will be the concentration of Ni in a solution that is made at 25°C and a high pH by adding 1.0 mL of 0.250 M Ni(NO3)2 to 100 mL of 0.058 M ammonia? You can assume that all of the Ni(NO3)2 originally dissolves to pro- duce Ni2+ and NO3 and that the value of [NH3] at equilib- rium is approximately equal to the analytical concentration of ammonia.
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was used to titrate 25 ml. of the sample solution with the presence of an ammonium buffer (pH 10). If 15.80 ml. of the standard EDTA was used to reach the end point, calculate the molar concentration and the ppm concentration of the unknown Ca^2+ (atomic weight of Ca = 40.08g/mole) solution The amount of 0.2915g of benzoic acid was dissolved in 100 ml. of...
equilibrium Calculate the concentration of Ni2+ in a solution with a formal Niy2-concentration of 0.015 M at pH = 3.0. NiY2-: logK; = 18.4; Aya- = 2.1x10-11
EDTA concentrations for each titration
Fine 2 Part A: Standardization of EDTA Concentration of CaCl, solution ().01 m Rough Fine 1 Volume of CaCl, Initial Volume EDTA 0.72 22.69 Final Volume EDTA 12.51 32,13 Volume EDTA added 11.79 quy Calculate EDTA concentration. Show the calculations for your fine titrations. 32.13. 4.51 9.38 Calculation: Calculation: Average concentration EDTA using fine titrations, Average volume of EDTA added using fine titrations1.4
An unknown solution was analyzed for Ni by an EDTA titration. A 50.00 mL sample of the unknown was treated with 25.00 mL of 0.2404 M EDTA. The excess EDTA was then back titrated with 8.52 mL of 0.0694 M Zn2+ to reach the equivalence point. What was the concentration of Ni (in unit of M) in the 50.00 mL sample? Please keep your answer to three decimal places.