23. A 25.00 mL water sample is titrated with a 0.0120 M EDTA solution. The equivalence...
a) A 25.00-mL sample of monoprotic acid was titrated with 0.0800 M potassium hydroxide solution. The equivalence point was reached after 18.75 mL of base was added. Calculate the concentration of the acid. b) A 15.00-mL sample of 0.120 M nitric acid was titrated with 0.0800 M potassium hydroxide. Calculate the pH of the sample when 10.00 mL of the base has been added.
3. A 25.00 mL 0.0250 M calcium carbonate sample is titrated with 14.3 mM EDTA solution. Both sample and titrant are buffered at pH = 10.0 a. What is the titration reaction and what is the value of the conditional formation constant? b. What is the calcium ion concentration when 12.35 mL of titrant has been added? c. What is pCa2+ at the equivalence volume?
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...
2)a. A 15.00 ml sample of an unknown H2SO4 solution is titrated with a 0.30 M NaOH solution. The equivalence point is reached when 18.00 ml of NaOH solution is added. What is the concentration of the Unknown H2SO4 solution? (1st write balance equation)
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
thanks Question 23 (2.5 points) Saved A 25.00-ml sample of propanoic acid, CH3CH2COOH, of unknown concentration was titrated with 0.143 M KOH. The equivalence point was reached when 35.28 mL of base had been added. What is the concentration of the propanoate ion at the equivalence point? 0.143 M 0.0837 M 0.202 M 0.128 M 0.147 M نعمه
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.
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point (i.e. 50.0 mL EDTA has been added), what is the equilibrium concentration of Ca2, [Ca2], and what is the pCa? The formation constant of CaY, Kaa 5.0 x 1010, and α4 of EDTA at pH 10.0 is 0.35 4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point...
6. (8) A 50.0 mL sample of hard water containing Ca2 was titrated with 0.0500 M EDTA standard solution at pH 10 and with Eriochrome Black T indicator. The endpoint was reached when 11.35 mL of EDTA was added a) (6) Calculate the concentration of Ca* in the unknown sample in moles per liter (M). b) (2) What is the pCa of the solution?
Problem 4: EDTA titration with 16.55 ml of o.0114 M EDTA at pH-10. A 50.0 mL sample of water containing both Ca? and Mg is titrated in another 50.0 mL sample, the Mg* was precipitated as Mg(OH)2 and then, Ca2* was titrated at pH 13 with 9.25 ml of the same EDTA solution. Calculate ppm CaCo, (FW-100.09) and MgCO, (FW-84.31) in the sample. FWca: 40.08; FWm: 24.30 Problem 4: EDTA titration with 16.55 ml of o.0114 M EDTA at pH-10....