Problem: A solution containing 50.0 mL of 0.100 M EDTA buffered to pH 10.00 was titrated...
a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M HCl. kb for CN is 2.0x10-5. A.calculate the pH of the solution prior to the start of the titration. B after the addition of 10.0 mL. C. after the addition of 25.0 mL of 0.100 M HCl. D. at the equivalence point. E. after the addition of 60.0 mL of 0.100 M HCl
A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was titrated with 0.0400 M EDTA. Answer the following questions and enter your results with numerical value only. Calculate the equivalence volume, Ve, in milliliters. Calculate the concentration (M) of free metal ion at V = 1/2 Ve. If the formation constant (Kf) is 1012.00. Calculate the value of the conditional formation constant Kf’ (=αY4- * Kf) and enter your result as scientific notation form....
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....
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...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO s titrated with 0.100 M Ce4+ resulting in the formation of Fe3+ and Ce3+. A Pt indicator electrode and a saturated calomel electrode are used to monitor the titration. Write the balanced titration reaction titration reaction:> Complete the two half-reactions that occur at the Pt indicator electrode. Write the half-reactions as reductions half-reaction: Ce e half-reaction: Fe e- E 0.767 V Select the two equations that can be...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO, is titrated with 0.100 M Ce*+ resulting in the formation of Fe+ and Ce3+. APt indicator electrode and a saturated calomel electrode are used to monitor the titration Write the balanced titration reaction. titration reaction:-> Complete the two half reactions that occur at the Pt indicatorelecrode Write the half-reactions as reductions half-reaction: Ice + e-→ We were unable to transcribe this imageсез+] . 0.241 (Ce+] 「 0.241 E...
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M Ce4+ to give Fe3+ and Ce3+ using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. > (b) Complete the two half reactions for the Pt electrode. Ce té E° = 1.70 V Fe +e = E° = 0.767 V [Fe2+11 1 - 0.241 E= 0.767 – 0.05916) (c) From the list in the column at the right, select...
(10 marks) Calculate the pH after titrating 50.0 mL of a 0.100 M weak base solution (Kb = 7 x10-9) with: 0.200 M HBr to the equivalence point b. 50.0 mL of 0.200 M HBr
7. Calculate the pH of the solution obtained by titrating 50.0 mL of 0.100 M HNO2(aq) with 0.150 M NaOH(aq) to the equivalence point. Take Ka = 5.6 x 10 - M for HNO2(aq).
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...