Answered: To prepare 100 mL of TE buffer (10mM…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.21QAP

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A 100-mL sample of hard water is titrated with the EDTA solution in Problem 2. The same amount of Mg2 is added as previously, and the volume of EDTA required is 31.84 mL. a. What volume of EDTA is used in titrating the Ca2 in the hard water? _____________mL b. How many moles of EDTA are there in that volume? _____________ moles c. How many moles of Ca2 are there in the 100 mL of water? _____________ moles d. If the Ca2 comes from CaCO3, how many moles of CaCO3 are there in one liter of the water? How many grams of CaCO3 are present per liter of the water? _____________ mol / L _____________ g / L e. If 1 ppm CaCO3 = 1 mg per liter, what is the water hardness in ppm CaCO3? _____________ ppm CaCO3
bn the lab vou titrated 40 ml of 0.006 M Ca with 0.008 M EDTA at pH 10. What was the pCa in that titration at the following points r4 B 16. After adding 1I5 ml of titrant, the pCa is (a) 2.35 (b) 2.66 (c) 2.92 (d) 3.22 C17. At equivalence point, the pCa is (a) 6.36 (b) 6.81 (c) 7.45 (d) 7.98 C18. Alter adding 45 ml of titrant, the pCa is (a) 8.75 (b) 9.32 (c) 9.95 (d) 10.37
li. 9:-7 Describe the preparation of 2000 mL of 0.108 M barium chloride from solid BaC12.2H2O if you know the molecular * ? weight of barium chloride (244.3 g/mol) 52.769 gm 0.0527 mg 52.769 mL The best controlled in complexometric titrations between metal – ligand is a-Temperature degree b- Concentration of ion c- pH How many moles of solute are present in * ?125 mL of 0.20M NaHCO3 0.125 mol O 0.0025 mol O 0.025 moL II
5.) A 4.59mL sample of HCl (sp. gr. = 1.3) required 5.5mL of 0.9544N NaOH in titration. Calculate the %w/w of HCl in the sample.
B? The concentrations of acid and base in buffer B are twice the concentrations of buffer A (buffer B is twice as strong as buffer A). Show that the ratio of the volume of titrant required to raise the pH of each buffer 1 unit (VB/VA) is directly related to the ratio of the buffer strengths (strengthe/strengthA) be Buffer capuaty (defined ar Me auoler of naud ar Hhe nuolet ofaud or have needed to change the uubon hu 1 unuf / hy the pH change and voturme huffer ucd in hbres of
50mL of 0.025 M HF is titrated with 0.045 M NaOH. a) What amount of NaOH is required for equivalency point? b) What is the pH of the solution at this point? Note that Ka of HF is 6.6x10-4
Please provide only typed answer solution no handwritten solution needed allowed
G.268.
The solutbility constant for Ce(IO3)3 is 3.2x10^-10. What is the Ce3+ concentration in a solution prepared by mixing 50 mL of 0.0450 M Ce3+ with 50 mL of: A.) 0.0450 M IO3- ? B.) 0.0500 M IO3- ?
Pls solve this question correctly in 5 min i will give u like for sure You have the following chemicals available: NaH2PO4 (s), Na2HPO42H2O (s), Na3PO4 (s), 6.00 M HCl, and 6.00 M NaOH. Describe two different ways to prepare 500.0 mL of a pH 7.40 buffer where the base concentration if 0.100 M.
2. 25.00 mL of 0.05600 M Fe" is made up in a solution that is buffered at pH 7.50. Oxalate is added as an auxiliary complexing agent to keep Fe(OH), from precipitating. The oxalate ion is adjusted so that it's free concentration is 0.250 M. The solution is titrated with a 0.02414 M solution of EDTA. How many mL of EDTA solution are required to reach the equivalence point in the titration? а. Ve = 25,007 0,0 S600 58.00 mL 0,02414 b. Calculate a at this pH. Calculate a for the solution. с. d. Calculate the conditional formation constant, K,. CS Scanned with CamScanner
You need to prepare 2L of concentrated TBE buffer. How much Tris do you need for an a) 5x,b) 10x, c) 2x TBE stock s-n? (working concentration of Tris in 1xTBE is 10.8g/L)

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To prepare 100 mL of TE buffer (10mM Tris and 1mM EDTA) What volumes of the above Tris (1M) and EDTA (0.2M) solutions should be used?