6. Water sample was titrated with EDTA after pH adjustment using Eriochrome black T indicator. Knowing that the concentration of EDTA is 0.050 M and density of water sample equals to 1.10 g/mL. (CaCO,= 100.09 amu).The following results was obtained trials volume of water sample (mL) volume of EDTA (mL) 250.0 250.0 250.0 250.0 10.05 7.00 10.50 10.10 Calculate he total hardness of water as CaCO, and accordingly classify this water. The following results was obtained 1Nm 4

6. Water sample was titrated with EDTA after pH adjustment using Eriochrome black T indicator. Knowing that the concentration of EDTA is 0.050 M and density of water sample equals to 1.10 g/mL. (CaCO,= 100.09 amu).The following results was obtained trials volume of water sample (mL) volume of EDTA (mL) 250.0 250.0 250.0 250.0 10.05 7.00 10.50 10.10 Calculate he total hardness of water as CaCO, and accordingly classify this water. The following results was obtained 1Nm 4

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.54QE

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In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 2: Methyl red: pH transition = 4.8-6.0 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 4: Thymolthalein: pH transition = 8.5-10.5 O Indicator 5: Indigo Carmine: pH transition= 11.6- 14.0 O Indicator 3: Cresol red: pH transition = 7.2-8.8
In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 4: Thymolthalein: pH transition = 8.5-10.5 OIndicator 5: Indigo Carmine: pH transition= 11.6- 14.0 Indicator 3: Cresol red: pH transition 7.2-8.8 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 2: Methyl red: pH transition = 4.8-6.0
n 0 The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic acid with a 0.10 M solution of a strong monoprotic base. Data points at 1 mL increments. 14.0 12.0 10.0 Hd 8.0 6.0 4.0 2.0 0.0 0.0 10.0 20.0 ession# 188... 30.0 Volume of titrant (mL) 40.0 50.0
20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 HO 8.0 6.0 4.0 2.0 0.0 0.0 10.0 20.0 30.0 Volume of titrant (mL) 40.0 444444 50.0 (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999.
Answer if true or false , if false, put the correct answer 1. There is 11.34 mmol in 0.2011 of 0.5604 M HgCl2 2. The x axis of sigmoidal titration curve is p function of the analyte or titrant 3.The concentration of the secondary standard is relative to a primary standard 4. There is 110 mmol in 79.8 mL of 0.1379 M NH4VO3 (116.98 g/mol)
The end point of a titration was reached after 22.2 mL22.2 mL of 0.050 M0.050 M disodium EDTA titrant was dispensed into a solution containing the zinc ion. Calculate the moles of disodium EDTA used. moles of disodium EDTA: = mol
Solution A: 1.7 x 10-5 M HCI Solution B: 3.40 8 of CH3C0ONa.3H20 in 250 mL of 0.1 M CH3COOH (Buffer solution) 0.IM NaOH and methyl red indicator pH solution steps obseration Solution A Addition of a few drops the colour changes from clear to pink 4.68 of methylred (HCL) Addition of 10 drops of The colour change from clear to pink 4.73 0.1 M NAOH Soluion B Addition of a few drops The colour change from pink to clear of methyl red (buffer solution) Addition of 10 drops of The colour stays the same 4.73 0.1 M NaOH a) Calculate the pH of a buffer system made up of 0.25 M C6H5C0OH and 0.35 M C6H5COONa. b)What is the pH after the addition of 20 mL of 0.I M HCI to 500 ml of the above buffer solution? c)Describe how you would prepare a IL solution of 0.1 M sodium acetate (CH3CO0Na)/0.I M acetic acid (CH3C0OH) buffer system with a pH of about 5.
Chemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.
A water was tested for water hardness. A 50.00 mL aliquot was prepared and buffered to pH 10.0, it required 23.55 mL of 0.0250 MEDTA. A second aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA titrant. Calculate the total hardness of the water (expressed in ppm CaCO). a. 727.2 ppm b. 1179 ppm c. Insufficient data d. 380.2 ppm Calculate the calcium hardness of the water (expressed in ppm CaCQ:). a. Insufficient data b. 1179 ppm c. 727.2 ppm d. 380.2 ppm Calculate the magnesium hardness of the water (expressed in ppm MECO:) a. 727.2 ppm b. Insufficient data c. 380.2 ppm d. 1179 ppm
A Consider the pH titration curve above (pH vs volume in ml). The pk, of the weak base being titrated and the pH of the equivalence point are, respectively: 12 11 10 8 7 5 4 2 1 10 20 30 40 O 2.5 and 4.0 • 5.4 and 4.5 O 11.2 and 5.4 O 11.2 and 4.5 O 4.5 and 5.4 Based on the indicator information above, which of the following indicators could be used successfuly in the titration in Part A? (Select all correct responses. Indicator Colour (low pH – high pH) pK, methyl yellow red-yellow 3.1 methyl orange red-yellow 3.7 bromophenol blue yellow-blue 4.2 bromocresol green yellow-blue 4.7 methyl red pink-yellow 5.1 bromocresol purple bromothymol blue yellow-purple 6.3 yellow-blue 7.0 phenol red yellow-red 7.9 O phenol red cresol red yellow-red 8.3 O bromocresol purple thymol blue yellow-blue 8.9 O methyl yellow thymolphthalein colourless-blue 9.2 O bromothymol blue O thymol blue O thymolphthalein Part C Baseu on the table above, what colour is methyl orange at pH3? Submit Request Answer Part…
25.00 mL of a weak monoprotic acid is titrated with a 2.00 M solution of NaOH. The following data is collected mL NaOH added PH 5.55 half-way point 2.50 equivalence point 5.00 saved Use the pH at the half-way point point to estimate the pK, of the acid. 00000 5.55 6.43 05.12 8.76 6.01 O 5.92
Consider the titration of 100.0 mL of 0.100 M hydrazine (H2NNH2, K, = 3.0×10-6) by 0.200 M HNO3. Despite the symmetric nature of the hydrazine's molecular structure, it accepts only a single proton from HNO3 in aqueous solution. (Kw = 1.00×10-14) %3D %3D (a) Calculate the pH of the solution after addition of 0.0, 20.0, 25.0, 40.0, 50.0, and 100.0 mL of HNO3 to the solution. (Note: you need to consider the range of applicability of the Henderson- Hasselbalch equation and need to check if water autoionization can be neglected. See Figure 15.18 in the textbook.) (b) Based on your answer to part (a), sketch the titration curve, marking the calculated points and labeling the equivalence and half-equivalence points. (c) Although still weak, ammonia (NH3, Kb = 1.8×10-5) is a stronger base than hydrazine. Sketch the titration curve for 100.0 mL of 0.100 M ammonia by 0.200 M HNO3 on the same axes as your answer to part (b); be sure to label the curve. %3D Note: a qualitative sketch is…