1. Calcium ion was titrated with EDTA at pH 11, using calmagite as indicator. Which is...
1. Calcium ion was titrated with EDTA at pH 11, using calmagite as indicator. Which is the principal species of calmagite at pH 11? What color was observed before the equivalence point? After the equivalence point?
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1. Calcium ion was titrated with EDTA at pH 11, using calmagite
as indicator. Which is...
The calmagite indicator changes from a pink to a blue color during the titration. Describe why...
The calmagite indicator changes from a pink to a blue color during the titration. Describe why the color change occurs. This question is part of the experiment "determination of water hardness", and you should answer the question based on the following background information(abstract information and you can get the answer). In this titration Calmagite is used an indicator for both calcium and magnesium. The equation below shows the competition reaction between the calmagite indicator (In) and EDTA for Mg and...
1. What is the amount in grams of EDTA you will need to measure out to...
1. What is the amount in grams of EDTA you will need to measure out to prepare a 250 mL 0.01 M EDTA solution ? The molar mass of EDTA is 374.27 g/mol. 2. Titration Data from three water samples Water Volume of 0.01 Water Drops of MEDTA Moles Ca2+ sample indicator used to of concentration volume Calmagite reach Ca2+ in water (M) end point source 50 mL4 2 ml USFISA drinking water fountain USF BSF drinking water fountain 50...
3. A 25.00 mL 0.0250 M calcium carbonate sample is titrated with 14.3 mM EDTA solution....
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?
1a) If a titration was preformed in which an acid of pH 6 was being titrated....
1a) If a titration was preformed in which an acid of pH 6 was being titrated. The equivalence point of the titration was near pH 8. What indicators should be added to the acid solution before the titration is carried out? 1b) What is color of the acidic solution, before any base is added? 1c) What is color of the solution after the equivalence point is reached at a pH of 8?
The metal ion Mn+ was titrated with 0.0500 M EDTA. The initial solution contained 100.0 mL...
The metal ion Mn+ was titrated with 0.0500 M EDTA. The initial solution contained 100.0 mL of 0.0500 M metal ion (Mn+) buffered at a pH of 9.00. a) Calculate the equivalence volume (Veq). b) What is the concentration of the free metal ion at volume V = Veq/2. c) If the conditional formation constant, K’f = 5.4 X 1010, calculate the concentration of free metal ion at volume V = Veq.
A 100 mL sample of 0.060 M is titrated with 0.060 M EDTA at pH 9.00....
A 100 mL sample of 0.060 M is titrated with 0.060 M EDTA at pH 9.00. The value of Kf for the Ca^2+ -EDTA complex is 10.65 and the fraction of free EDTA in the Y^4- form, ay+ , is at pH 9.00. The Y4- was not given how am i suppose to solve this. What is Kf' , the conditional formation constant, for CA^2+ at pH 9.00? What is the equivalence point volume, Ve, in milliliters? Calculate the concentration...
(10) (3) 4. The metal ion Mnt was titrated with 0.0500 M EDTA. The initial solution...
(10) (3) 4. The metal ion Mnt was titrated with 0.0500 M EDTA. The initial solution contained 100.0 mL of 0.0500 M metal ion (M9+) buffered at a pH of 9.00. a) Calculate the equivalence volume (Veg). b) What is the concentration of the free metal ion at volume V = Veg/2. c) If the conditional formation constant, K'r = 5.4 X 1010, calculate the concentration of free metal ion at volume V = Veq. (4)
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...
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 150.0 mL sample of 0.080 M Ca2+ is titrated with 0.080 M EDTA at pH 9.00. The value of log Kr for the Ca2+-EDTA c...
A 150.0 mL sample of 0.080 M Ca2+ is titrated with 0.080 M EDTA at pH 9.00. The value of log Kr for the Ca2+-EDTA complex is 10.65 and the fraction of free EDTA in the Y- form, ay, is 0.041 at pH 9.00. What is K/, the conditional formation constant for Ca²+ at pH 9.00? What is the equivalence point volume, Ve, in milliliters? ml V = Ve= Calculate the concentration of Ca²+ at V = { v. [Ca2+1...
A 140.0 mL sample of 0.080 M Ca2+ is titrated with 0.080 M EDTA at pH...
A 140.0 mL sample of 0.080 M Ca2+ is titrated with 0.080 M EDTA at pH 9.00. The value of log?f for the Ca2+−EDTA complex is 10.65 and the fraction of free EDTA in the Y4− form, ?Y4− , is 0.041 at pH 9.00. What is ?′f , the conditional formation constant, for Ca2+ at pH 9.00? ?′f= What is the equivalence point volume, ?e , in milliliters? ?e= mL Calculate the concentration of Ca2+ at ?=12?e . [Ca2+]= M...
1. What is the amount in grams of EDTA you will need to measure out to prepare a 250 mL 0.01 M EDTA solution ? The molar mass of EDTA is 374.27 g/mol. 2. Titration Data from three water samples Water Volume of 0.01 Water Drops of MEDTA Moles Ca2+ sample indicator used to of concentration volume Calmagite reach Ca2+ in water (M) end point source 50 mL4 2 ml USFISA drinking water fountain USF BSF drinking water fountain 50...
(10) (3) 4. The metal ion Mnt was titrated with 0.0500 M EDTA. The initial solution contained 100.0 mL of 0.0500 M metal ion (M9+) buffered at a pH of 9.00. a) Calculate the equivalence volume (Veg). b) What is the concentration of the free metal ion at volume V = Veg/2. c) If the conditional formation constant, K'r = 5.4 X 1010, calculate the concentration of free metal ion at volume V = Veq. (4)
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 150.0 mL sample of 0.080 M Ca2+ is titrated with 0.080 M EDTA at pH 9.00. The value of log Kr for the Ca2+-EDTA complex is 10.65 and the fraction of free EDTA in the Y- form, ay, is 0.041 at pH 9.00. What is K/, the conditional formation constant for Ca²+ at pH 9.00? What is the equivalence point volume, Ve, in milliliters? ml V = Ve= Calculate the concentration of Ca²+ at V = { v. [Ca2+1...
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