EDTA (ethylenediaminetetraacetic acid) is the most widely used metal chelator in analytical chemistry, which forms strong 1:1 complexes with most metal ions. Water hardness can be determined by titrating Ca2+, Mg2+ and other metal ions with EDTA. During the titration, ammonium-ammonium chloride buffer is often used. Which of the following descriptions about the function of ammonium-ammonium chloride is/are correct?
To act as a masking agent
To form complex with Ca2+ and Mg2+
To be used as a metal ion indicator
To maintain the pH of the solution around 10
Correct answer is d) To maintain the pH of solution around 10.
Explanation: EDTA is insoluble in water at low pH. It is because, the most prominant species is H4Y.
For metals ion to form complexes with EDTA, it must be present in anionic form so that metals do not have to abstract protons from them. When pH is increased, the protons start dissociating. At pH 10, Y4- is predominant and hence, the complexometric reaction proceeds swiftly.
EDTA (ethylenediaminetetraacetic acid) is the most widely used metal chelator in analytical chemistry, which forms strong...
i am insure what are the correct answers for this one EDTA Titration 1. EDTA (cthylenediaminetetraacetic acid) is the most widely used metal chelator in analytical chemistry, which forms strong 1:1 complexes with most metal ions. Water hardness can be determined by titrating Ca, Mg and other metal ions with EDTA. During the titration, ammonium-ammonia chloride buffer is often used. Which of the following descriptions about the function of ammonium-ammonia chloride is/are correct? (a) To react with EDTA To form...
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...
2. Ethylenediaminetetraacetic acid (EDTA) is used for a range of applications because of its ability to strongly bind metal ions via its six ligating groups. EDTA is used in the paper industry to bind Mn2+ (and other metal) ions from catalyzing the decomposition of hydrogen peroxide (H2O2), which is an important chemical for bleaching the pulp. In this example, we are going to focus on the chelation of free Mn2+ ions in a solution at pH = 7. a) If...
Ethylenediaminetetraacetic acid (EDTA) is used for a range of applications because of its ability to strongly bind metal ions via its six ligating groups. EDTA is used in the paper industry to bind Mn2+ (and other metal) ions from catalyzing the decomposition of hydrogen peroxide (H2O2), which is an important chemical for bleaching the pulp. In this example, we are going to focus on the chelation of free Mn2+ ions in a solution at pH = 7. (a) If there...
2. Calculate the concentration of one liter of the resulting calcium chloride solution (assuming you started with 102.7 mg of calcium carbonate) in units of molar and millimolar. Also calculate the concentration in “parts-per-million as CaCO3”. (Refer to section 13.5 of your textbook, if needed.) a. If a standard Ca2+ solution is 100 ppm and 50 mL of solution is used for the standardization, calculate the approximate volume of 2.5 mM EDTA4- solution needed to reach the end point of...
1. Write the balanced equation for the reaction between calcium carbonate and hydrochloric acid in water, generating aqueous calcium chloride and liberating carbon dioxide gas. (You will need this for Part 1 of the experiment!) 2. Calculate the concentration of one liter of the resulting calcium chloride solution (assuming you started with 102.7 mg of calcium carbonate) in units of molar and millimolar. Also calculate the concentration in "parts-per-million as CaCO3". (Refer to section 13.5 of your textbook, if needed.)...
The following primary standards can be used for the standardization of bases except. a. Benzoic acid b. Oxalic acid c. CaCO3 d. KHP A solution that may contain NaOH, Na 2CO3, and NaHCO3, alone or in compatible combination was titrated with 0.1200 M HCl. The volume of the acid required to reach the phenolphthalein endpoint was 25.67 mL while 38.13 mL to reach the methyl red endpoint. What are the components of the mixture? a. Na2CO3 only b. NaOH only...