When used for treating heavy metal poisoning the EDTA solution much have an approximately neutral...
When used for treating heavy metal poisoning the EDTA solution much have an approximately neutral pH. Explain which conjugate pair would be used to make this solution.
Homework Answers
EDTA (Ethylenediaminetetraacetic acid) is used in various medicinal applications, one of them is de-toxification of poisoning caused.
This is achieved by the chelation process.
Calcium disodium ethylenediamine tetraacetic acid is the chelation product used to treat poisoning. This CaNa2EDTA is more useful to treated poisoning caused due to metals that have a higher affinity towards this product than towards calcium.
Chelating agent + Micronutrients reaction helps to remove heavy metals through urine. The role of neutral pH is to enhance the action of EDTA chelation, which is key in this detoxification.
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When used for treating heavy metal poisoning the EDTA solution much have an approximately neutral...
2. Ethylenediaminetetraacetic acid (EDTA) is used for a range of applications because of its ability to...
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...
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...
EDTA (ethylenediaminetetraacetic acid) is the most widely used metal chelator in analytical chemistry, which forms strong...
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...
Lab 9 - Qualitative Analysis of Cations One common compound that is used in detecting metal...
Lab 9 - Qualitative Analysis of Cations One common compound that is used in detecting metal cations is ethylenediaminetetraacetic acid or simply EDTA. EDTA forms complexes with metals cations which effectively chelates them in solution. The EDTA- anion binds the metal cations which often result in a chelated metal-EDTA anion. For example, iron (III) will form the [Fe(EDTA)]- anion and would be highly soluble in water. With this information, would EDTA be useful in this lab for detecting the 9...
1. The pH of coffee is approximately 5.5. How many times greater is the (H') in Concom neutral water? Solution: 2....
1. The pH of coffee is approximately 5.5. How many times greater is the (H') in Concom neutral water? Solution: 2. Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone in kilograms is required to completely neutralize a 3.8 x 10°L lake with a pH of 4.5? Solution:
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the so...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
Question 13 The pH of a solution is 2.62 at 25°C. Calculate the pOH of this...
Question 13 The pH of a solution is 2.62 at 25°C. Calculate the pOH of this solution at 25°C. 4.88 11.4 8.33 Question 18 Calculate the pH of a 0.400 mol L-1 solution of formic acid, Kg = 1.8 x 10-4 2.29 2.07 4.00 3.44 3.71 Question 30 2 pts Which of the following is TRUE? A buffer has the best resistance to pH change when the buffer's pH is significantly lower than the pk, of the acid used to...
Buffers 1. Indicate which of the following pairs of compounds could be used to make a buffer solution by placing an X i...
Buffers 1. Indicate which of the following pairs of compounds could be used to make a buffer solution by placing an X in the appropriate column. Buffer Solution | Not a Buffer Solution Pair of Compounds HF and Cl H.COs and OH HNO2 and NO NHa and NH L 2. Write out the reaction of acetic acid CH.COOH reacting with water. 3. What is the pH of a buffer solution in which the (CH3COOH) is 0.229 M and the (CH...
Complete the table for an aqueous solution @ 25°C each row represents one solution Грн POH...
Complete the table for an aqueous solution @ 25°C each row represents one solution Грн POH 3.25 0.25 (H) (OH) Acidic or basic 6.14x10 12.25 1.77 9.83x102 A 0.185M solution of weak acid has a pH of 2.95. Calculate the lonization constant (K) for the acid. For this you will need to determine the relationship between the [HA], and the [H01. You're given [HA] and you'll need to find [H,0+- you can get this from pH. Just as we have...
Extraction Q1. Why doesn’t the neutral organic compound dissolve in the 1.5 M NaOH solution? Q2....
Extraction Q1. Why doesn’t the neutral organic compound dissolve in the 1.5 M NaOH solution? Q2. Why is diethyl ether a good choice for the organic solvent in this extraction experiment? Q3. What experimental difficulty would you encounter if you neglected to include the drying step before evaporating the ether solution of the neutral organic compound? Q4. Why are the two organic compounds recrystallized before their melting points are determined? Q5. What IR bands are most useful in distinguishing a...
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...
Lab 9 - Qualitative Analysis of Cations One common compound that is used in detecting metal cations is ethylenediaminetetraacetic acid or simply EDTA. EDTA forms complexes with metals cations which effectively chelates them in solution. The EDTA- anion binds the metal cations which often result in a chelated metal-EDTA anion. For example, iron (III) will form the [Fe(EDTA)]- anion and would be highly soluble in water. With this information, would EDTA be useful in this lab for detecting the 9...
1. The pH of coffee is approximately 5.5. How many times greater is the (H') in Concom neutral water? Solution: 2. Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone in kilograms is required to completely neutralize a 3.8 x 10°L lake with a pH of 4.5? Solution:
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
Question 13 The pH of a solution is 2.62 at 25°C. Calculate the pOH of this solution at 25°C. 4.88 11.4 8.33 Question 18 Calculate the pH of a 0.400 mol L-1 solution of formic acid, Kg = 1.8 x 10-4 2.29 2.07 4.00 3.44 3.71 Question 30 2 pts Which of the following is TRUE? A buffer has the best resistance to pH change when the buffer's pH is significantly lower than the pk, of the acid used to...
Buffers 1. Indicate which of the following pairs of compounds could be used to make a buffer solution by placing an X in the appropriate column. Buffer Solution | Not a Buffer Solution Pair of Compounds HF and Cl H.COs and OH HNO2 and NO NHa and NH L 2. Write out the reaction of acetic acid CH.COOH reacting with water. 3. What is the pH of a buffer solution in which the (CH3COOH) is 0.229 M and the (CH...
Complete the table for an aqueous solution @ 25°C each row represents one solution Грн POH 3.25 0.25 (H) (OH) Acidic or basic 6.14x10 12.25 1.77 9.83x102 A 0.185M solution of weak acid has a pH of 2.95. Calculate the lonization constant (K) for the acid. For this you will need to determine the relationship between the [HA], and the [H01. You're given [HA] and you'll need to find [H,0+- you can get this from pH. Just as we have...
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