Homework Answers
The buffer is used to maintain the pH of the solution around 10.
To stabilize the metal-EDTA complex.
Ammonia acts as a masking agent for zinc ions. Thus minimises the affect go zinc metal ion in determination of hardness of water.
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i am insure what are the correct answers for this one
EDTA Titration 1. EDTA (cthylenediaminetetraacetic...
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...
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...
0.1001 Sample Volume ViEDTA VI EDTA 0135L 02して'8_1 O1241L AVEDTA ,moles EDTA moles EDTA Moles E...
0.1001 Sample Volume ViEDTA VI EDTA 0135L 02して'8_1 O1241L AVEDTA ,moles EDTA moles EDTA Moles EDTA Molesca2. Sample [Ca2* moles Ca moles Ca2 mg CaCO3 mg CaCO3 Sample Hardness USGS Hardness Classification mg CaCO3 Accepted Hardness % Error Chemicals, Materials and Equipment Eriochrome Black T indicator solution (0.4 g/L) Disodium EDTA solution (0.0100 M) Ammonia/Ammonium Chloride Buffer (pH 10) Magneisum Chloride Solution (1x103 M) Saturated CaSO4 solutions previously prepared and equilibrated to 60°C and 90°0C hot/stir plate 60°C and 90°C...
Please show steps for 32 and 33. Data Table 1: EDTA Titration Volume Trial Initial EDTA...
Please show steps for 32 and 33.
Data Table 1: EDTA Titration Volume Trial Initial EDTA Volume (mL) Final EDTA Volume (mL) Total Volume EDTA Used (mL) 1 9 mL 8.6 mL .3mL 2 8.6 6 2.6 mL 3 6 4.2 1.8mL Average Volume of EDTA Used (mL) 1.6mL Data Table 2: Water Hardness Average Volume of EDTA Used (mL) Concentration Ca2+ lons Per Liter of Water (mol/L) Water Hardness (ppm CaCO3) 1.6mL 32 Using the following equation, determine the...
Water Hardness by EDTA Titration Objective: To determine [Ca2+,MG2+] and [Mg2+] concentration in an unknown water...
Water Hardness by EDTA Titration Objective: To determine [Ca2+,MG2+] and [Mg2+] concentration in an unknown water sample A 0.0107 molarity solution of EDTA is prepared for the experiment. 25 mL of an unknown is pipetted and diluted 100 mL with distilled water and adjusted to a pH between 8 and 10 with NH4OH. A 10.00 mL portion of the diluted unknown is transferred to a 250 mL flask with 3 mL of pH 10 ammonia buffer and tiny amount of...
please help with the answers to this pre lab! Date: Analyzing Calcium in Milk 1. Name...
please help with the answers to this pre lab!
Date: Analyzing Calcium in Milk 1. Name three reasons why calcium is an essential element for good nutrition and good health. 2. What features of the EDTA molecule allow it to form stable complexes with metal ions? 3. What is the purpose of adding sodium hydroxide to milk for the EDTA titration of calcium ion? Describe the safety hazards and precautions associated with the use of NaOH solution. 4. What method...
how would I calculate my results from the first two data the first data is my...
how would I calculate my results from the first two data the
first data is my results and the second data I have to calculate
each of those with the information that I have on the first 3
trails I really really need help and i just dont understand thank
you.
1 concentration of EDTA solution 2 molar mass of CaCO3 0.0100 M 100.09 g/mol Trail 1 -Trail 2 Trail 3 12 12.01 11.99 5 Unknown analysis Part 1 (pH...
2. Calculate the concentration of one liter of the resulting calcium chloride solution (assuming you started...
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. For calculating the pH of 0.01010 M KH PO., which of the following strategies is...
1. For calculating the pH of 0.01010 M KH PO., which of the following strategies is correct? A. Treat as monoprotic acid system and use Kai B. Treat as monoprotic acid system and use Kaz C. Treat as amphiprotic system and use Ka, and Kaz D. Treat as amphiprotic system and use Kaz and Kaz 2. A 0.100 M NaOH solution is used for titrating an 0.0750 M acetic acid solution (pKa-4.76). What is the pH of the solution when...
1. Write the balanced equation for the reaction between calcium carbonate and hydrochloric acid in water,...
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.)...
0.1001 Sample Volume ViEDTA VI EDTA 0135L 02して'8_1 O1241L AVEDTA ,moles EDTA moles EDTA Moles EDTA Molesca2. Sample [Ca2* moles Ca moles Ca2 mg CaCO3 mg CaCO3 Sample Hardness USGS Hardness Classification mg CaCO3 Accepted Hardness % Error Chemicals, Materials and Equipment Eriochrome Black T indicator solution (0.4 g/L) Disodium EDTA solution (0.0100 M) Ammonia/Ammonium Chloride Buffer (pH 10) Magneisum Chloride Solution (1x103 M) Saturated CaSO4 solutions previously prepared and equilibrated to 60°C and 90°0C hot/stir plate 60°C and 90°C...
Please show steps for 32 and 33.
Data Table 1: EDTA Titration Volume Trial Initial EDTA Volume (mL) Final EDTA Volume (mL) Total Volume EDTA Used (mL) 1 9 mL 8.6 mL .3mL 2 8.6 6 2.6 mL 3 6 4.2 1.8mL Average Volume of EDTA Used (mL) 1.6mL Data Table 2: Water Hardness Average Volume of EDTA Used (mL) Concentration Ca2+ lons Per Liter of Water (mol/L) Water Hardness (ppm CaCO3) 1.6mL 32 Using the following equation, determine the...
please help with the answers to this pre lab!
Date: Analyzing Calcium in Milk 1. Name three reasons why calcium is an essential element for good nutrition and good health. 2. What features of the EDTA molecule allow it to form stable complexes with metal ions? 3. What is the purpose of adding sodium hydroxide to milk for the EDTA titration of calcium ion? Describe the safety hazards and precautions associated with the use of NaOH solution. 4. What method...
how would I calculate my results from the first two data the
first data is my results and the second data I have to calculate
each of those with the information that I have on the first 3
trails I really really need help and i just dont understand thank
you.
1 concentration of EDTA solution 2 molar mass of CaCO3 0.0100 M 100.09 g/mol Trail 1 -Trail 2 Trail 3 12 12.01 11.99 5 Unknown analysis Part 1 (pH...
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. For calculating the pH of 0.01010 M KH PO., which of the following strategies is correct? A. Treat as monoprotic acid system and use Kai B. Treat as monoprotic acid system and use Kaz C. Treat as amphiprotic system and use Ka, and Kaz D. Treat as amphiprotic system and use Kaz and Kaz 2. A 0.100 M NaOH solution is used for titrating an 0.0750 M acetic acid solution (pKa-4.76). What is the pH of the solution when...
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.)...
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