Aim: Estimate the amount of Nickel present in a given solution as bis(dimethylglyoximato)nickel(II) gravimetrically by counterpoise filter paper.
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Nickel(II) reacts with dimethylglyoxime [C4H6(NOH)2] to form a neutral coordination complex. The formation of the red chelate occurs quantitatively in an aqueous solution at pH 5 to 9. Usually, citric acid is added to lower the interference of other ions like iron.
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![SHREE MALLIKARJUN COLLEGE SYBSC
SAFETY: Refer to MSDS of nickel nitrate, nickel chloride, dimethylglyoxime, citric acid, ethanol
-Dr. Mithil S. Fal Desai
Aim: Estimate the amount of Nickel present in a given solution as
bis(dimethylglyoximato)nickel(II) gravimetrically by counterpoise filter paper.
Chemicals: Nickel salt (nickel nitrate, nickel chloride), dimethylglyoxime, citric acid, ethanol.
Apparatus: Beaker, conical flask, funnel, Whatman 41, glass rod with policemen, water bath,
oven.
Theory: Nickel(II) reacts with dimethylglyoxime [C4H6(NOH)2] to form a neutral coordination
complex. The formation of the red chelate occurs quantitatively in an aqueous solution at pH 5
to 9. Usually, citric acid is added to lower the interference of other ions like iron.
Reaction
Ni2+
(aq)+ 2C4H8N2O2(aq) [Ni(C4H7N2O2)2](s) + 2H+
(aq)
Procedure:
1) Pipette out 25 mL of nickel solution in a 100 mL beaker and add 5 mL of 0.5% citric acid
solution with constant stirring.
2) Add 25 mL of 1% dimethylgloxime solution to the beaker (red color precipitate is formed)
and keep the beaker along with precipitate to digest in a water bath for 30 min.
3) After 30 min, cool the solution and add 1-2 mL of DMG solution along the sides of the beaker
and check for complete precipitation.
4) Take 2 filter papers having the same weight and place them in the same funnel. (If the weight
of the two filter papers is not equal cut the top edge of filter paper to adjust the weight.)
5) Transfer the precipitate to the filter paper and wash the precipitate with distilled water until
the filtrate shows a negative chloride test. Finally, add 5-10 mL of alcohol to remove the excess
water.
6) Keep the funnel along with filter paper in the oven at 80-90 0C for around 45 min.
7) After 45 min, cool the filter papers in a desiccator and then weigh both the filter papers with
(W1) and without precipitate (W2). (To get the constant weights to repeat the step 6 and 7)
8) The difference in weight quantitatively corresponds to Ni-DMG complex formed.
Observation
Table 1.
Constant
weight of filter
paper without
precipitate
“W1’ (g)
Constant
weight of filter
paper with
precipitate
“W2’ (g)
Weight of
Ni-complex
‘A’=W2 – W1
(g)
Molecular
weight of
Complex
‘B’ (g)
Atomic weight
Ni ‘C’(g)
Amount of Ni
in 25 mL
‘x' = A* C/B
(g)
58.71
Result: Amount of nickel in 500 mL is ______g.
Note: To get a better result G4 crucible shall be used.](https://image.slidesharecdn.com/determinationofni-dmg-210421045100/85/Aim-Estimate-the-amount-of-Nickel-present-in-a-given-solution-as-bis-dimethylglyoximato-nickel-II-gravimetrically-by-counterpoise-filter-paper-1-320.jpg)
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Lab 9: Chemical Reactions II
Pre-lab Questions
1. What is a limiting reagent?
2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield.
Experiment: Synthesis of Garden Lime
Procedure
**Take photographs of your experiment set up and your results. Submit them with your laboratory report.**
1. Table 1 provides an example set of data for 1.0 g CaCl2.
2. For Trial 1, weigh into a 250 mL beaker the amount of calcium chloride (CaCl2) shown in Table 1. Record the exact mass you weigh out in the Trial 1 column of the Data section.
3. Measure 50.0 mL of distilled water into a 100 mL graduated cylinder. Pour the water into the 250 mL beaker with the calcium chloride.
4. Stir the solution with a stirring rod until all of the calcium chloride is dissolved.
5. Weigh out 2.5 g of potassium carbonate (K2CO3) in a 50 mL beaker. Record the exact mass in the Data section.
6. Measure 25.0 mL of distilled water into a 100 mL graduated cylinder. Add the water into the 50 mL beaker containing the potassium carbonate.
7. Stir the potassium carbonate in the distilled water with a stirring rod until it is all dissolved.
8. Pour the K2CO3 solution into the 250 mL beaker that has the CaCl2 solution. Rinse the beaker that contained the K2CO3 with a few mL of water and add this to the CaCl2 solution. Stir the mixture.
9. As soon as the reaction begins, record your observations in the Data section. Continue stirring until you see no more precipitate forming.
10. Set up the funnel in the Erlenmeyer flask as shown in Figure 2.
HINT: Do NOT begin filtering yet!
11. Zero the scale and weigh a piece of filter paper and a watch glass. Record the masses of both items in the Data section.
12. Prepare a filtering funnel as shown in Figure 2: fold a piece of filter paper in half twice to make quarters, and open the paper to make a small cone (three quarters are open on one side and one quarter is on the opposite side). Place the paper cone into the funnel and hold it in place with your fingers. Pour a small amount of distilled water through the paper to secure it inside the funnel.
13. Filter the mixture by pouring it into the filter paper in the funnel. Use the stirring rod and distilled water in a wash bottle to transfer the entire solid into the filter paper.
HINT: For best results, be sure to transfer all of the precipitate into the filter paper. Use a rubber policeman if it is available to help with the transfer.
14. Rinse the remaining solid in the filter paper twice with distilled water from a wash bottle to rinse off excess sodium chloride (NaCl). After all the liquid has filtered through, rinse the product with approximately 5 mL of ethanol to aid in its drying. Allow the ethanol to completely finish filtering through the paper.
15. Remove the filter paper carefully so as to not lose any product. Gently unfold the filter paper and lay it flat on the pre-weighed wat ...
Synthesizing nickle ammonium chloride chemistry two
The document describes a lab procedure for synthesizing and analyzing Ni(NH3)nCl2. Students will synthesize the compound from NiCl2∙6H2O, then use a back titration method to determine the mass percent of NH3 in the product. They will titrate the sample with excess HCl, then back titrate the leftover HCl with NaOH. The mixed indicator bromocresol green and methyl red will signal the endpoint, allowing calculation of NH3 content from reagent amounts and volumes. The procedure aims to accurately determine NH3 mass percent while avoiding issues like volatile loss during direct titration.
Unit 4 Lab StoichiometryCHEM 1806Purpose To practice the conce.docx
Unit 4 Lab: StoichiometryCHEM 1806
Purpose: To practice the concept of Stoichiometry
Materials: Student Supplied – Distilled water, paper towels, small paper cup, mug
LabPaq materials: 100 mL glass beaker, Funnel, 25 mL cylinder, Goggles, Digital Scale, Weighing boat, 2.5 g Calcium chloride, dehydrate, Filter paper, 2 g Sodium carbonate.
Procedure:
1. While wearing goggles, weigh out 1.0 g CaCl2 and put it into the 100 mL beaker. Record the actual mass of CaCl2 you are using in Table 1.
2. Add 25 mL of distilled water to the beaker and stir. This is now the “Calcium chloride solution”
3. Calculate how much sodium carbonate you will need for a full reaction. Write that calculation in the Results and Discussion section.
4. Weigh out the calculated amount of Na2CO3 and put it in a small paper cup. (Record actual mass in Data Table 1)
5. Add 25 mL distilled water to the paper cup and stir to make “sodium carbonate solution.”
6. Pour the sodium carbonate solution into the beaker with the calcium chloride solution.
7. Record observations. Write out the reaction of what occurred in the results section. (The solid is calcium carbonate.)
8. Fold the filter paper in half, then in quarters. Record the mass of the filter paper.
9. Place the filter paper in the funnel and open one side.
10. Place the funnel in a mug or other cup to balance it.
11. Carefully swirl and pour the contents of the beaker into the filter paper. (Don’t let the solution overflow.)
12. Rinse the beaker with 1-3mL of distilled water and pour that water into the filter paper as well. (If there is a little solid left in the beaker, leave it. It is experimental error.)
13. When the liquid has drained, lay the filter paper and precipitate on a plate or paper towels to allow it to dry. (mine took overnight, some people take 3 days)
14. When dry, weigh the precipitate + filter paper, record it, and calculate the mass of the precipitate.
15. In the discussion, calculate the theoretical yield and percent yield.
(4 pts) Data:
Table 1: Data
Mass of CaCl2
Mass of Na2CO3 needed
Actual mass of Na2CO3 used
Observation of reaction
Mass of filter paper
Mass of filter paper + precip
Actual yield of Calcium Carbonate
1. (3 pts) Calculate how much Na2CO3 you need to completely react your mass of CaCl2. (Show that calculation here)
2. (2 pts) Write out the reaction that occurred to form calcium carbonate. Remember to identify the phases and balance the equation.
3. (2 pts) Calculate the actual yield of Calcium Carbonate. (Show your work)
4. (2 pts) Calculate the theoretical yield of Calcium Carbonate. (Show your work)
5. (2 pts) Calculate your percent yield of Calcium Carbonate. (Show your work)
Insert a picture of your filter paper with yield for 2 pts extra credit. ;-)
When you are finished, save the file as LASTNAME_Stoich and upload it to the Dropbox for Unit 4 Labs.
Unit 4 Lab: Ionic ReactionCHEM 1806
Purpose: To observe several ionic reactions and practice net ionic equations
...
Complex Preparation lab manual
This document provides procedures for preparing several transition metal complexes. It describes preparing hexaamminecobalt(III)chloride from cobaltous chloride hexahydrate and ammonium chloride. It also describes preparing hexaamminenickel(II)chloride from nickel chloride hexahydrate and aqueous ammonia, as well as potassium tris(oxalato)ferrate(III) trihydrate from ferrous ammonium sulfate and oxalic acid. The document gives the name, structure, properties and theoretical yield calculations for each complex prepared.
How to write laboratory report (journal)
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Chemical reduction technique for the synthesis of nickel nanoparticles
Chemical reduction technique was used to synthesize nickel powder using hydrazine hydrate as reducing agent,
nickel chloride hexahydrate as precursor and polyvinylpyrrolidone (PVP) as capping agent in ethylene glycol
medium. Experiments were carried out with mole ratios 13:1 and 20:1 of hydrazine to nickel chloride
hexahydrate by keeping the amounts of ethylene glycol and NaOH as constant. Variation of capping agent
concentration and temperature was also studied. X-ray diffraction (XRD) analysis was performed and the crystal
size was calculated using Debye-Scherrer equation. XRD peaks where corresponds to that of the face-centered
cubic nickel crystals, in accordance with the literature. Likewise, no oxygen peaks were found in XRD pattern,
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electron microscopy (SEM) and the elemental composition was determined using energy dispersive X-ray
analysis. The elemental composition was found to be nickel with small traces of oxygen.
Chapter 27
Gravimetric analysis is a technique for determining the amount of an analyte by converting it into a solid product whose mass can be easily measured. There are two main types of gravimetric analysis: combustion analysis and precipitation analysis. Combustion analysis involves burning a sample to convert carbon and hydrogen into gases like CO2 and H2O whose masses are then measured. Precipitation analysis involves adding a reagent to convert the analyte into a solid precipitate. The mass of the solid precipitate is then measured to calculate the original amount of analyte. Key factors that affect precipitation analysis include the solubility, filterability, and purity of the solid product. Gravimetric analysis is an accurate and inexpensive analytical technique
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Probing of DNA structured with Nanoparticles
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Synthesis and Characterization of Silica-Nickel Nanocomposite through sol-gel...
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To estimate the amount of zinc as zn2 p2o7 in the given solution of zinc sulp...
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IIT JEE Main Sample Paper Set2 Questions
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To estimate the amount of nickel as ni dmg in the solution of nickel chloride...
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ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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Aim: Estimate the amount of Nickel present in a given solution as bis(dimethylglyoximato)nickel(II) gravimetrically by counterpoise filter paper.
- 1. SHREE MALLIKARJUN COLLEGE SYBSC SAFETY: Refer to MSDS of nickel nitrate, nickel chloride, dimethylglyoxime, citric acid, ethanol -Dr. Mithil S. Fal Desai Aim: Estimate the amount of Nickel present in a given solution as bis(dimethylglyoximato)nickel(II) gravimetrically by counterpoise filter paper. Chemicals: Nickel salt (nickel nitrate, nickel chloride), dimethylglyoxime, citric acid, ethanol. Apparatus: Beaker, conical flask, funnel, Whatman 41, glass rod with policemen, water bath, oven. Theory: Nickel(II) reacts with dimethylglyoxime [C4H6(NOH)2] to form a neutral coordination complex. The formation of the red chelate occurs quantitatively in an aqueous solution at pH 5 to 9. Usually, citric acid is added to lower the interference of other ions like iron. Reaction Ni2+ (aq)+ 2C4H8N2O2(aq) [Ni(C4H7N2O2)2](s) + 2H+ (aq) Procedure: 1) Pipette out 25 mL of nickel solution in a 100 mL beaker and add 5 mL of 0.5% citric acid solution with constant stirring. 2) Add 25 mL of 1% dimethylgloxime solution to the beaker (red color precipitate is formed) and keep the beaker along with precipitate to digest in a water bath for 30 min. 3) After 30 min, cool the solution and add 1-2 mL of DMG solution along the sides of the beaker and check for complete precipitation. 4) Take 2 filter papers having the same weight and place them in the same funnel. (If the weight of the two filter papers is not equal cut the top edge of filter paper to adjust the weight.) 5) Transfer the precipitate to the filter paper and wash the precipitate with distilled water until the filtrate shows a negative chloride test. Finally, add 5-10 mL of alcohol to remove the excess water. 6) Keep the funnel along with filter paper in the oven at 80-90 0C for around 45 min. 7) After 45 min, cool the filter papers in a desiccator and then weigh both the filter papers with (W1) and without precipitate (W2). (To get the constant weights to repeat the step 6 and 7) 8) The difference in weight quantitatively corresponds to Ni-DMG complex formed. Observation Table 1. Constant weight of filter paper without precipitate “W1’ (g) Constant weight of filter paper with precipitate “W2’ (g) Weight of Ni-complex ‘A’=W2 – W1 (g) Molecular weight of Complex ‘B’ (g) Atomic weight Ni ‘C’(g) Amount of Ni in 25 mL ‘x' = A* C/B (g) 58.71 Result: Amount of nickel in 500 mL is ______g. Note: To get a better result G4 crucible shall be used.