Tin chloride, also known as stannous chloride, is used in various chemical reactions, including precipitation reactions. It forms precipitates with many metals, often as insoluble chlorides. However, as I mentioned before, it's particularly interesting in the context of precious metals like gold and platinum group metals (PGMs) due to its selective reactions. When using tin chloride in solution, observing a blue coloration can indicate the presence of certain PGMs, such as iridium. This color change is due to the formation of specific complexes between the tin ions and the metal ions in solution. These complexes often have distinctive colors, which can be used as qualitative tests for the presence of particular metals. In the case of iridium, the formation of a blue complex with tin chloride is a classic test used in analytical chemistry to detect its presence. This selective reaction is valuable in separating and identifying PGMs from other metals, especially in the context of refining and analysis. However, it's important to note that while the blue coloration can suggest the presence of iridium or other PGMs, further confirmatory tests are typically required for accurate identification and quantification. Additionally, interpretation should consider other possible sources of color interference and potential reactions in the sample matrix. The formation of a green coloration after adding tin chloride solution can indicate the presence of palladium (Pd) in the sample. Like with iridium, palladium forms specific complexes with tin ions, resulting in a green color. The reaction between palladium ions and tin chloride leads to the formation of a complex with a distinct green color. This reaction is utilized in analytical chemistry as a qualitative test for the presence of palladium in solution. Similar to the test for iridium, the green coloration produced by the reaction with tin chloride is a preliminary indication of the presence of palladium. However, further confirmatory tests are typically needed for accurate identification and quantification, especially in complex sample matrices. This selective reaction and color change are valuable tools in the analysis and separation of precious metals, contributing to various applications in refining, mining, and analytical chemistry. While the classic color associated with gold complexes is purple, there are other colors that gold can exhibit depending on its oxidation state and the ligands present in its coordination sphere. Some of these colors include: Yellow: Gold metal itself has a characteristic yellow color, which is why it's often referred to as "yellow gold." Red: Gold(III) complexes can sometimes exhibit a reddish color, especially in certain oxidation states and ligand environments. Orange: Certain gold complexes may appear orange, particularly when they contain ligands that absorb light in the blue region of the spectrum. White or Colorless: In some cases, particularly with very small gold nanoparticles, the color may appear white or colorless, especially when dispersed in solution. Blue: While less common, certain gold complexes, especially those with specific ligands or in unusual oxidation states, can exhibit a blue coloration. These colors can vary based on factors such as the oxidation state of gold, the coordination environment (including the nature of ligands attached to the gold ion), and the presence of other metals or ligands that can interact with the gold ion. Therefore, while purple is indeed a common color associated with gold complexes, the color can vary depending on the specific chemical conditions. ...so yes, your experiment is still very interesting. Most miners are not equipped with the materials, equipment or knowledge as it pertains to invisible elements, and therefore, there is highly likely a rich tapestry underfoot. The potential for discovering valuable elements and compounds, especially those that are invisible or present in trace amounts, is fascinating. Many traditional mining operations focus on extracting visible ores and minerals, often overlooking the wealth of valuable materials that may exist in minute concentrations or in unconventional forms. With advancements in analytical techniques and technology, there's increasing awareness of the presence of valuable elements in various geological formations, including ores that may not be visibly apparent. For example, the presence of precious metals like gold, platinum group metals (PGMs), and rare earth elements (REEs) in low concentrations or in complex mineralogical associations is an area of growing interest for exploration and mining companies. Invisible elements can exist in a variety of forms, from finely dispersed particles to chemical compounds that require specialized extraction and processing methods. Detecting and extracting these elements often require sophisticated analytical instruments and techniques, as well as expertise in mineralogy, geochemistry, and metallurgy. Exploration and mining efforts that incorporate a multidisciplinary approach, combining geological, geochemical, and mineralogical data with advanced analytical methods, have the potential to uncover previously overlooked resources. This can lead to the development of new mining projects and the utilization of innovative extraction and processing technologies to recover valuable materials efficiently and sustainably. Overall, the exploration for and extraction of invisible elements represent exciting opportunities for the mining industry to tap into new sources of wealth while also addressing challenges related to resource depletion and environmental sustainability. ~ CHEERS
With hcl , there in solution was enough hcl so I don’t add new one remember I use urea ? Urea kills just nitric but don’t do nothing to hcl that way you don’t see me adding hcl
Tin chloride, also known as stannous chloride, is used in various chemical reactions, including precipitation reactions. It forms precipitates with many metals, often as insoluble chlorides. However, as I mentioned before, it's particularly interesting in the context of precious metals like gold and platinum group metals (PGMs) due to its selective reactions.
When using tin chloride in solution, observing a blue coloration can indicate the presence of certain PGMs, such as iridium. This color change is due to the formation of specific complexes between the tin ions and the metal ions in solution. These complexes often have distinctive colors, which can be used as qualitative tests for the presence of particular metals.
In the case of iridium, the formation of a blue complex with tin chloride is a classic test used in analytical chemistry to detect its presence. This selective reaction is valuable in separating and identifying PGMs from other metals, especially in the context of refining and analysis.
However, it's important to note that while the blue coloration can suggest the presence of iridium or other PGMs, further confirmatory tests are typically required for accurate identification and quantification. Additionally, interpretation should consider other possible sources of color interference and potential reactions in the sample matrix.
The formation of a green coloration after adding tin chloride solution can indicate the presence of palladium (Pd) in the sample. Like with iridium, palladium forms specific complexes with tin ions, resulting in a green color.
The reaction between palladium ions and tin chloride leads to the formation of a complex with a distinct green color. This reaction is utilized in analytical chemistry as a qualitative test for the presence of palladium in solution.
Similar to the test for iridium, the green coloration produced by the reaction with tin chloride is a preliminary indication of the presence of palladium. However, further confirmatory tests are typically needed for accurate identification and quantification, especially in complex sample matrices.
This selective reaction and color change are valuable tools in the analysis and separation of precious metals, contributing to various applications in refining, mining, and analytical chemistry.
While the classic color associated with gold complexes is purple, there are other colors that gold can exhibit depending on its oxidation state and the ligands present in its coordination sphere. Some of these colors include:
Yellow: Gold metal itself has a characteristic yellow color, which is why it's often referred to as "yellow gold."
Red: Gold(III) complexes can sometimes exhibit a reddish color, especially in certain oxidation states and ligand environments.
Orange: Certain gold complexes may appear orange, particularly when they contain ligands that absorb light in the blue region of the spectrum.
White or Colorless: In some cases, particularly with very small gold nanoparticles, the color may appear white or colorless, especially when dispersed in solution.
Blue: While less common, certain gold complexes, especially those with specific ligands or in unusual oxidation states, can exhibit a blue coloration.
These colors can vary based on factors such as the oxidation state of gold, the coordination environment (including the nature of ligands attached to the gold ion), and the presence of other metals or ligands that can interact with the gold ion. Therefore, while purple is indeed a common color associated with gold complexes, the color can vary depending on the specific chemical conditions.
...so yes, your experiment is still very interesting. Most miners are not equipped with the materials, equipment or knowledge as it pertains to invisible elements, and therefore, there is highly likely a rich tapestry underfoot. The potential for discovering valuable elements and compounds, especially those that are invisible or present in trace amounts, is fascinating. Many traditional mining operations focus on extracting visible ores and minerals, often overlooking the wealth of valuable materials that may exist in minute concentrations or in unconventional forms.
With advancements in analytical techniques and technology, there's increasing awareness of the presence of valuable elements in various geological formations, including ores that may not be visibly apparent. For example, the presence of precious metals like gold, platinum group metals (PGMs), and rare earth elements (REEs) in low concentrations or in complex mineralogical associations is an area of growing interest for exploration and mining companies.
Invisible elements can exist in a variety of forms, from finely dispersed particles to chemical compounds that require specialized extraction and processing methods. Detecting and extracting these elements often require sophisticated analytical instruments and techniques, as well as expertise in mineralogy, geochemistry, and metallurgy.
Exploration and mining efforts that incorporate a multidisciplinary approach, combining geological, geochemical, and mineralogical data with advanced analytical methods, have the potential to uncover previously overlooked resources. This can lead to the development of new mining projects and the utilization of innovative extraction and processing technologies to recover valuable materials efficiently and sustainably.
Overall, the exploration for and extraction of invisible elements represent exciting opportunities for the mining industry to tap into new sources of wealth while also addressing challenges related to resource depletion and environmental sustainability.
~ CHEERS
From Morocco to California big great to you Sir.
Thank u Sar ji❤❤❤
Best ore demonstration for gold💪💪💪👍.
If you roast your ore first it should oxidize pyrite and liberate the gold
If you disolving in aqua regia you don’t need to roast 😜
The sulfur takes your oxidizer away, heat your material first, get rid of sulfur
@@myadventure7069
you could be right but @shermdeazy and @parkertoolman9759 have a point.
Sulfide bonds are weak against the heat
sukses selalu tuan,selamat malam
Merhaba üstad senin sayfanı arapça yayın yapan biri kullanıyor bilmem farkında mısınız
No I don’t know nothing
hangi kanal ?
@@sindecade2023 o kanala abone değilim bir iki kez özledim tekrardan önüme çıkarsa paylaşırım
when you used the potassium nitrate was by itself or with HCL? or with water?
With hcl , there in solution was enough hcl so I don’t add new one remember I use urea ? Urea kills just nitric but don’t do nothing to hcl that way you don’t see me adding hcl
❤❤❤❤❤
NEEES
KNO3 works much better ,very nice
If there be gold then h202 works too but if no gold then no gold .
Birde türkçe alt yazı koyarsan sevinirim
youtube.com/@user-mk2gq6pm4x?si=7L-Kfw3YTetEWUHf
Bilgileri
Senin videonu yayınlayanın
Senin videolarını arapça olarak birisi yayınlıyor
Sir, what is the name of the channel?