0
Add your answer:
Earn +20 pts
Why blue colour of an iodine solution dischargers when sodium thiosulphate aded?
When sodium thiosulfate is added to an iodine solution, a reaction occurs where iodine is reduced to iodide ions by thiosulfate, causing the blue color to disappear. This is due to the formation of a colorless complex between iodine and thiosulfate, resulting in a color change.
How you neutralize Iodine solutions?
To neutralize iodine solutions, you can add a reducing agent such as sodium thiosulfate or sodium bisulfite. These chemicals will react with the iodine to form iodide ions, reducing the concentration of free iodine in the solution. It is important to carefully follow established laboratory protocols and safety measures when handling these chemicals.
What ions form when Potassium and Iodine react and what are their symbols?
When potassium and iodine react, they form potassium iodide. The ions involved are K+ (potassium ion) and I- (iodide ion).
How does potassium and sodium thiosulphate turn yellow?
Potassium and sodium thiosulfate can turn yellow due to the formation of a colored complex with iodine. When iodine is added to a solution containing thiosulfate, it forms a triiodide ion which has a yellow color. This reaction is commonly used in chemistry as an indicator for the presence of thiosulfate ions in solution.
Does sodiun thiosulphate reacts with silverchloride?
Yes, sodium thiosulfate can react with silver chloride to form a complex, but it is not a direct chemical reaction. When sodium thiosulfate is added to a solution containing silver chloride, the thiosulfate ions can complex with the silver ions liberated from the silver chloride, forming a soluble complex called a coordination compound.
Why blue colour of an iodine solution dischargers when sodium thiosulphate aded?
When sodium thiosulfate is added to an iodine solution, a reaction occurs where iodine is reduced to iodide ions by thiosulfate, causing the blue color to disappear. This is due to the formation of a colorless complex between iodine and thiosulfate, resulting in a color change.
How you neutralize Iodine solutions?
To neutralize iodine solutions, you can add a reducing agent such as sodium thiosulfate or sodium bisulfite. These chemicals will react with the iodine to form iodide ions, reducing the concentration of free iodine in the solution. It is important to carefully follow established laboratory protocols and safety measures when handling these chemicals.
What ions form when Potassium and Iodine react and what are their symbols?
When potassium and iodine react, they form potassium iodide. The ions involved are K+ (potassium ion) and I- (iodide ion).
How does potassium and sodium thiosulphate turn yellow?
Potassium and sodium thiosulfate can turn yellow due to the formation of a colored complex with iodine. When iodine is added to a solution containing thiosulfate, it forms a triiodide ion which has a yellow color. This reaction is commonly used in chemistry as an indicator for the presence of thiosulfate ions in solution.
Do iodine and lithium bromide react?
Iodine and lithium bromide do not react with each other. However, iodine can form a complex with lithium ions in a solution containing lithium bromide.
Why KI doesn't react with Na2S2O3?
Potassium iodide (KI) does not react with sodium thiosulfate (Na2S2O3) because the two compounds belong to different chemical families and do not have a significant affinity for each other. KI is a salt of potassium and iodine, while sodium thiosulfate is a salt of sodium and thiosulfate ions. The lack of reactivity between KI and Na2S2O3 is due to their stable chemical structures and the absence of driving forces for a reaction to occur.
Does sodiun thiosulphate reacts with silverchloride?
Yes, sodium thiosulfate can react with silver chloride to form a complex, but it is not a direct chemical reaction. When sodium thiosulfate is added to a solution containing silver chloride, the thiosulfate ions can complex with the silver ions liberated from the silver chloride, forming a soluble complex called a coordination compound.
WHAT happens when sodium atoms react with iodine atoms to produce sodium iodine?
When sodium atoms react with iodine atoms, they undergo a redox reaction to form sodium iodide. Sodium atoms lose an electron to form Na+ ions, while iodine atoms gain an electron to form I- ions. These ions then combine to form sodium iodide crystals.
Why amnomiun thiocyanate is added in the titration of sodium thiosulphate with copper?
Ammonium thiocyanate is added in the titration of sodium thiosulphate with copper to detect the end point of the reaction. When all the thiosulfate ions react with copper ions, excess copper ions will react with ammonium thiocyanate forming a reddish-brown complex. This color change indicates that all the thiosulfate has reacted and the titration is complete.
Why hypo is commonly used as a reducing agent in iodine titrations?
Hypo, or sodium thiosulfate, is commonly used as a reducing agent in iodine titrations because it reacts with iodine to form iodide ions. This reaction helps in determining the amount of iodine present in the solution, as iodine is reduced to iodide ions. This reaction is quantitative and has a clear end point, making hypo a suitable reducing agent for iodine titrations.
When leadII nitrate reacts with sodium iodine what is the correct formula for the product ledII iodine?
The correct formula for the product of lead(II) nitrate reacting with sodium iodide is lead(II) iodide, which has the formula PbI2. This is because lead(II) ions from lead(II) nitrate react with iodide ions from sodium iodide to form lead(II) iodide as the product.
Why is sodium thiosulphate used in iodometric titration?
Sodium thiosulfate is used in iodometric titration as a titrant to react with excess iodine after it has reacted with the analyte. This reaction helps determine the amount of iodine that reacted with the analyte, enabling the quantification of the analyte's concentration. Sodium thiosulfate is preferred due to its ability to efficiently reduce iodine to iodide ions in a one-to-one stoichiometry.
