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The solution of potassium iodide (if it is not extremely diluted) is more dense.
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Yes, the amount of potassium iodide added to the potassium iodate solution in iodometric titration affects the amount of iodine liberated. Potassium iodide serves as a reducing agent, reacting with the iodate ion to form iodine. The quantity of potassium iodide added determines the rate and completeness of this reaction, impacting the amount of liberated iodine available for titration.
No, Lugol's solution is not flammable. It is a solution of iodine and potassium iodide in water, and it does not pose a fire hazard.
When potassium iodide is oxidized, it forms iodine. Potassium iodide loses electrons hence it is oxidized. This reaction can be observed by the change in color of the solution from colorless to brown/yellow due to the formation of iodine.
Potassium iodide (SSKI) contains only potassium iodide dissolved in water, while Lugol's solution contains a combination of potassium iodide and elemental iodine dissolved in water. Lugol's solution is typically more concentrated and is used for certain medical procedures, while SSKI is used primarily as a nutritional supplement to prevent iodine deficiency.
To calculate the molarity, you first need to convert the mass of KI to moles using its molar mass (166 g/mol). Then, divide the moles by the volume of solution in liters (0.1 L) to get the molarity. The molarity of the solution is approximately 1.45 M.
To prepare a 5% potassium iodide solution, weigh 5 grams of potassium iodide and dissolve it in 100 mL of water. Stir until the potassium iodide is completely dissolved to achieve a 5% solution.
To find the number of moles of potassium iodide needed, multiply the volume of the solution (750 ml) by the molarity (1.8 moles/L). First, convert the volume to liters (750 ml = 0.75 L), then multiply 0.75 L by 1.8 moles/L to get 1.35 moles of potassium iodide.
A strong iodide solution that contains 5% iodine and 10% potassium iodide is often used for iodine tinctures or antiseptic solutions. This combination provides a powerful disinfectant with broad antimicrobial properties, commonly used for wound care and surface disinfection. It is important to handle strong iodide solutions with care due to their potency and potential for skin irritation.
The solution of potassium iodide (if it is not extremely diluted) is more dense.
A yellow precipitate of lead iodide is formed due to the reaction between potassium iodide and lead nitrate. This reaction is a double displacement reaction, where the potassium from potassium iodide swaps places with the lead from lead nitrate, forming the insoluble lead iodide.
Potassium iodide solution is a compound because it is a pure substance made up of potassium and iodine chemically bonded together in a fixed ratio.
When potassium iodide and lead nitrate are mixed, a yellow precipitate of lead iodide forms in the solution, while potassium nitrate remains dissolved in the liquid.
The symbol equation for silver nitrate solution and potassium iodide is: AgNO3(aq) + KI(aq) -> AgI(s) + KNO3(aq).
When ferric chloride (FeCl3) is added to a solution of potassium iodide (KI), it reacts to form iron(III) iodide (FeI3) and potassium chloride (KCl). The iron(III) iodide produced is a brownish-red color, indicating the presence of the Fe3+ ion. This reaction can be represented by the following chemical equation: 2FeCl3 + 6KI -> 2FeI3 + 6KCl
The compound precipitate formed when potassium iodide is added to a solution of lead nitrate is lead iodide, which is a yellow precipitate. This reaction is a double displacement reaction where the potassium ion and nitrate ion switch partners to form potassium nitrate and lead iodide.