It is given that, when sodium chloride is added to a solution of silver nitrate, a white precipitate is formed. This precipitate will be dissolved when ammonia is added to this mixture. Now a pale yellow precipitate will appear when a solution of potassium bromide is added to it. Now this precipitate will be dissolved when sodium thiosulfate is added and finally a yellow precipitate is formed when potassium iodide is added to this solution. The balanced equations are to be stated to explain these observations. The conclusion drawn corresponding to the size of the K sp values for AgCl , AgBr and AgI is to be stated. Concept introduction: The formation of solid in a solution is known as precipitation. Solubility product, K sp , is defined as the concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
It is given that, when sodium chloride is added to a solution of silver nitrate, a white precipitate is formed. This precipitate will be dissolved when ammonia is added to this mixture. Now a pale yellow precipitate will appear when a solution of potassium bromide is added to it. Now this precipitate will be dissolved when sodium thiosulfate is added and finally a yellow precipitate is formed when potassium iodide is added to this solution. The balanced equations are to be stated to explain these observations. The conclusion drawn corresponding to the size of the K sp values for AgCl , AgBr and AgI is to be stated. Concept introduction: The formation of solid in a solution is known as precipitation. Solubility product, K sp , is defined as the concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
Solution Summary: The author explains that the formation of solid in a solution is known as precipitation. The balanced equations are to explain these observations.
It is given that, when sodium chloride is added to a solution of silver nitrate, a white precipitate is formed. This precipitate will be dissolved when ammonia is added to this mixture. Now a pale yellow precipitate will appear when a solution of potassium bromide is added to it. Now this precipitate will be dissolved when sodium thiosulfate is added and finally a yellow precipitate is formed when potassium iodide is added to this solution. The balanced equations are to be stated to explain these observations. The conclusion drawn corresponding to the size of the
Ksp values for
AgCl,AgBr and
AgI is to be stated.
Concept introduction:
The formation of solid in a solution is known as precipitation. Solubility product,
Ksp, is defined as the concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution.
What happens to the buffer system if some hydrochloric acid is added to the solution?
The hydrochloric acid reacts with the fluoride ions so the pH decreases only slightly.
The hydrochloric acid reacts with the fluoride ions so the pH decreases significantly.
) The hydrochloric acid reacts with the hydrofluoric acid so the pH increases only slightly.
The hydrochloric acid reacts with the hydrofluoric acid so the pH increases significantly.
Explain why some precipitates do not dissolve once formed with HCl. Explain by showing some examples.
What change will be caused by addition of a small amount of HCI to a solution containing fluoride ions and hydrogen fluoride?
A) The concentration of fluoride ions will increase as will the concentration of hydronium ions
B) The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase.
*) The fluoride ions will precipitate out of solution as its acid salt.
D) The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase.
E) The concentration of hydronium ions will increase signiticantly.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell