Show all work fol fuf tieunt! Using LeChatelier\'s principle, decide whether eac
ID: 1043125 • Letter: S
Question
Show all work fol fuf tieunt! Using LeChatelier's principle, decide whether each of the following compounds would be more or less soluble in the following solutions than in pure water. Briefly explain your answer for each. (8 pts) 1. re water silver bromide in 0.100 M HBr more soluble less soluble same solubility Explain silver bromide in 0.100 M HNO3 more soluble less soluble same solubility Explain: iron (I1) hydroxide in 0.100 M HCI Explain: more soluble less soluble same solubility iron (II) hydroxide in 0.100 M Na0OH Explain: more soluble less soluble same solubilityExplanation / Answer
(a)
Silver bromide in HBr is less soluble than in pure water because of release of common Bromide ions by HBr which supress the solubility of silver bromide.
(b)
SIlver bomide i HNO3 is same solubility as in pure water.
(c)
Iron(II) hydroxide in HCl is more solubility than in pure water.
Because, the hydroxide ions from the equilibrium will be removed by the H+ ions coming from HCl and hence the equilibrium is shifted towards right side and hence the solubility is increased.
(d)
Iron(II) hydroxide in NaOH is less soluble than in pure water. Because of the common OH- ions coming from NaOH, the equilibrium will be shifted towards left side and hence the solubility is supressed.