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  • SrSO4 Solubility in Acid - Chemistry Stack Exchange
    $\begingroup$ In analytical chemistry books, $\ce{SrSO4}$ is said to be soluble in boiling concentrated $\ce{HCl}$ and $\ce{HNO3}$ solutions On the other hand, $\ce{BaSO4}$ is said to be soluble in concentrated sulfuric acid, because of the formation of both $\ce{HSO4^-}$ ion and of the complex $\ce{H2[Ba(SO4)_2]}$, which is decomposed by
  • How to determine sulfate ions in a solution by precipitation?
    Well-known insoluble sulfate compounds are $\ce{PbSO4, SrSO4, CaSO4}$, and $\ce{BaSO4}$ Note that all of these cations have a somewhat high (+2) charge and are large Note that all of these cations have a somewhat high (+2) charge and are large
  • Calcium ion and sulfate did not form precipitate
    In fact, the solubilities of $\ce{BaSO4, SrSO4}$ and $\ce{CaSO4}$ are such that a saturated solution of $\ce{SrSO4}$ will always give precipitate when barium is added but never with calcium or strontium; while a saturated solution of $\ce{CaSO4}$ will give a precipitate if either strontium or barium is added but never with calcium
  • Precipitation reaction stoichiometry? - Chemistry Stack Exchange
    First, I wrote the equation: Sr + SO4 -> SrSo4 (I know this is excluding ions, because I am primarily focused on the stoichiometry part) I figured moles of Na2So4 and Sr(NO3)2, which correspond to moles of strontium These are 003 moles Na2SO4 and 0 014 moles Sr(NO3)2
  • inorganic chemistry - Identification of lithium and strontium salts . . .
    This is because $\ce{SrSO4}$ is much less soluble in water than $\ce{Li2SO4}$ ($\pu{0 0132 g}$ versus $\pu{34 8 g}$ in $\pu{100 g}$ of $\ce{H2O}$ at $\pu{20 ^\circ C}$ ) Adding diluted $\ce{HCl_{aq}}$ and $\ce{BaCl2}$ to a solution is commonly used as a test for $\ce{SO4^2-}$ (if it is present, $\ce{BaSO4}$ precipitates)
  • Why does the solubility of some salts decrease with temperature . . .
    What you refer to, the decreased in a solid's solubility in a liquid with increased temperature, is frequently called retrograde or inverse solubility, and occurs when the dissolution of the solute is exothermic
  • solubility - MgSO4 is soluble while BaSO4 isnt, whats the role of . . .
    I came across a question asking the reason behind MgSO4 is soluble while BaSO4 is insoluble in H2O Now, I know Solubility has inverse relation with Lattice energy
  • solubility - Which has a greater dominance: hydration enthalpy or . . .
    lets say i am comparing solubility of sulfate and hydroxides of alkaline earth metals when comparing solubility two terms come into effect Lattice energy and the hydration energy both contribute to the solubility but sometimes there is a dominance of one term over the other In order to account for this dominance a new term was introduced
  • aqueous solution - What determines whether a double displacement . . .
    In normal displacement reactions, reactivity plays a large role and sometimes the reaction doesn't even happen So is there anything limiting double displacement reactions? For example $\\ce{2KI + P
  • What is the solubility trend of alkaline earth metal fluorides?
    I was going through JD Lee and I found certain contradictory statements First: With most compounds, on descending the group, the hydration energy decreases more rapidly than the lattice energy: hence the compounds become less soluble as the metal gets larger





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