A student trying to determine if a white solid is a true hydrate heats the sample and finds that there is evolution of water, that the residue obtained is soluble in water and that the solution is coloriess. Is this a true hydrate? Explain.

In CHEM 160, you learned that AgBr does not dissolve in water.  Why is that?  (Choose the best answer.) Group of answer choices A:It is possible to separate the Ag+ and Br- ions in water under reasonable conditions but this step requires more energy than what is released by the solvation of these ions by H2O molecules. B:We lied in CHEM 160 - AgBr is actually very soluble in water. C:It is possible to separate the Ag+ and Br- ions in water under reasonable conditions and this step requires less energy than what is released by the solvation of these ions by H2O molecules. D:Separating the Ag+ and Br- ions to an appreciable extent in water requires to much energy to accomplish under reasonable conditions. Consider this picture depicting the hydration of an atom or ion by water molecules.  Of the choices below, what is the only atom or ion that the yellow particle in the center can be?   Group of answer choices A:K+ ion B:oxygen atom in ethanol (CH3CH2OH) C:Cl-…

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ing and lea x t/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References] A molecule or ion that donates the hydrogen in a hydrogen bond is a hydrogen bond donor A molecule or ion that binds to this hydrogen is a hydrogen bond acceptor. Specify the hydrogen bonding behavior of the 4 species below by selecting: donor for species that act as donors only acceptor for species that act as acceptors only both for species that act as both donors and acceptors neither for species that act neither as donors nor as acceptors. H2N CH3 Hydrogen bonding behavior both CH3 H3C Hydrogen bonding behavior neither H3C. Hydrogen bonding behavior CH3 H3C. CH3 Hydrogen bonding behavior +

All three compounds are slightly soluble in water. For each compound determine the following: PbS Ksp = 8.4 x 10-28 | PbS04 Ksp = 1.8 x 10-8 Pb(103)2 Ksp = 2.6 x 10-13 a) Which compound would be the most (least) soluble and how do you know? b) Determine the solubility in moles/L for Pb(103)2. c) Calculate the number of grams of Pb(I03)2 dissolved in 1 L of solution? d) Is there a way to decrease the concentration of Pb2+(aq) ion in a solution containing PbS04? e) Calculate the concentration in moles/L of PbS04 in a saturated solution of the salt?

Please do it both...