Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Cadmium sulfate: Difference between pages

{{Chembox

| Verifiedfields = changed

| Watchedfields = changed

| verifiedrevid = 476999882

| Name = Cadmium sulfate

| ImageFile = CdSO4(H2O).jpg

| ImageName = Cadmium sulfate

| IUPACName = Cadmium(II) sulfate

| OtherNames = Sulfuric acid, cadmium salt (1:1),

|Section1={{Chembox Identifiers

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo2_Ref = {{cascite|changed|??}}

| CASNo2 = 7790-84-3

| CASNo2_Comment = (octahydrate)

| CASNo3_Ref = {{cascite|changed|??}}

| CASNo3 = 13477-21-9

| CASNo3_Comment = (tetrahydrate)

| PubChem = 24962

| PubChem_Comment = (anhydrous)

| PubChem3 = 16211218

| PubChem3_Comment = (octahydrate)

| PubChem1 = 23618914

| PubChem1_Comment = (tetrahydrate)

| ChEBI3 = 86157

| ChEBI3_Comment = (octahydrate)

| Gmelin = 8295

|Section2={{Chembox Properties

| Formula = CdSO₄ <br> CdSO₄·H₂O (monohydrate) <br> 3CdSO₄·8H₂O (octahydrate)

| MolarMass = 208.47 g/mol (anhydrous) <br> 226.490 g/mol (monohydrate) <br> 769.546 g/mol (octahydrate)

| Appearance = White [[hygroscopic]] solid

| Odor = odorless

| Density = 4.691 g/cm³ (anhydrous) <br> 3.79 g/cm³ (monohydrate) <br> 3.08 g/cm³ (octahydrate)<ref>{{RubberBible87th}}</ref>

| Solubility = ''anhydrous:'' <br> 75 g/100 mL (0 °C) <br> 76.4 g/100 mL (25 °C) <br> 58.4 g/100 mL (99 °C) <hr> ''monohydrate:'' <br> 76.7 g/100 mL (25 °C) <hr> ''octahydrate:'' <br> very soluble

| SolubleOther = slightly soluble in [[methanol]], [[ethyl acetate]] <br> insoluble in [[ethanol]]

| MeltingPtC = 1000

| MeltingPt_notes = (anhydrous) <br> 105 °C (monohydrate) <br> 40 °C (octahydrate)

| BoilingPt = (decomposes to basic sulfate and then oxide)

| pKa =

| pKb =

| Viscosity =

| RefractIndex = 1.565

| MagSus = -59.2·10⁻⁶ cm³/mol

|Section3={{Chembox Structure

| MolShape =

| Coordination =

| CrystalStruct = orthorhombic (anhydrous) <br> monoclinic (hepta & octahydrate)

| Dipole =

|Section4={{Chembox Thermochemistry

| DeltaHf = −935&nbsp;kJ·mol⁻¹<ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A21}}</ref>

| Entropy = 123&nbsp;J·mol⁻¹·K⁻¹<ref name=b1 />

|Section7={{Chembox Hazards

| ExternalSDS =[https://web.archive.org/web/20080907181930/https://www.vinquiry.com/pdf/MSDS/CADMIUMSULFATE.pdf]

| NFPA-H = 3

| NFPA-F = 1

| NFPA-R = 0

| GHSPictograms = {{GHS06}}{{GHS08}}{{GHS09}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|301|330|340|350|360|372|410}}

| PPhrases = {{P-phrases|201|202|260|264|270|271|273|281|284|301+310|304+340|308+313|310|314|320|321|330|391|403+233|405|501}}

| LD50 = 280 mg/kg (oral, rat)

| REL = Ca<ref name=PGCH>{{PGCH|0087}}</ref>

| PEL = [1910.1027] TWA 0.005 mg/m³ (as Cd)<ref name=PGCH/>

| IDLH = Ca [9 mg/m³ (as Cd)]<ref name=PGCH/>

|Section8={{Chembox Related

| OtherAnions = [[Cadmium acetate]],<br/>[[Cadmium chloride]],<br/>[[Cadmium nitrate]]

| OtherCations = [[Zinc sulfate]],<br/>[[Calcium sulfate]],<br/>[[Magnesium sulfate]]

'''Cadmium sulfate''' is the name of a series of related [[inorganic compound]]s with the [[chemical formula|formula]] CdSO₄·{{mvar|x}}H₂O. The most common form is the monohydrate CdSO₄·H₂O, but two other forms are known CdSO₄·{{frac|8|3}}H₂O and the [[anhydrous]] salt (CdSO₄). All salts are colourless and highly soluble in water.

==Structure, preparation, and occurrence==

[[File:EntryWithCollCode100316.png|thumb|left|Portion of structure of CdSO4 illustrating the distorted tetrahedral geometry at Cd (dark blue spheres).<ref>{{cite journal |doi=10.1524/zkri.1980.0011|title=A Reinvestigation of the Crystal Structures of HgSO₄ and CdSO₄|journal=Zeitschrift für Kristallographie - Crystalline Materials|year=1980|volume=153|issue=1–2|pages=121–129|bibcode=1980ZK....153..121A|last1=Aurivillius|first1=Karin|last2=Stålhandske|first2=Claes}}</ref>]]

[[X-ray crystallography]] shows that CdSO₄·H₂O is a typical coordination polymer. Each Cd²⁺ center has [[octahedral coordination geometry]], being surrounded by four oxygen centers provided by four sulfate ligands and two oxygen centers from the [[bridging ligand|bridging]] water [[ligand]]s.<ref>{{cite journal|author1=Theppitak, C. |author2=Chainok, K. |title=Crystal Structure of CdSO₄(H₂O): A Redetermination" |journal=Acta Crystallographica Section E|year=2015|volume=71|issue=10 |pages=i8–pi9|doi=10.1107/S2056989015016904|pmid=26594423 |pmc=4647421 }}</ref>

Cadmium sulfate hydrate can be prepared by the reaction of cadmium metal or its oxide or hydroxide with dilute sulfuric acid:

:{{chem2 | CdO + H2SO4 -> CdSO4 + H2O }}

:{{chem2 | Cd + H2SO4 -> CdSO4 + H2 }}

The anhydrous material can be prepared using [[sodium persulfate]]:{{cn|date=January 2022}}

:{{chem2 | Cd + Na2S2O8 -> CdSO4 + Na2SO4 }}

Cadmium sulfates occur as the following rare minerals drobecite (CdSO₄·4H₂O), voudourisite (monohydrate), and lazaridisite (the 8/3-hydrate).

==Applications==

Cadmium sulfate is used widely for the electroplating of cadmium in electronic circuits. It is also a precursor to cadmium-based pigment such as [[cadmium sulfide]]. It is also used for [[electrolyte]] in a [[Weston standard cell]] as well as a [[pigment]] in fluorescent screens.

==References==

<references/>

{{Cadmium compounds}}

{{Sulfates}}

[[Category:Cadmium compounds]]

[[Category:Sulfates]]