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Sr( oh) 2 soluble or insoluble

Continue The question is: Is sr (OH)2 ( hydroxy) soluble or insoluble in ? Answer: Sr(OH)2 (Strontium ) soluble in water What is soluble and insoluble? Solubility is a property of a solid, liquid or gas-eating chemical called soluble solvent in solid, liquid or gas-vulnerable solvents. The soluble of the substance depends on the physical and chemical properties of the solvent, as well as on the temperature, pressure and pH of the solution. The degree of solubility of the substance in a particular solvent is measured as the concentration of saturation, in which the addition of the solution does not increase the concentration of the solution and begins to precipitate the excess amount of the solution. The soluble of the substance is completely different from the speed of the solution, which is how quickly it dissolves. Insoluble Term insoluble often applied to bad or very poorly soluble compounds. The overall threshold for describing something as insoluble is less than 0.1 grams per 100 ml of solvent. Soluble List KClO3 ( Potassium chlorate ) KNO3 ( Potassium nitrate ) K2CO3 ( Potassium carbonate ) LiNO3 ( Lithium nitrate ) MgBr2 ( Magnesium bromide ) NaI ( Sodium iodide ) KC2H3O2 ( potassium acetate ) FeSO4 ( Iron(II) sulfate ) CuSO4 ( Copper sulfate ) Na2S ( sodium ) Na3PO4 ( Trisodium phosphate ) RbCl ( Rubidium chloride ) BaBr2 ( Barium bromide ) AlCl3 ( chloride ) HNO3 ( Nitric ) FeCl2 ( Iron dichloride ) BaI2 ( Barium iodide ) MnCl2 ( Manganous chloride ) AgClO3 ( chlorate ) CoBr2 ( Cobalt bromide ) K2S ( Potassium sulfide ) CuCl2 ( Copper chloride ) K3PO4 ( Potassium phosphate ) KI ( Potassium iodide ) (NH4)2SO4 ( AMMONIUM SULFATE ) Na2CO3 ( Sodium carbonate ) CaBr2 ( Calcium bromide ) Li3PO4 NH4NO3 ( Ammonium nitrate ) HgCl2 ( Mercury(II) chloride ) BaCl2 ( Barium chloride ) NaSO4 ( Sodium sulfate ) HCl ( ) AgC2H3O2 ( Silver acetate ) pb(c2h3o2)2 ( Lead(II) acetate ) KSO4 Li2CO3 ( Lithium carbonate ) Li2S ( Lithium sulfide ) Hg2SO4 ( MERCUROUS SULFATE ) Pb(NO3)2 ( Lead dinitrate ) NH4Cl ( AMMONIUM CHLORIDE ) NH4OH ( ammonium hydroxide ) ZnSO4 ( Zinc sulfate ) CaCrO4 ( CALCIUM CHROMATE ) CsOH ( Cesium hydroxide ) (NH4)3PO4 ( Ammonium phosphate ) LiOH ( ) BaS ( ) K2SO4 ( POTASSIUM SULFATE ) Na2SO4 ( Sodium sulfate ) NiCl2 (NICKEL CHLORIDE ) NiBr2 (NICKEL BROMIDE) MgSO4 (magnesium sulfate) NH4I (Ammonium iodide) HgCl2 (MERCURIC CHLORIDE ) MgCl2 (Magnesium Chloride) H2SO4 (Sulphuric Acid) CaCl2 (Calcium Chloride) BaF2 fluoride ) Na3PO4 (sodium phosphate ) Cu (NO3)2 (Copper (II) nitrate ) AgNO3 ( ) MgC2O4 (magnesium oxalate) KCl (potassium chloride) Al2,SO4)3 (Aluminum sulfate) Ca (NO3) 2 ( nitrate ) MgS ( ) NaNO3 () NiI2 (Nickel (II) iodide) (NH4)2CO3 (AMMONIUM CARBONATE ) HCN (hydrogen cyanide) NaBr (sodium bromide ) NH4Br (AMMONIUM BROMIDE) AlCl3 (aluminium chloride) SrS () FeCl3 (iron (III) chloride ) LiBr (lithium bromide) KOH () )nBr2 (zinc bromide) NH3 (ammonia ) NaOH () CuBr2 (Copper (II) bromide) Fe (NO3)2 (iron (II) Nithrat ) nahco3 (sodium bicarbonate) CaSO4 (calcium sulfate) NaCl (sodium chloride) KBr (potassium bromide) (NH4)2S (ammonium sulfide ) LiCl (lithium chloride) nCl2 (zinc chloride) Ba(OH)2 () CoCl2 (Cobalt Chloride (II) Ba (NO3)2 (Barium Nitrate) AgClO4 (Silver ) Mg (NO3)2 (NITRATE) NO3) 2 (Zinc Nitrate) Senior (OH)2 (Hydroxynd Strontium) Fe (NO3)3 (Iron Nitrate (III) NaC2H3O2 (sodium acetate) Ba (ClO4)2 (BARARIUM PERCHLORATE ) HgSO4 (Mercury (II) sulfate ) Ca (C2H3O2)2 C4H6O4Ba (Barium acetate) K2O (potassium oxide) NaClO (sodium hypochloro) CuCl (Copper (I) chloride ) Senior (NO3)2 (Nitrate Strontium) Cu (C2H3O2)2 kclo4 (POTASSIUM PERCHLORATE) NaClO4 (Sodium Perchlorate) NaClO3 ( ) C4H6O4Ca (Calcium acetate) ung (CH3COO)2 (zinc acetate) CH3OH (methanol) Ba,C2H3O2)2 Al (NO3)) 3 (NO3)) aluminium nitrate) K2SO3 (potassium sulfite) H3PO4 (phosphoric acid) MnI2 (manganese (II) iodide ) CoSO4 CsCl Ca (ClO4)2 MgI2 (magnesium iodine NI (NO3)2 (Nickel (II) nitrate) Cu (CH3COO)2 (Copper (II) Acetate ) C12H22O11 (Sucrose) Cr (NO3)2 NiSO4 (Nickel (II) sulfate ) aluminium acetate NH4C2H3O2 NaPO4 Iron (III) Acetate H2SO3 (Sulphuric acid) Co (NO3)2 (Cobalt (II) nitrate ) Mn (NO3)2 (Manganese , II) Nitrate) Li2SO4 (Lithium-sulfate ) SO2 (Sulfur dioxide ) AlBr3 (ALUMINUM BROMID) C2H7NO2 (Ammonium Acetate) Na2SO3 (Sodium sulfite) NonI22 (zinc iodide) HClO4 () HBr (hydrogen bromide) CaI2 (Calcium iodide) Insoluble list Ag2CO3 (Silver Carbonate ) Hg2I2 (Mercury (I) iodide) CuCO3 (Copper Carbonate) BaCO3 (Carbonate Baria) AgOH (Silver Hydroxide) Fe2S3 (Iron Sulfide (III) ) MgCO3 (Magnesium Carbonate) Ag2O () CuS (Copper (II) sulf ) Hg2Cl2 (Mercury (I) chloride ) AgCO3 (Silver carbonate ) PbCl2 (Lead dichloride ) PbI2 (Lead (II) iodide ) Cu (OH)2 (Copper (II) hydroxide) AgCl2 () AgCl (Silver Chloride) Ag3PO4 (Silver Phosphate) Cu3(PO4)2 (Copper (II) phosphate ) FePO4 (iron (III) phosphate ) NiCO3 (Nickel (II) carbonate) SrCO3 (Carbonate strontium) Ag2S (Silver Sulphide) (LEAD CHROMATE) PbF2 (Lead fluoride) Fe (OH)3 (Ferric hydroxid) Fe2O3 (Iron oxide (III) PbS (Lead (II) sulfide) PbSO4 (Lead (II) sulfate) Ca3 (PO4)2 (calcium phosphate) Ba3(PO4)2 ( barium phosphate ) PbI ( Lead(II) iodide ) HgI2 ( Mercury diiodide ) Hg2Br2 ( Mercury(I) bromide ) Al2S3 ( Aluminium sulfide ) Ag2CrO4 ( Silver chromate ) Pb(OH)2 ( Lead(II) hydroxide ) Cu(OH)2 ( Copper(II) hydroxide ) Li3PO4 ( Lithium Phosphate ) SrSO4 ( Strontium sulfate ) AgBr ( ) MgO ( MAGNESIUM OXIDE ) Zn(OH)2 ( ) PbBr2 ( Lead(II) Bromide ) ZnCO3 ( ZINC CARBONATE ) Zn3(PO4)2 ( Zinc Phosphate ) Mg(C2H3O2)2 FeS ( Iron(II) sulfide ) CaCO3 ( Calcium carbonate ) Mg(OH)2 ( ) Mg3(PO4)2 ( Magnesium Phosphate ) AgI ( ) FeCO3 ( Iron(II) carbonate ) Ag2SO4 ( ) ZnS ( ) Al(OH)3 ( Aluminium hydroxide ) PbCO3 ( Lead carbonate ) AgSO4 ( silver(II) sulfate ) Fe(OH)2 ( Iron(II) hydroxide ) NiS ( ) CdCO3 ( CARBONATE ) Mn(OH)2 ( Manganese hydroxide ) CoCO3 ( Cobalt(II) carbonate ) Ni(OH)2 ( Nickel(II) hydroxide ) BaCrO4 ( Barium chromate ) CoS ( cobalt(ii) sulfide ) Co(OH)2 ( Cobalt(II) hydroxide ) FeO(OH) ( Iron(III) hydroxide ) CuCrO4 ( Copper(II) chromate ) Cd(OH)2 ( Cadmium hydroxide ) CaF2 (calcium fluoride) Cr2S3 Pb3 (PO4)2 CaC2O4 MnCO3 (Manganese (II) carbonate) HC2H3O2 low soible (Slightly soluble) Ca (soluble) Ca (I) OH)2 ( ) CaS ( ) PbCl2 (Lead dichloride) H2CO3 (Carbon acid) H2S () We get responses from resources www.quora.com answers.yahoo.com answers.com www.quia.com quizlet.com www.reference.com socratic.org pubchem.ncbi.nlm.nih.gov If the answer is wrong. Please comment below or contact us. The question is: Is sr (OH)2 (strontium hydroxy) soluble or insoluble in water? Answer: Sr(OH)2 (Strontium Hydroxide) soluble in water-soluble or insoluble This is a list of solubility rules for solids in water. Solubility is the result of interaction between polar water molecules and that make up the crystal. Two forces determine the degree to which the decision will occur: This force tends to bring ions into the solution. If this is the predominant factor, the compound can be very soluble in water. This force tends to keep the ions in a solid state. When this is the main factor, then the water solubility can be very low. However, it is not easy to estimate the relative magnitude of these two forces or quantify such electrolytes water. Therefore, it is easier to refer to a set of generalizations, sometimes called solubility rules, which is based on experiments. It is a good idea to memorize the information in this table. All elements of Group I (alkaline metals - Na, Li, K, Cs, Rb) are soluble. NO3: All nitrates are soluble. chlorate (ClO3-), perchlorate (ClO4-), acetate (CH3COO- or C2H3O2-, as oac-) salts are soluble. Cl, Br, I: All chlorides, bromides and iodides are soluble, except for silver, mercury and lead (e.g. AgCl, Hg2Cl2 and PbCl2). SO42: Most sulfates are soluble. The exceptions are BaSO4, PbSO4 and SrSO4. CO32: All carbonates are insoluble, with the exception of NH4 and Group 1 elements. OK: All are insoluble, with the exception of Group 1, Ba (OH)2 and Sr (OH)2. Ca(OH)2 lightly soluble. S2: All are insoluble, with the exception of Group 1 and Group 2 and NH4. So do some solids dissolve in water? Sugar, which we use to sweeten coffee or tea, is a molecular solid in which individual molecules are together by relatively weak intermolecular forces. When sugar dissolves in water, weak bonds between individual sucrose molecules break down, and these C12H22O11 molecules are released into the solution. Energy is required to break the bonds between the C12H22O11 molecules in sucrose. It also takes energy to break the hydrogen bonds in the water, which must be broken to insert one of these sucrose molecules into the solution. Sugar dissolves in water because energy is given when slightly polar sucrose molecules form intermolecular bonds with polar water molecules. Weak bonds, which are formed between solvent and solvent, compensate for the energy needed to disrupt the structure of both pure solvent and solvent. In the case of sugar and water, this process works so well that up to 1,800 grams of sucrose can dissolve in a liter of water. Ion solids (or salts) contain positive and negative ions, which are held together by a strong force of attraction between particles with opposite charges. When one of these solids dissolves in water, the ions that form solid are released into the solution, where they become associated with the molecules of the polar solvent. H2O NaCl (s) Nak (aq) - Cl- (aq) We can generally assume that salts are separated into their ions when they dissolve in water. Ion compounds dissolve in water if the energy released when the ions interact with water molecules compensates for the energy needed to break the ion bonds in the solid, and the energy needed to release water molecules so that the ions can be inserted into the solution. Solubility Equilibria Discussions of equilibria soluble are based on the following assumption: When solids dissolve in water, they are separated to give elementary particles from which they are formed. Thus, molecular solids are separated to give individual molecules H2O C12H22O11 (s) C12H22O11 (aq) and ion solids are separated to give solutions to the positive and negative ions they contain. H2O NaCl (s) Nak (aq) - Cl- (aq) When salt is first added, it is fast and split up. Thus, the conductivity of the solution at first glance increases rapidly. dissolve NaCl (s) Naz (aq) (aq) of these ions soon become large enough that the backlash begins to compete with the forward reaction, leading to a decrease in the speed with which Naz and Cl- ions enter the solution. Associated Nak (aq) - Cl- (aq) NaCl (s) precipitation Eventually, the concentrations of Naz and Cl- ion become large enough that the rate at which precipitation occurs accurately balances the speed at which NaCl dissolves. Once this happens, there is no change in the concentration of these ions over time, and the reaction is in balance. When this system achieves equilibrium, it is called a saturated solution because it contains a maximum concentration of ions that can exist in balance with solid salt. The amount of salt that should be added to this volume of solvent to form a saturated solution is called salt solubility. The rules of solubility there are a number of patterns in the data derived from measuring the solubility of different salts. These models form the basis for the rules outlined in the table below, which can guide predictions of whether the salt will dissolve in water. These rules are based on the following definitions of terms soluble, intractable and slightly soluble. Salt dissolves if dissolved in water to give a solution with a concentration of at least 0.1 moles per liter at room temperature. Salt is insoluble if the concentration of amovable solution is less than 0.001 M at room temperature. Slightly soluble salts give solutions that fall between these extremes. Rules of ion ion ion compounds in water-soluble salts 1. Ions Naz, CK and NH4 form soluble salts. Thus, NaCl, KNO3, (NH4)2SO4, Na2S and (NH4)2CO3 are soluble. 2. Nitrate (NO3-) ion forms soluble salts. Thus, Cu (NO3)2 and Fe (NO3)3 are soluble. 3. Chloride (Cl-), bromide (Br-), and iodide ion (I-) usually form soluble salts. The exceptions to this rule are the salts of Pb2, Hg22, Ag and Cu ions. NonCl2 is soluble, but CuBr is not. 4. Ion sulfate (SO42-) usually forms soluble salts. Exceptions include BaSO4, SrSO4 and PbSO4, which are intractable, and Ag2SO4, CaSO4 and Hg2SO4, which are slightly soluble. Insoluble salts 1. Sulfides (S2-) are usually insoluble. Exceptions include Na2S, K2S, (NH4)2S, MgS, CaS, SrS and BaS. 2. Oxides (O2-) are usually insoluble. Exceptions include Na2O, K2O, SrO and BaO, which are soluble, and Cao, which is slightly soluble. 3. Hydroxides (OH-) are usually intractable. Exceptions include NaOH, KOH, Sr(OH)2 and Ba (OH)2, which are soluble, and Ca (OH)2, which is slightly soluble. 4. Chromates (CrO42-) are usually intractable. The exceptions are Na2CrO4, K2CrO4, (NH4)2CrO4 and MgCrO4. 5. Phosphates (PO43-) and carbonates (CO32-) are generally insoluble. The exceptions are the salts of the Naz, CK and NH4 ions. Ions. sr(oh)2 soluble or insoluble

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