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Cobalt chloride solubility1/6/2024 ![]() ![]() Box 9300, Portland, ME 04101-9300, USA Department of Applied Medical Science, University of Southern Maine, 96 Falmouth St., P.O. Box 9300, Portland, ME 04101-9300, USA Maine Center for Environmental Toxicology and Health, University of Southern Maine, 96 Falmouth St., P.O. 4 Wise Laboratory of Environmental and Genetic Toxicology, University of Southern Maine, 96 Falmouth St., P.O.3 Department of Environmental Health Sciences, Yale School of Public Health, New Haven, CT, USA.2 Department of Chemical & Biological Engineering, University of Maine, Orono, ME, USA.1 Wise Laboratory of Environmental and Genetic Toxicology, University of Southern Maine, 96 Falmouth St., P.O.The second product, Na 2CrO 4, also adheres to Rule #1, which states that salts of alkali metals tend to be soluble.īecause both products are soluble, no precipitate form as a result of this reaction. Therefore, this compound will not contribute to any precipitation being formed. Although Rule #5 says that hydroxides tend to be insoluble, Rule #1 states that salts of alkali metal cations tend to be soluble, and Rule #1 precedes Rule #5. The first product, KOH, is an example of two rules contradicting each other. Predict if a precipitate will form as a result of this reaction:Ĭonsider again the products of the reaction: if either is insoluble, a precipitate will form. Therefore, because of this compound, a precipitate will form in the course of this reaction.ĥ. According to Rule #5, that sulfides tend to be insoluble. A precipitate of this compound will not form. The products of the reaction must be examined if either of the substances formed in the reaction is insoluble, a precipitate will form.Ĭonsidering NaNO 3, Rule #3 states that nitrates tend to be soluble. Predict whether a precipitate will form as a result of this reaction: Because Rule #3 precedes Rule #4, the compound is insoluble and will form a precipitate.Ĥ. Rule #4 states that bromides are usually soluble, but Rule #3 states that salts of silver are insoluble. Letters a and c are both likely to form precipitates.Ĭoncerning a) CaSO 4, although sulfates tend to be soluble, Rule #5 indicates that calcium sulfate is an important exception to this rule.įor b), Rule #1 indicates that table salt (NaCl) is soluble because it is a salt of an alkali metal.Ĭ) is an example of two rules contradicting each other. Which of these substances is likely to form a precipitate? Therefore, it will not form a precipitate.ģ. This is perchlorate, which according to Rule #2 is likely to be soluble. Therefore, FeCO 3 is likely to form a precipitate.Ģ. ![]() Fluorides such as BaF 2, MgF 2, and PbF 2 are frequently insoluble.Īccording to Rule #5, carbonates tend to be insoluble.Phosphates such as Ca 3(PO 4) 2 and Ag 3PO 4 are frequently insoluble.Group II carbonates (CaCO 3, SrCO 3, and BaCO 3) are insoluble, as are FeCO 3 and PbCO 3. Arsenic, antimony, bismuth, and lead sulfides are also insoluble. Most sulfides of transition metals are highly insoluble, including CdS, FeS, ZnS, and Ag 2S.Thus, Fe(OH) 3, Al(OH) 3, Co(OH) 2 are not soluble. Hydroxide salts of transition metals and Al 3 + are insoluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of Group I elements are soluble. Most hydroxide salts are only slightly soluble.Important exceptions to this rule include CaSO 4, BaSO 4, PbSO 4, Ag 2SO 4 and SrSO 4. AgNO 3 and Ag(C 2H 3O 2) are common soluble salts of silver virtually all others are insoluble. Thus, AgCl, PbBr 2, and Hg 2Cl 2 are insoluble. Important exceptions to this rule are halide salts of Ag +, Pb 2 +, and (Hg 2) 2+. Salts containing Cl -, Br -, or I - are generally soluble.Salts containing nitrate ion (NO 3 -) are generally soluble.Salts containing the ammonium ion (NH 4 +) are also soluble. Salts containing Group I elements (Li +, Na +, K +, Cs +, Rb +) are soluble.If there two rules appear to contradict each other, the preceding rule takes precedence. The following are the solubility rules for common ionic solids. ![]()
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