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What is the reaction between MgCl2 and AgNO3?
AgNO3 + MgCl2 = AgCl + Mg(NO3)2AgCl is obtained as the precipitate.- If you have learned the solubility rules, you will know that nitrates are soluble and that silver chloride is insoluble. So, let's say (B) is AgNO3 and (A) is NaCl, or KCl or even MgCl2. In all three cases a precipitate is form….OUTHER…………… If you have learned the solubility rules, you will know that nitrates are soluble and that silver chloride is insoluble. So, let's say (B) is AgNO3 and (A) is NaCl, or KCl or even MgCl2.NaCl(aq) + AgNO3(aq) ==> NaNO3(aq) + AgCl(s)KCl(aq) + AgNO3(aq) ==> KNO3(aq) + AgCl(s)MgCl2(aq) + 2AgNO3(aq) ==> Mg(NO3)2(aq) + 2AgCl(s)In all three cases a precipitate is formed.
What's the difference between acid base reactions, precipitate reactions, and redox reactions?
An acid and a base will always react to produce a salt and water. A salt is composed of the positive ion from the base, and the negative ion from the acid.A redox reaction, short for oxidation-reduction reaction always involves the change in oxidation state of two elements. All single replacement reactions are redox reactions. Some synthesis and decomposition reactions can also be redox reactions.Precipitation Reactions occur when cations and anions of aqueous solutions combine to form an insoluble ionic solid, called a precipitate. Whether or not such a reaction occurs can be determined by using the solubility rules for common ionic solids. Since not all aqueous reactions form precipitates, one must consult the solubility rules before determining the state of the products and writing a net ionic equation. Being able to predict these reactions allows scientists to calculate what ions are present in a solution, and allows industries to form chemicals by extracting certain elements from these reactions.Precipitation Reactions
How does each solubility rule actually work?
The solubility rules are basically a set of statements that will help guide you determine which substances are soluble, and to what extent.There are various effects of solubility on reactions. It depends on the solubility of a solute, there are three possible results: 1) if the solution has less solute than the maximum amount that it is able to dissolve (its solubility), it is a dilute solution; 2) if the amount of solute is exactly the same amount as its solubility, it is saturated; 3) if there is more solute than is able to be dissolved, the excess solute separates from the solution. If this separation process includes crystallization, it forms a precipitate. Precipitation lowers the concentration of the solute to the saturation in order to increase the stability of the solution.Solubility RulesThe following are the solubility rules for common ionic solids. If there two rules appear to contradict each other, the preceding rule takes precedence.Salts containing Group I elements (Li+, Na+, K+, Cs+, Rb+) are soluble . There are few exceptions to this rule. Salts containing the ammonium ion (NH4+) are also soluble.Salts containing nitrate ion (NO3-) are generally soluble.Salts containing Cl -, Br -, or I - are generally soluble. Important exceptions to this rule are halide salts of Ag+, Pb2+, and (Hg2)2+. Thus, AgCl, PbBr2, and Hg2Cl2 are insoluble.Most silver salts are insoluble. AgNO3 and Ag(C2H3O2) are common soluble salts of silver; virtually all others are insoluble.Most sulfate salts are soluble. Important exceptions to this rule include CaSO4, BaSO4, PbSO4, Ag2SO4 and SrSO4 .Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al3+ are insoluble. Thus, Fe(OH)3, Al(OH)3, Co(OH)2 are not soluble.Most sulfides of transition metals are highly insoluble, including CdS, FeS, ZnS, and Ag2S. Arsenic, antimony, bismuth, and lead sulfides are also insoluble.Carbonates are frequently insoluble. Group II carbonates (CaCO3, SrCO3, and BaCO3) are insoluble, as are FeCO3 and PbCO3.Chromates are frequently insoluble. Examples include PbCrO4 and BaCrO4.Phosphates such as Ca3(PO4)2 and Ag3PO4 are frequently insoluble.Fluorides such as BaF2, MgF2, and PbF2 are frequently insoluble.
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