explain what a precipitate is and how it is formed based on solubility principle and how can be separated.
Precipitation
Precipitation reactions occur when cations and anions in aqueous solution 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. Because 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. The ability to predict these reactions allows scientists to determine which ions are present in a solution, and allows industries to form chemicals by extracting components from these reactions.
Properties of Precipitates
Precipitates are insoluble ionic solid products of a reaction, formed when certain cations and anions combine in an aqueous solution. The determining factors of the formation of a precipitate can vary. Some reactions depend on temperature, such as solutions used for buffers, whereas others are dependent only on solution concentration. The solids produced in precipitate reactions are crystalline solids, and can be suspended throughout the liquid or fall to the bottom of the solution. The remaining fluid is called supernatant liquid. The two components of the mixture (precipitate and supernate) can be separated by various methods, such as filtration, centrifuging, or decanting.
SOLUBILITY RULES
Whether or not a reaction forms a precipitate is dictated by the solubility rules. These rules provide guidelines that tell which ions form solids and which remain in their ionic form in aqueous solution. The rules are to be followed from the top down, meaning that if something is insoluble (or soluble) due to rule 1, it has precedence over a higher-numbered rule.
there are three possible conditions for an aqueous solution of an ionic solid:
Q < Ksp. The solution is unsaturated, and more of the ionic
solid, if available, will dissolve.
Q = Ksp. The solution is saturated and at equilibrium.
Q > Ksp. The solution is supersaturated, and ionic
solid will precipitate.
(The ion product (Q) of a salt is the product of the concentrations of the ions in solution raised to the same powers as in the solubility product expression. It is analogous to the reaction quotient (Q) discussed for gaseous equilibria. Whereas Ksp describes equilibrium concentrations, the ion product describes concentrations that are not necessarily equilibrium concentrations.
An ion product can in principle have any positive value, depending on the concentrations of the ions involved. Only in the special case when its value is identical with Ks does it become the solubility product. A solution in which this is the case is said to be saturated)
explain what a precipitate is and how it is formed based on solubility principle and how...
Based on the solubility rules which precipitate should form from this unbalanced equation? . Fe(NO3)3 + NalO 3 - ? A. Fe(103)3 B. FelO3 C. NaNO3 D. FeNaz ОА OB OD Based on the solubility rules which precipitate should form from this unbalanced equation? Cu(NO3)2 + Na2CO3 -? A. NaNO3 B. CuCO3 B. Cucos C. Cu2CO3 Di D. No precipitate forms OB OA oc OD Based on the solubility rules which precipitate should form from this unbalanced equation? AgNO3 +...
Solutions of AgNO3 and KCl are combined and 0.683 g of a precipitate are formed. What is the precipitate and how many moles were formed?
16.51. How can we predict if a precipitate is formed when two dissolutions are mixed?
Explain in terms of ion concentrations and Ksp why a precipitate forms for some solutions. When ammonia is added to a solution that has Cu(OH)2(s) precipitate in it, the precipitate dissolves. Use Le Châtelier’s principle to explain this. Based on your observations, when a colour change occurs but no phase change occurs, what kind of reaction might have occurred?
not sure how answer this question or even begin
Practice Problems with Solubility in Acidic or Complexing Solutions 1. Like we do with our titrations, sometimes it's worthwhile to consider a stoichiometric reaction before dealing with an equilibrium in solubility problems also! For example, if you mix together 10.00 mL of 0.100 M AgNO3 and 10.00 mL of 0.100 M K CrO4... a. What precipitates, and how many grams of that precipitate are made? b. What are the concentrations of...
Question 6 of 6 How can you tell if a precipitate has formed in solution? The color of the liquid will change. The solution will become cloudy. Bubbles will form in the solution. The solution will become transparent.
B. Solubility Equilibrium; Finding a Value for Ksp 2. Explain why PbCl 2 did not precipitate immediately on addition of HCl. What conditions must be met by [Pb2 + ] and [Cl- ] if PbCl 2 is to form? 3. Explain your observations in Steps 3 (The amount of precipitate begins to decrease as it dissolves in the hot water.) and 4 (The precipitate reappears, forming after the test tube was put in ice water.) of the procedure. In which...
Solubility Rules TABLE 1: SOLUBILITY RULES FOR CATIONS Precipitating agent lons that will form a precipitate Cl", Br", Agt, Pb2+, and Hg22 Ca2+, Sr2+, Ba2+, Agt, and Pb2+ All metal ions (with widely varying Ksp values) except Li, Na+, K+, and NHA All metal ions except Lit, Na, K, NH4+, Ca?, Srl, and Ba? CO32- All metal ions except Lit, Na, K, and NHA PO43- All metal ions except Lit, Na, K, and NH4 50,2- OH S2- Pre-Lab Questions 1....
What types of observations would indicate to you that a chemical reaction occurred 3ooo 2. Two substances are mixed and a precipitate forms. How could you decide which one of the products is the precipitate? (Remember, a precipitate is an insoluble solid formed in a reaction.) Would a low solubility value or a high solubility value be associated with the substance that formed the precipitate? 3. Is the solution resulting from a "neutralization" reaction the same as pure water? Explain:
Trial Temperature (C) Precipitate formed (Y/N) 1 0 Y 2 10 Y 3 25 Y 4 45 N 5 60 N Table 2. Température effect on calcium oxalate solubility Question 1: What would be a reasonable research hypothesis for this experiment? Question 2: Based on the results from Table 2, what is the temperature effect on calcium oxalate solubility? Question 3: Based on the results from Table 2, would calcium oxalate be soluble at 20 C? What about 50 C?...