GENERAL CHEMISTRY 103 Chapter 7 Classifying Chemical Reactions Precipitation and Acid-Base Reactions

FALL 2021 GENERAL CHEMISTRY

A precipitate forms when mixing solutions of silver nitrate (AgNO3) and sodium chloride (NaCl). Complete the net ionic equation for this reaction by filling in the blanks. Do not include charges on any ions and do not include phase symbols. The two possible products for this reaction are NaNO3 and AgCl. The solubility guidelines indicate that AgCl is insoluble. Na+ and NO3− ions are both soluble with no exceptions. It is clear that the reaction involves Ag+ ions and Cl− ions, and the product is AgCl. The balanced net ionic equation is shown below. Ag+(aq)+Cl−(aq)⟶AgCl(s)

FALL 2021 GENERAL CHEMISTRY

A precipitate forms when mixing solutions of silver nitrate (AgNO3) and sodium chloride (NaCl). Complete the net ionic equation for this reaction by filling in the blanks. Do not include charges on any ions and do not include phase symbols. Answer 1: Not quite right - check out the answer explanation. Ag+(aq)+Cl−(aq) → NaO (s) Answer 2: Not quite - review the answer explanation to help get the next one. Cl+(aq)+CO−(aq) → AgNa (s) Answer Explanation Correct answers:$Ag^+ (aq)}+Cl^-(aq) AgCl\ (s)}Ag+(aq)+Cl−(aq) → AgCl (s)​ The two possible products for this reaction are NaNO3 and AgCl. The solubility guidelines indicate that AgCl is insoluble. Na+ and NO3− ions are both soluble with no exceptions. It is clear that the reaction involves Ag+ ions and Cl− ions, and the product is AgCl. The balanced net ionic equation is shown below. Ag+(aq)+Cl−(aq)⟶AgCl(s)

Fall 2021 GENERAL CHEMISTRY 112

Al(OH)3 Mg(OH)2 Ionic compounds containing the hydroxide ion are mostly insoluble with the exception of the hydroxides of group 1 metal cations and barium hydroxide. Therefore, of the given choices, only aluminum hydroxide and magnesium hydroxide will form precipitates. Your answer: Al(OH)3

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Apply Solubility Rules Precipitation Reactions and Solubility Rules A precipitation reaction is one in which dissolved substances react to form one (or more) solid products. Many reactions of this type involve the exchange of ions between ionic compounds in aqueous solution and are sometimes referred to as double displacement, double replacement, or metathesis reactions. These reactions are common in nature and are responsible for the formation of coral reefs in ocean waters and kidney stones in animals. They are used widely in industry for production of a number of commodity and specialty chemicals. Precipitation reactions also play a central role in many chemical analysis techniques, including spot tests used to identify metal ions and gravimetric methods for determining the composition of matter (see the last module of this chapter). The extent to which a substance may be dissolved in water, or any solvent, is quantitatively expressed as its solubility, defined as the maximum concentration of a substance that can be achieved under specified conditions. Substances with relatively large solubilities are said to be soluble. A substance will precipitate when solution conditions are such that its concentration exceeds its solubility. Substances with relatively low solubilities are said to be insoluble, and these are the substances that readily precipitate from solution. More information on these important concepts is provided in a later chapter on solutions. For purposes of predicting the identities of solids formed by precipitation reactions, one may simply refer to patterns of solubility that have been observed for many ionic compounds (Table 1). Soluble Ionic Compounds contain these ionsExceptions to these solubility rules include NH4+ group 1 metal cations: Li+ Na+ K+ Rb+ Cs+ none Halides: Cl− Br− I− halide compounds of Ag+, Hg2+2, and Pb2+ F− fluoride compounds with group 2 metal cations, Pb2+ and Fe3+ C2H3O2− HCO3− NO3− ClO3− none SO42− sulfate compounds with Ag+, Ba2+, Ca2+, Hg22+, Pb2+, and Sr2+ Insoluble Ionic Compounds contain these ionsExceptions to these insolubility rules include CO32− CrO42− PO43− S2− compounds of these anions with group 1 metal cations and NH4+ OH− hydroxide compounds with group 1 metal cations and Ba2+ A vivid example of precipitation is observed when solutions of potassium iodide and lead nitrate are mixed, resulting in the formation of solid lead iodide. 2KI(aq)+Pb(NO3)2(aq)⟶PbI2(s)+2KNO3(aq) This observation is consistent with the solubility guidelines. The only insoluble compound among all those involved is lead iodide, one of the exceptions to the general solubility of iodide salts. The net ionic equation representing this reaction is: Pb2++2I−(aq)⟶PbI2(s) Lead iodide is a bright yellow solid that was formerly used as an artist's pigment known as iodine yellow (Figure 1). The properties of pure PbI2 crystals make them useful for fabrication of X-ray and gamma ray detectors. A photograph shows a beaker filled with a solution. A colored opaque precipitate can be seen suspended in the solution and collected at the bottom of the beaker. Figure 1. A precipitate of PbI2 forms when solutions containing Pb2+ and I− are mixed. (credit: Der Kreole/Wikimedia Commons) The solubility guidelines in Table 1 may be used to predict whether a precipitation reaction will occur when solutions of soluble ionic compounds are mixed together. One merely needs to identify all the ions present in the solution and then consider if possible cation/anion pairing could result in an insoluble compound. For example, mixing solutions of silver nitrate and sodium fluoride will yield a solution containing Ag+, NO3−, Na+, and F− ions. Aside from the two ionic compounds originally present in the solutions, AgNO3 and NaF, two additional ionic compounds may be derived from this collection of ions: NaNO3 and AgF. The solubility guidelines indicate all nitrate salts are soluble but that AgF is one of the exceptions to the general solubility of fluoride salts. A precipitation reaction, therefore, is predicted to occur, as described by the following equations. NaF(aq)+AgNO3(aq)Ag+(aq)+F−(aq)→AgF(s)+NaNO3(aq)→AgF(s)(molecular)(net ionic) Example: Predicting Precipitation Reactions Question: Predict the result of mixing reasonably concentrated solutions of the following ionic compounds. If precipitation is expected, write a balanced net ionic equation for the reaction. (a) potassium sulfate and barium nitrate (b) lithium chloride and silver acetate (c) lead nitrate and ammonium carbonate Solution: (a) The two possible products for this combination are KNO3 and BaSO4. The solubility guidelines indicate that BaSO4 is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is Ba2+(aq)+SO42−(aq)⟶BaSO4(s) (b) The two possible products for this combination are LiC2H3O2 and AgCl. The solubility guidelines indicate that AgCl is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is Ag+(aq)+Cl−(aq)⟶AgCl(s) (c) The two possible products for this combination are PbCO3 and NH4NO3. The solubility guidelines indicate that PbCO3 is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is Pb2+(aq)+CO32−(aq)⟶PbCO3(s)

FAL 2021 GENERAL CHEMISTRY

Carbonates are typically insoluble, but one exception would be a carbonate containing what kind of cation? Select the correct answer below ammonia transition metallic group two metalloid ammonium The ammonium ion or group one metal ions constitute the exceptions for carbonate insolubility, so of the options, ammonium carbonate will be the only water soluble compound. ammonium The ammonium ion or group one metal ions constitute the exceptions for carbonate insolubility, so of the options, ammonium carbonate will be the only water soluble compound.

FALL 2021 GENERAL CHEMISTRY

Common ionic compounds containing ions from which of the following groups are always soluble in water? the alkali metals Common ionic compounds containing alkali metal (group 1) ions are soluble in water without exception.

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How do you write a complete chemical equation? Chemical equation for a chemical reaction is written as follows: Identify the reactants and the products of the chemical reaction. Write down the formulae or symbols of the reactants only the left hand side with a sign of plus (+) between them. The formulae or symbols of the products formed in.. . https://www.bing.com/videos/search?q=HOW+DO+YOU+WRITE+NET+IONIC+EQUATION+AND+SOLV&cvid=edbe50d6ab1 Net Ionic Equations LEARNING OBJECTIVES Define spectator ion. Define net ionic equation. Write and balance net ionic equations. YES, WE NEED THE CROWD At sports events around the world, we can see a small number of athletes fiercely competing on the field. They get tired, dirty, and sometimes hurt as they try to win the game. Surrounding them are thousands of spectators watching and cheering. Would the game be different without the spectators? Yes, it definitely would. They provide encouragement to the team and generate enthusiasm. The spectators are not really playing the game. but they are certainly a part of the process. Net Ionic Equations We can write a molecular equation for the formation of silver chloride precipitate: The corresponding ionic equation is: If you look carefully at the ionic equation, you will notice that the sodium ion and the nitrate ion appear unchanged on both sides of the equation. When the two solutions are mixed, neither the Na + nor the NO 3 − ions participate in the reaction. They can be eliminated from the reaction. A spectator ion is an ion that does not take part in the chemical reaction and is found in solution both before and after the reaction. In the above reaction, the sodium ion and the nitrate ion are both spectator ions. The equation can now be written without the spectator ions. The net ionic equation is the chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction. Notice that in writing the net ionic equation, the positively-charged silver cation was written first on the reactant side, followed by the negatively-charged chloride anion. This is somewhat customary because that is the order in which the ions must be written in the silver chloride product. However, it is not absolutely necessary to order the reactants in this way. Net ionic equations must be balanced by both mass and charge. Balancing by mass means making sure that there are equal numbers of each element. Balancing by charge means making sure that the overall charge is the same on both sides of the equation. In the above equation, the overall charge is zero, or neutral, on both sides of the equation. As a general rule, if you balance the molecular equation properly, the net ionic equation will end up being balanced by both mass and charge. Sample Problem: Writing and Balancing Net Ionic Equations When aqueous solutions of copper(II) chloride and potassium phosphate are mixed, a precipitate of copper(II) phosphate is formed. Write a balanced net ionic equation for this reaction. Step 1: Plan the problem . Write and balance the molecular equation first, making sure that all formulas are correct. Then write the ionic equation, showing all aqueous substances as ions. Carry through any coefficients. Finally, eliminate spectator ions and write the net ionic equation. Step 2: Solve . Molecular equation: Ionic equation: Notice that the balancing is carried through when writing the dissociated ions. For example, there are six chloride ions on the reactant side because the coefficient of 3 is multiplied by the subscript of 2 in the copper(II) chloride formula. The spectator ions are K + and Cl − and can be eliminated. Net ionic equation: Step 3: Think about your result For a precipitation reaction, the net ionic equation always shows the two ions that come together to form the precipitate. The equation is balanced by mass and charge. SUMMARY Net ionic equations are described and an example of writing a net ionic equation is given. PRACTICE Do the practice equations at the web site below: http://www.files.chem.vt.edu/RVGS/ACT/notes/net_ionic_rxns/net_ionic_rxns.html REVIEW What does the name "spectator ion" mean? Is there a reaction if no precipitate or gas is formed in an ionic equation? What do we need to balance in net ionic equations? Glossary net ionic equation: The chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction. spectator ion: An ion that does not take part in the chemical reaction and is found in solution both before and after the reaction.

FALL 2021 GENERAL CHEMISTRY

How do you write a net ionic equation? There are three steps to writing a net ionic equation: Balance the chemical equation. Write the equation in terms of all of the ions in the solution. In other words, break all of the strong electrolytes into the ions they form in aqueous solution. In the net ionic equation, all species with (s), (l), and (g) will be unchanged. Net ionic equations are an important aspect of chemistry as they represent only the entities that change in a chemical reaction. They are most commonly used in redox reactions, double replacement reactions, and acid-base neutralizations. Net Ionic Equation Example. The net ionic equation for the reaction that results from mixing 1 M HCl and 1 M NaOH is: H +(aq) + OH -(aq) → H 2O(l) The Cl - and Na + ions do not react and are not listed in the net ionic equation. The net ionic equation: Na + + Cl - + Ag + + NO 3 - → AgCl + Na + + NO 3 -. Cl - + Ag + → AgCl -. The above net ionic equation indicates Chloride ions and silver cations are responsible for the formation of AgCl white precipitate and this does not include the remaining ions (Na + and NO 3 -). What is the full ionic equation? The full ionic equation would be: Ca 2+ + 2Cl − + 2Ag + + 2NO3 − ---> Ca2 + + 2NO3 − + 2AgCl(s) and the net ionic equation would be:2Cl −(aq) + 2Ag +(aq) --> 2AgCl(s) or, in reduced balanced form,Ag + + Cl − --> AgCl(s) What are the rules for writing an ionic equation? If no state is provided for an element, use the state found on the periodic table. If a compound is said to be a solution, you can write it as aqueous, or ( aq ). If there is water in the equation, determine whether or not the ionic compound will dissolve using a solubility table. ... If there is not water, the ionic compound is a solid ( s ). .What is an example of an ionic reaction? For example, in the reaction between silver nitrate (AgNO 3) and sodium chloride (NaCl) in water, the complete ionic equation is: Ag + (aq) + NO 3- (aq) + Na + (aq) + Cl - (aq) → AgCl (s) + Na + (aq) + NO 3- (aq) Notice the sodium cation Na + and nitrate anion NO 3- appear on both the reactants and products side of the arrow. Ion Examples With Positive & Negative Charges An ion is defined as an atom or group of atoms where the number of electrons is not equal to the number of protons. Electrons have a negative charge, whereas protons have a positive charge. When an atom gains electrons, this results in a negative charge. This type of ion is called an anion. When an atom loses electrons, this results in a positive charge. A positively charged ion is called a cation. Enjoy exploring several examples of ions of both types. Advertisement Examples of Positive Ions Positive ions are typically metals or act like metals. Many common materials contain these ions. Mercury is found in thermometers, for instance, and aluminum is a metal that is found in a surprising amount of things. It's even an ingredient in baking soda and in certain other food products! The positive charge (more protons versus electrons) for a cation is shown by a number and plus sign after the formula. If there's just a plus sign, it means the charge is plus 1. Review some examples of cations, or positive ions. aluminum Al3+ barium Ba2+ bismuth Bi3+ cadmium Cd2+ calcium Ca2+ cesium Cs+ chromium (III) Cr3+ cobalt Co2+ copper (I) Cu+ copper (II) Cu2+ hydrogen H+ iron (II) Fe2+ iron (III) Fe3+ lead (II) Pb2+ lithium Li+ magnesium Mg2+ mercury (I) Hg22+ nickel Ni2+ potassium K+ rubidium Rb+ silver Ag+ sodium Na+ strontium Sr2+ tin (II) Sn2+ zinc Zn2+ IN ORDER TO WRITE AND NET ICONIC EQUATION YOU NORMALLY, Step 1: Plan the problem . Write and balance the molecular equation first, making sure that all formulas are correct. Then write the ionic equation, showing all aqueous substances as ions. Carry through any coefficients. Finally, eliminate spectator ions and write the net ionic equation. Step 2: Solve . Which is a spectator ion in the net ionic equation? In the above reaction, the sodium ion and the nitrate ion are both spectator ions. The equation can now be written without the spectator ions. The net ionic equation is the chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction.

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LINKS: Solubility table - Wikipedia Is FeCl3 ( Iron(III) chloride ) Soluble or Insoluble in water ? (bengislife.com)

FALL 2021 GENERAL CHEMISTRY

Note: At 3:23 in the video, the net ionic reaction states that AgF precipitates as a solid; this is not correct, it is a soluble compound. LINK: https://youtu.be/Op4z-2vHpSY

FALL 2021 GENERAL CHEMISTRY

Of the following halide compounds, which is the least soluble in water Correct answer: magnesium fluoride Most ionic compounds containing halide ions are soluble in water. The only exception among the given choices is magnesium fluoride (MgF2) because fluorides of group 2 metal cations are insoluble, and magnesium is in group 2. Your answer: WHEN YOUR ANSWER IS WRONG? lithium fluoride All common lithium-containing ionic compounds are soluble. Recall that lithium is in group 1.

Fall 2021 GENERAL CHEMISTRY

Question: Is FeCl3 ( Iron(III) chloride ) Soluble or Insoluble in water ?Answer: FeCl3 ( Iron(III) chloride ) is Soluble in waterWhat is Soluble and Insoluble ?SolubilitySolubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a solid, liquid, or gaseous solvent. The solubility of a substance fundamentally depends on the physical and chemical properties of the solute and solvent as well as on temperature, pressure and the pH of the solution. The extent of the solubility of a substance in a specific solvent is measured as the saturation concentration, where adding more solute does not increase the concentration of the solution and begins to precipitate the excess amount of solute. The solubility of a substance is an entirely different property from the rate of solution, which is how fast it dissolves.https://en.wikipedia.org/wiki/SolubilityInsolubleThe term insoluble is often applied to poorly or very poorly soluble compounds. A common threshold to describe something as insoluble is less than 0.1 g per 100 mL of solvent.https://en.wikipedia.org/wiki/SolubilitySoluble ListKClO3 ( 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 sulfide )Na3PO4 ( Trisodium phosphate )RbCl ( Rubidium chloride )BaBr2 ( Barium bromide )AlCl3 ( Aluminium chloride )HNO3 ( Nitric acid )FeCl2 ( Iron dichloride )BaI2 ( Barium iodide )MnCl2 ( Manganous chloride )AgClO3 ( Silver 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 ( Hydrochloric acid )AgC2H3O2 ( Silver acetate )pb(c2h3o2)2 ( Lead(II) acetate )KSO4Li2CO3 ( 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 ( Lithium hydroxide )BaS ( Barium sulfide )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 ( Sulfuric acid )CaCl2 ( Calcium chloride )BaF2 ( Barium fluoride )Na3PO4 ( sodium phosphate )Cu(NO3)2 ( Copper(II) nitrate )AgNO3 ( Silver nitrate ) MgC2O4 ( Magnesium oxalate )KCl ( Potassium chloride )Al2(SO4)3 ( Aluminium sulfate )Ca(NO3)2 ( Calcium nitrate )MgS ( Magnesium sulfide )NaNO3 ( Sodium nitrate )NiI2 ( Nickel(II) iodide )(NH4)2CO3 ( AMMONIUM CARBONATE )HCN ( hydrogen cyanide )NaBr ( sodium bromide )NH4Br ( AMMONIUM BROMIDE )AlCl3 ( aluminum chloride )SrS ( Strontium sulfide ) FeCl3 ( Iron(III) chloride )LiBr ( Lithium bromide )KOH ( Potassium hydroxide )ZnBr2 ( Zinc bromide )NH3 ( ammonia )NaOH ( Sodium hydroxide )CuBr2 ( Copper(II) bromide )Fe(NO3)2 ( Iron(II) Nitrate )nahco3 ( Sodium bicarbonate )CaSO4 ( calcium sulfate )NaCl ( sodium chloride )KBr ( Potassium bromide )(NH4)2S ( Ammonium sulfide ) LiCl ( Lithium chloride )ZnCl2 ( Zinc chloride )Ba(OH)2 ( Barium hydroxide )CoCl2 ( Cobalt(II) chloride )Ba(NO3)2 ( Barium nitrate )AgClO4 ( Silver perchlorate )Mg(NO3)2 ( MAGNESIUM NITRATE )Zn(NO3)2 ( Zinc nitrate )Sr(OH)2 ( Strontium hydroxide )Fe(NO3)3 ( Iron(III) nitrate )NaC2H3O2 ( sodium acetate )Ba(ClO4)2 ( BARIUM PERCHLORATE )HgSO4 ( Mercury(II) sulfate )Ca(C2H3O2)2C4H6O4Ba ( Barium Acetate )K2O ( Potassium oxide )NaClO ( sodium hypochlorite )CuCl ( Copper(I) chloride )Sr(NO3)2 ( Strontium nitrate )Cu(C2H3O2)2 kclo4 ( POTASSIUM PERCHLORATE )NaClO4 ( Sodium perchlorate )NaClO3 ( SODIUM CHLORATE )C4H6O4Ca ( Calcium Acetate )Zn(CH3COO)2 ( Zinc acetate )CH3OH ( methanol )Ba(C2H3O2)2Al(NO3)3 ( aluminum nitrate )K2SO3 ( Potassium sulfite )H3PO4 ( Phosphoric acid )MnI2 ( Manganese(II) iodide )CoSO4CsClCa(ClO4)2MgI2 ( magnesium iodide )Ni(NO3)2 ( Nickel(II) nitrate )Cu(CH3COO)2 ( Copper(II) Acetate )C12H22O11 ( sucrose )Cr(NO3)2 NiSO4 ( Nickel(II) sulfate )aluminum acetateNH4C2H3O2NaPO4Iron(III) AcetateH2SO3 ( Sulfurous acid )Co(NO3)2 ( Cobalt(II) nitrate )Mn(NO3)2 ( Manganese(II) Nitrate )Li2SO4 ( Lithium sulfate )SO2 ( Sulfur dioxide )AlBr3 ( ALUMINUM BROMIDE )C2H7NO2 ( Ammonium Acetate )Na2SO3 ( Sodium sulfite )ZnI2 ( Zinc iodide )HClO4 ( Perchloric acid )HBr ( Hydrogen bromide )CaI2 ( Calcium iodide )Insoluble ListAg2CO3 ( Silver carbonate )Hg2I2 ( Mercury(I) iodide )CuCO3 ( Copper carbonate )BaCO3 ( Barium carbonate )AgOH ( Silver Hydroxide )Fe2S3 ( Iron(III) sulfide )MgCO3 ( Magnesium carbonate )Ag2O ( Silver oxide )CuS ( Copper(II) sulfide )Hg2Cl2 ( Mercury(I) chloride )AgCO3 ( Silver carbonate )PbCl2 ( Lead dichloride )PbI2 ( Lead(II) iodide )Cu(OH)2 ( Copper(II) hydroxide )AgCl2 ( Silver chloride )AgCl ( Silver chloride )Ag3PO4 ( Silver phosphate )Cu3(PO4)2 ( Copper(II) phosphate )FePO4 ( Iron(III) phosphate )NiCO3 ( Nickel(II) carbonate )SrCO3 ( Strontium carbonate )Ag2S ( Silver sulfide )AlPO4 ( Aluminum phosphate )cui2 ( copper iodide )pbcro4 ( LEAD CHROMATE )PbF2 ( Lead fluoride )Fe(OH)3 ( Ferric hydroxide )Fe2O3 ( Iron(III) oxide )PbS ( Lead(II) sulfide )PbSO4 ( Lead(II) sulfate )Ca3(PO4)2 ( calcium phosphate )BaSO4 ( Barium sulfate )hno2 ( Nitrous acid )aglBa3(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 ( silver bromide )MgO ( MAGNESIUM OXIDE )Zn(OH)2 ( zinc hydroxide )PbBr2 ( Lead(II) Bromide )ZnCO3 ( ZINC CARBONATE )Zn3(PO4)2 ( Zinc Phosphate )Mg(C2H3O2)2FeS ( Iron(II) sulfide )CaCO3 ( Calcium carbonate )Mg(OH)2 ( Magnesium hydroxide )Mg3(PO4)2 ( Magnesium Phosphate )AgI ( Silver iodide )FeCO3 ( Iron(II) carbonate )Ag2SO4 ( Silver sulfate )ZnS ( Zinc sulfide )Al(OH)3 ( Aluminium hydroxide )PbCO3 ( Lead carbonate )AgSO4 ( silver(II) sulfate )Fe(OH)2 ( Iron(II) hydroxide )NiS ( Nickel sulfide )CdCO3 ( CADMIUM 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)2CaC2O4MnCO3 ( Manganese(II) carbonate )HC2H3O2low solubility ( Slightly soluble )Ca(OH)2 ( Calcium hydroxide )CaS ( Calcium sulfide )PbCl2 ( Lead dichloride )H2CO3 ( Carbonic acid )H2S ( Hydrogen sulfide )

FALL 2021 GENERAL CHEMISTRY

The solubility of which of the following compounds could NOT be analyzed using the solubility rules? Correct answer: CCl4 Carbon tetrachloride is not an ionic compound, so its solubility in water cannot be determined by the solubility rules. Your answer: AgBr The solubility of silver bromide can be determined with the solubility rules because it is an ionic compound. It is an insoluble compound because silver halides are generally insoluble.

FALL 2021 GENERAL CHEMISTRY

Which of the following carbonate compounds is soluble in water? Correct answer: (NH4)2CO3 Ionic compounds containing the carbonate ion are mostly insoluble with the exception of the carbonates of group 1 metal cations and the ammonium ion. Therefore, of the given choices, only ammonium carbonate will be soluble. Your answer: CaCO3 Carbonates are generally insoluble. Calcium carbonate is not an exception.

Fall 2021 GENERAL CHEMISTRY

Which of the following compounds would form a precipitate in solution? LiNO3AlPO4CsBrRbHCO3AnswerAlPO4Phosphates are typically insoluble, and aluminum is not an exception to this rule. Compounds containing group 1 elements and halide ions are typically soluble. Therefore, LiNO3, CsBr, and RbHCO3 will not form precipitates.

Fall 2021 GENERAL CHEMISTRY

Which of the following iron (III) compounds will be insoluble in water? According to the solubility rules, the only choice that is insoluble is iron (III) hydroxide (Fe(OH)3). Most common hydroxides are insoluble. The only exceptions are hydroxides of the group 1 metal cations and barium hydroxide. Your answer: FeCl3 Most common chloride-containing ionic compounds are soluble. Iron (III) chloride (FeCl3) is not an exception.

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Which of the following is NOT water soluble? Correct answer: AgCl Silver chloride is an exception to the solubility of halides.

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Which type of anion will typically result in an insoluble compound? chromate According to solubility rules chromates will be insoluble except when combined with group one metal cations or the ammonium ion.

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a solid A precipitate is a solid ionic compound that separates from a liquid solution. It is generally composed of anions and cations. Your answer: a cation A cation usually makes up part of a precipitate; it is not the best description.