Multiple ChoicePredict whether a chemical reaction occurs and write the balanced molecular equation.Ag2SO4 (aq) + KCl (aq) →778views3rank3comments
Multiple ChoicePredict whether a chemical reaction occurs and write the balanced molecular equation.MgBr2 (aq) + NaC2H3O2 (aq) →634views3comments
Multiple ChoiceDetermine the balanced equation for the neutralization equationCa(OH)2 (aq) + HCN (aq) →1079views3rank4comments
Textbook QuestionYou are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next an Na2SO41aq2 solution is added and a white precipitate forms. What is the identity of the unknown white solid?424views
Textbook QuestionWhich of the following solutions will not form a precipitate when added to 10 mL of 0.10 M KOH? (LO 4.10, 4.11) (a) 10 mL of 0.10 NH4Cl (b) 10 mL of 0.10 M PbSO4 (c) 10 mL of 0.10 M Fe(NO3)3 (d) 10 mL of 0.10 M AgCH3CO2779views
Textbook QuestionWhat kind of reaction is the 'water-splitting' reaction? H2O(l)¡H2(g) + ½ O2(g) (a) an acid-base reaction (b) a metathesis reaction (c) a redox reaction (d) a precipitation reaction556views
Textbook QuestionThree cations, Ni2+ , Cu2+ , and Ag+, are separated using two different precipitating agents. Based on Figure 17.23, what two precipitating agents could be used? Using these agents, indicate which of the cations is A, which is B, and which is C.416views
Textbook QuestionWrite a balanced chemical equation for the reaction that occurs when (a) Mg(s) reacts with Cl2(g)835views
Textbook QuestionBalance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (b) NH4NO3(s) → N2O(g) + H2O(g)331views
Textbook QuestionBalance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) C3H6(s) + O2(g) → CO2(g) + H2O(l)409views
Textbook QuestionBalance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) NaClO31s2¡NaCl1s2 + O2(g)331views
Textbook QuestionWill precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (c) Na2S and FeCl3.776views
Textbook QuestionIdentify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction.(b) LiOH and MnCl2999views
Textbook Question(a) When chlorine atoms react with atmospheric ozone, what are the products of the reaction?611views
Textbook QuestionSeparate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?1162views
Textbook QuestionYou know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3, CaCl2, or Al21SO423. A friend suggests that you test a portion of the solution with Ba1NO322 and then with NaCl solutions. According to your friend's logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle? (a) Barium sulfate could precipitate. (b) Silver chloride could precipitate. (c) Silver sulfate could precipitate. (d) More than one, but not all, of the reactions described in answers a–c could occur. (e) All three reactions described in answers a–c could occur.1504views1rank
Textbook QuestionThree solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb1CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCl2 present. What solid(s) will precipitate?2312views4rank
Textbook QuestionAssume that an aqueous solution of a cation, represented as a red sphere, is allowed to mix with a solution of an anion, represented as a yellow sphere. Three possible outcomes are represented by boxes (1)–(3): Which outcome corresponds to each of the following reactions? (a) 2 Na+(aq) + CO32-(aq) S (b) Ba2+(aq) + CrO42-(aq) S (c) 2 Ag+(aq) + SO32-(aq) S582views
Textbook QuestionAssume that an aqueous solution of a cation, represented as a blue sphere, is allowed to mix with a solution of an anion, repre-sented as a red sphere, and that the following result is obtained: Which combinations of cation and anion, chosen from the fol-lowing lists, are compatible with the observed results? Explain Cations: Na+, Ca2+, Ag+, Ni2+ Anions: Cl-, CO3 2-, CrO4 2-, NO3834views
Textbook QuestionAssume that an aqueous solution of OH-, represented as a blue sphere, is allowed to mix with a solution of an acid HnA, represented as a red sphere. Three possible outcomes are depicted by boxes (1)–(3), where the green spheres represent An-, the anion of the acid: Which outcome corresponds to each of the following reactions? (a) (b) (c)532views
Textbook QuestionMagnesium ions are removed in water treatment by the addition of slaked lime, Ca(OH)2. Write a balanced chemical equation to describe what occurs in this process906views
Textbook QuestionNatural gas consists primarily of methane, CH4(g). (b) Write a balanced chemical equation for the incomplete combustion of methane to product CO(g) as the only carbon-containg product.611views
Textbook QuestionWrite a balanced equation for the reaction that occurs in each of the following cases: (c) A fresh surface of lithium metal is exposed to oxygen gas.449views
Textbook QuestionWrite a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas.457views
Textbook QuestionWrite a balanced equation for the reaction that occurs in each of the following cases: (c) Sodium reacts with oxygen.498views
Textbook QuestionWrite a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water.639views
Textbook QuestionClassify each of the following reactions as a precipitation, acid–base neutralization, or oxidation–reduction. (a) (b) (c)881views
Textbook QuestionComplete and balance each equation. If no reaction occurs, write 'NO REACTION.' c. CrBr2(aq) + Na2CO3(aq)¡412views
Textbook QuestionComplete and balance each equation. If no reaction occurs, write 'NO REACTION.' b. KCl(aq) + CaS(aq)¡1432views1rank
Textbook QuestionComplete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. LiI(aq) + BaS(aq)1081views1rank
Textbook QuestionComplete and balance each equation. If no reaction occurs, write 'NO REACTION.' d. NH4Cl(aq) + AgNO3(aq)¡376views
Textbook QuestionComplete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. NaNO3(aq) + KCl(aq)¡2409views1rank
Textbook QuestionA solution containing several metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H2S is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with (NH4)2HPO4. No precipitate forms. Which of these metal cations are either possibly present or definitely absent: Al3+, Na+, Ag+, Mg2+?693views1rank
Textbook QuestionWrite a balanced equation for the reaction that occurs in each of the following cases: (d) Fluorine reacts with water.735views
Textbook QuestionWrite a balanced equation for the reaction that occurs in each of the following cases: (c) Sulfur reacts with hydrogen gas.693views
Textbook QuestionWrite a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' c. copper(II) nitrate and magnesium sulfide1641views
Textbook QuestionWrite a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. potassium carbonate and lead(II) nitrate1092views
Textbook QuestionWrite a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate1198views
Textbook QuestionIn the course of various qualitative analysis procedures, the following mixtures are encountered: (d) Ag+ and Mn2+. Suggest how each mixture might be separated.356views
Textbook QuestionIn the course of various qualitative analysis procedures, the following mixtures are encountered: (a) Zn2+ and Cd2+. Suggest how each mixture might be separated.407views
Textbook QuestionWhich of the following solutions will not form a precipitate when added to 0.10 M BaCl2? (a) 0.10 M LiNO3 (b) 0.10 M K2SO4 (c) 0.10 M AgNO31514views
Textbook QuestionSuggest how the cations in each of the following solution mixtures can be separated: (c) Pb2 + and Al3 +.457views
Textbook QuestionWhich of the following solutions will not form a precipitate when added to 0.10 M NaOH? (a) 0.10 M MgBr2 (b) 0.10 M NH4Br (c) 0.10 M FeCl21094views
Textbook QuestionHow would you prepare the following substances by a precipitation reaction? (a) PbSO4751views
Textbook QuestionHow would you prepare the following substances by a precipitation reaction? (b) Mg3(PO4)2318views
Textbook QuestionComplete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq)¡1131views
Textbook QuestionAssume that you have an aqueous mixture of NaNO3 and AgNO3. How could you use a precipitation reaction to separate the two metal ions?890views
Textbook QuestionA solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (b) What precipitate forms?382views
Textbook QuestionAssume that you have an aqueous mixture of BaCl2 and CuCl2. How could you use a precipitation reaction to sepa-rate the two metal ions?699views
Textbook QuestionWrite balanced chemical equations for (c) the combination reaction between nickel metal and chlorine gas.462views
Textbook QuestionA solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (a) Write the balanced chemical equation for the reaction that occurs.402views
Textbook QuestionAssume that you have an aqueous solution of an unknown salt. Treatment of the solution with dilute NaOH, Na2SO4, and KCl produces no precipitate. Which of the following cations might the solution contain? (a) Ag+ (b) Cs+ (c) Ba2+ (d) NH4 +792views
Textbook QuestionAssume that you have an aqueous solution of an unknown salt. Treatment of the solution with dilute BaCl2, AgNO3, and Cu(NO3)2 produces no precipitate. Which of the following anions might the solution contain? (a) Cl- (b) NO3 (c) OH- (d) SO4- 2-1039views
Textbook QuestionHow could you use a precipitation reaction to separate each of the following pairs of cations? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (a)627views
Textbook QuestionHow could you use a precipitation reaction to separate each of the following pairs of cations? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (b)549views
Textbook QuestionHow could you use a precipitation reaction to separate each of the following pairs of anions? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (a)754views
Textbook QuestionUranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear weapons. UF6 can be produced in a two-step reaction. Solid uranium (IV) oxide, UO2, is first made to react with hydrofluoric acid (HF) solution to form solid UF4 with water as a by-product. UF4 further reacts with fluorine gas to form UF6. (b) Which step is an acid-base reaction?925views
Textbook QuestionThe following three solutions are mixed: 100.0 mL of 0.100 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 100.0 mL of 0.200 M Ba(CN)2. (a) What ionic compounds will precipitate out of solution?632views
Textbook QuestionA 25.0-mL sample of 0.050 M barium nitrate solution was mixed with 25.0 mL of 0.050 M sodium sulfate solution labeled with radioactive sulfur-35. The activity of the initial sodium sulfate solution was 1.22⨉106 Bq/mL. After the resultant precipitate was removed by filtration, the remaining filtrate was found to have an activity of 250 Bq/mL. (a) Write a balanced chemical equation for the reaction that occurred.526views
Textbook QuestionA 250.0 g sample of a white solid is known to be a mixture of KNO3, BaCl2, and NaCl. When 100.0 g of this mixture is dis-solved in water and allowed to react with excess H2SO4, 67.3 g of a white precipitate is collected. When the remaining 150.0 g of the mixture is dissolved in water and allowed to react with excess AgNO3, 197.6 g of a second precipitate is collected. (a) What are the formulas of the two precipitates?459views
Textbook QuestionWrite balanced ionic equations for the following reactions. (b) Aqueous sodium hydroxide is neutralized by aqueous acetic acid.732views
Textbook QuestionWrite balanced ionic equations for the following reactions. (a) Aqueous perchloric acid is neutralized by aqueous calcium hydroxide.569views
Textbook QuestionWrite balanced ionic equations for the following reactions. (b) Aqueous barium hydroxide is neutralized by aqueous nitric acid.772views
Textbook QuestionWrite balanced ionic equations for the following reactions. (a) Aqueous hydrobromic acid is neutralized by aqueous calcium hydroxide.907views
Textbook QuestionAcetylene 1C2H22 and nitrogen 1N22 both contain a triple bond, but they differ greatly in their chemical properties. (c) Write balanced chemical equations for the complete oxidation of N2 to form N2O51g2 and of acetylene to form CO21g2 and H2O1g2. Write a balanced chemical equation for the complete oxidation of acetylene to form CO2( g) and H2O(g).343views
Textbook QuestionTrifluoroacetic acid has the chemical formula CF3CO2H. It is a colorless liquid that has a density of 1.489 g/mL. (b) Trifluoroacetic acid can react with NaOH in aqueous solution to produce the trifluoroacetate ion, CF3COO2. Write the balanced chemical equation for this reaction.1023views
Textbook QuestionA hydrochloric acid solution will neutralize a sodium hydroxide solution. Look at the molecular views showing one beaker of HCl and four beakers of NaOH. Which NaOH beaker will just neutralize the HCl beaker? Begin by writing a balanced chemical equation for the neutralization reaction. 1932views
Textbook QuestionPredict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' d. aqueous ammonium chloride and aqueous calcium hydroxide716views
Textbook QuestionPredict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' a. HCl(aq) + Hg2(NO3)2(aq)¡671views
Textbook QuestionPredict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' b. Cr(NO3)3(aq) + LiOH(aq)¡1416views
Textbook QuestionBaking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid 1H2CO32, which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO21g2 forms bubbles and causes the cake to rise. (a) A rule of thumb in baking is that 1/2 teaspoon of baking soda is neutralized by one cup of sour milk. The acid component in sour milk is lactic acid, CH3CH1OH2COOH. Write the chemical equation for this neutralization reaction.1550views
Textbook QuestionA solution contains one or more of the following ions: Hg2 2 + , Ba2 + , and Fe2 + . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Which ions were present in the original solution?1409views
Textbook QuestionA solution contains one or more of the following ions: Hg2 2 + , Ba2 + , and Fe2 + . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Write net ionic equations for the formation of each of the precipitates observed.831views
Textbook QuestionA compound with the formula XOCl2 reacts with water, yielding HCl and another acid H2XO3, which has two acidic hydrogens that react with NaOH. When 0.350 g of XOCl2 was added to 50.0 mL of water and the resultant solution was titrated, 96.1 mL of 0.1225 M NaOH was required to react with all the acid. (a) Write a balanced equation for the reaction of XOCl2 with H2O.522views
Textbook Question(a) Write a balanced equation for the reaction of potassium metal with water.1352views
Open QuestionSuppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate?272views
Open QuestionWrite balanced molecular equation for the reaction between nitric acid and calcium hydroxide.154views
Open QuestionFormic acid can react with NaOH in aqueous solution to produce the formate ion, HCOO−. Write the balanced chemical equation for this reaction.298views
Open QuestionWrite an equation for the precipitation reaction that occurs (if any) when you mix solutions of ammonium chloride and iron(III) nitrate mix.200views
Open QuestionEnter the molecular equation representing aqueous acetic acid neutralized by aqueous barium hydroxide.180views
Open QuestionIn a chemical equation, which symbol should be used to indicate that a substance is in solution?181views
Open QuestionThe mixing of which pair of reactants will result in a precipitation reaction?577views1rank
Open QuestionSuppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate?219views
Open QuestionWrite a balanced molecular equation for the reaction between nitric acid and calcium hydroxide.204views
Open QuestionWhich clue can be used to identify a chemical reaction as a replacement reaction?216views
Open QuestionIn which type of reaction do two simple elements combine together to form a more complex compound?166views
Open QuestionFor the science fair, deshawn demonstrated the ___ reaction between ozone and chlorine.182views
Open QuestionWhich type of reaction is NACl + AgNO3 → NaNO3 + AgCl? synthesis decomposition oxidation replacement296views1rank
Open QuestionWhich of the following is not a correct chemical equation for a double displacement reaction?184views
Open QuestionWhat else is produced during the combustion of butane, C4H10? 2 C4H10 + 13 O2 → 8________ + 10 H2O202views
Open QuestionGive an example of a chemical reaction during which a single substance breaks down.165views
Open QuestionWhat solid would form when phosphoric acid (H3PO4) is added to milk of magnesia (Mg(OH)2)?183views
Open QuestionWhat is produced when calcium reacts with fluorine in a synthesis reaction? Ca + F2 ________193views
Open QuestionWhich product in the reaction forms a precipitate?PbSO4 MgCl2 PbMg no precipitate formed173views
Open QuestionWhich one of the following would form a precipitate with PO43- ions in aqueous solution?175views
Open QuestionComplete the acid-base reaction between butyric acid HC4H7O2 and potassium hydroxide KOH.187views
Open QuestionConsider this reaction: acid + base salt + water. What type of reaction is this?146views
Open QuestionWhen a base is mixed with an acidic solution, neutralization occurs because the -157views
Open QuestionWrite the complete balanced equation for the decomposition of magnesium chlorate (Mg(ClO3)2).162views
Open QuestionA chemical reaction that involves both decomposition and synthesis is called a(n) reaction.144views
Open QuestionAn insoluble product (i.e., a solid) that forms from a reaction in solution is called a(n)188views