CHEM 001A Lecture Notes - Lecture 8: Nickel(Ii) Chloride, Hydrobromic Acid, Chemical Equation

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8 Mar 2018

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Solubility rules: soluble cations, group i ions (alkali metals) and nh4, soluble anions: And ch3coo (acetate: no3, cl , br , and i , except those of ag+, cu+, pb2+, hg22, sulfates (so4. 2+, ca2+, ba2+, sr2: combining anions and cations not listed above results in formation of an insoluble compound. 3(s) ni(po3)2(aq) + 6 na+(s) + 6 cl-(s) Quiz: given: cas(aq) + 2 hbr(aq)i cabr2(aq) + h2s(s, write the net ionic equation, classify the following compounds as soluble or insoluble, baco3, na2co3, fe(no3)3. 2-(aq) + cu(s: fe(s) fe2+(aq) + 2 e, cu2+(aq) + 2 e- cu(s) Rules: o. n. s of atoms in a neutral molecule sum to zero; o. n. s of atoms in an ion sum to charge on the ion, in each atom in a pure element, o. n. = zero: f2 = 0; fe = 0 o2 = 0 na = 0, in monatomic ion, o. n. = charge on the ion: f = 1 fe3+ = +3.

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1. (10)What ions and/or molecules are present in relatively large proportions in a solution of a weak acid, HF (aq)? Select all appropriate answers. H+ HF F- HF+ F+ F2+ H2- F2- H F 2. (10)What ions and/or molecules are present in relatively large proportions in a solution of a strong base NaOH (aq)? Select all appropriate answers. NaOH Na2+ OH2- OH- NaO+ OH+ Na Na+ OH 3. (10)What ions and/or molecules are present in relatively large proportions in a solution of a strong acid HClO3 (aq)? Select all appropriate answers. HClO3 ClO3- HCl+ Cl+ H+ ClO3+ O3- O32- HCl None of these is present in relatively large proportions 4. (10)What ions and/or molecules are present in relatively large proportions in a solution of the soluble ionic compound NiCl2 (aq)? Select all appropriate answers. Ni2+ NiCl2 Cl22- Cl2- Ni+ Cl2- Ni Cl Cl2 Cl- 5. (5)Which of the following equations represents the proper net ionic equation for the precipitation of an insoluble sulfide compound from ZnBr2(aq) and Na2S(aq). Na2S(aq) + ZnBr2(aq) ----> 2 NaBr(aq) + ZnS(s) Zn2+(aq) + S2-(aq) ----> ZnS(s) Na2S(aq) + 2 Br-(aq) ----> 2 NaBr(s) + S2-(aq) Br-(aq) + Na+(aq) ----> NaBr(s) S2-(aq) + ZnBr2(aq) ----> ZnS(s) + 2 Br-(aq) 3 S2-(aq) + 2 Zn3+(aq) ----> Zn2S3(s) Na2+(aq) + Br2-(aq) ----> Na2Br2(s) Na2S(aq) + ZnBr2(aq) ----> Na2Br2(aq) + ZnS(s) Zn+(aq) + S-(aq) ----> ZnS(s) 6. (5)Which of the following equations represents the proper net ionic equation for the complete neutralization reaction between the strong acid HI(aq) and the weak base NH3(aq)? H+ (aq) + NH3(aq) ----> NH4+ (aq) HI (aq) + OH- (aq) ----> H2O (l) + I- (aq) HI (aq) + NH3(aq) ----> NH4I (aq) I- (aq) + NH4+ (aq) ----> NH4I (aq) H+ (aq) + OH- (aq) ----> H2O (l) HI (aq) + OH- (aq) ----> H2IO (aq) H+ (aq) + NH4+ (aq) ----> NH5+ (aq) I- (aq) + OH- (aq) ----> HIO (aq) mark 7. (5)What are the spectator ions in the solution after completely precipitating an insoluble carbonate compound when mixing Ca(ClO3)2 (aq) and Na2CO3 (aq)? Ca2+ , ClO3- , Na+ , and CO32- Na+ and CO32- CO32- and ClO3- CO32- and Ca2+ Ca2+ and ClO3- Ca2+ and Na+ Na+ ClO3- ClO3- and Na+ Ca2+ 8. (5)What are the spectator ions in the solution after the complete neutralization reaction occurs when mixing the weak acid H2S (aq) and the strong base KOH (aq)? H+ , S2- , K+ , and OH- OH- and K+ H+ and OH- OH- and S2- K+ and S2- K+ and H+ S2- and H+ K+ S2-

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The amount of l3- in a solution can be determined by titration with a solution containing a known concentration of s2o32-(aq) (thiosulfate ion). The determination is based on the net ionic equation Given that it requires 38.2 mL of 0.450 M Na2s2o3(aq) to titrate a 25.0-ml sample of l0-(aq), calculate the molarity of l0-(aq) in the solution. The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 7.99-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCI(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+(ag). The Sb3+(aq) is completely oxidized by 39.4 mL of a 0.115 M aqueous solution of KBr03(aq). The unbalanced equation for the reaction is calculate the amount of antimony in the sample and its percentage in the ore. Write a balanced overall reaction from these unbalanced half-reactions. Cu rightarrow cu2+ Ag rightarrow Ag balanced overall reaction: An experiment was performed to test the relative activities of four metals, A, B, C, and D. Each solid metal was mixed with solutions of each of the other cations as shown in this chart. The results were indicated as follows y=yes a reaction occurred N=no a reaction did not occur For example, when A+ (aq) was mixed with B (s), a reaction occurred. Use this data to rank the neutral metals according to their activity. Rank these species by their ability to act as an oxidizing agent. Best oxidizing agent Best reducing agent. Best reducing agent Mg2+ Cu2t Ct2* Ag+ For the following reaction kcio3 rightarrow kci+3/2o2 assign oxidation states to each element on each side of the equation Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. H2SO4 + 2KOH rightarrow 2H2O+K2SO4 0.950 L of 0.450 M H2SO4 is mixed with 0.900 L of 0.290 M KOH. What concentration of sulfuric acid remains after neutralization? Enter the net ionic equation, including phases, for the reaction of AgNo3(aq) with BaO(aq). Write the net ionic equation (including phases) that corresponds to Fe(No3)2(aq)+Na2S(aq) rightarrow FeS(s) + 2NaNO3 (aq) If a solution containing 126.27 g of mercury(ll) chlorate is allowed to react completely with a solution containing 17.796 g of sodium sulfide, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction? Write the balanced equation for the reaction of aqueous Pb(CI03)2 with aqueous Nal. Include phases. What mass of precipitate will form if 1.50 L of concentrated Pb(CI03)2 is mixed with 0.850 L of 0.220 M Nal? Assume the reaction goes to completion. Predict whether the following compounds are soluble or insoluble in water: CuC03 KN03 Pb(N03)2 BaS04 PbCI2 CuCI2

Solution Investigation Question: What are some of the key characteristics of unknown sample of an aqueous solution containing an ionic compound?

1. Given that the cation is from Group 1A, what is the identity of the group 1A metal ion in your solution?

2. Given that the ionic compound contains either chloride or hydroxide, how can you determine which? (Two pieces of evidence are required and one must be related to solubility rules)

3. What is the concentration of your solution? (Your unknown sample is known to be about 1 M, but you need to determine the concentration to 3 significant figures using titration. You should plan ahead so that you know approximately what volume of your sample you will need in order to use approximately 25 mL of 0.100 M sulfuric acid for the titration).

CHEM 001A Lecture Notes - Lecture 8: Nickel(Ii) Chloride, Hydrobromic Acid, Chemical Equation

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