Question

Part A:

Part B:

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2. For the reactions that were to be completed in Part A of the experiment, prepare a table with the formulas from Group A as headings of the columns and the formulas of Group B as headings of the ows. Within the table, fill in the formula and systematic name of the predicted precipitates that will form. If no precipitate is expected from the reaction, write 'No Reaction'. For each predicted precipitate, look up the compound online, and write the expected color. Cite the source of the color information for each compound. Section3 4. Three of the seven tested reactions from Part B were acid/base reactions. For each acid/base reaction include the following: a. Molecular equation b. Complete ionic equation c. Net ionic equation d. For each reactant, indicate whether it was a strong acid, strong base weak acid or weak base. 5. Three of the seven tested reactions from part B were oxidation/ reduction reactions (HINT: only one of reactions 5 or 6 will react. For the other there will not be a reaction.) For each oxidation/ reduction reaction include the following: c. Molecular cquation f. Below each molecular equation, state which element was oxidized and indicate the oxidation number the element had as a reactant and product. Example: Zn(s) +2HBr(a)-ZnBr(aq) +H2(g) Zinc was oxidized. The oxidation number changed from 0 (reactant) to +2 (product) Pb(CH3CO2)2 (aq)+ Na2SO, (aq)PbSO4 +2 NaCH3CO2 Whether or not the reaction will actually take place depends on the solubility NaCH3CO2 Examination of the solubility rules shows that PbSO, is insoluble an is soluble, thus the equation can be completed with the predicted physical state ucts: Pb(CH,CO,)(ag) + Na,SO(ag)PbsO,(s) + 2 NaCH,CO,(aq) Ca(OH (aq) 2 HCl(aq)CaCl2(aq) 2 H2O0) CaCh is classified as a salt, which is an ionic compound made up of a cation other than H' and an anion other than OH or O. Thus, in this type of double replacement, the products typically consist of water and a salt. Below is another example, involving acetic acid in place of hydrochloric acid, producing water and the salt, sodium acetate. (Note where the protic H is located in the formula of acetic acid.) The physical state of the salt is predicted according to the solubility rules. NaOH(aq) CH,CO H(ag)Na(CH,Co2(aq)+ H,00) There are several common variations to these acid-base reactions with which you need to be familiar. If the product of the double replacement is carbonic acid (H2COs), it should be replaced with H20 and CO2. Carbonic acid is unstable in water and immediately decomposes Cto water and carbon dioxide. H,co,(aq) H20() + CO2(g) Thus, the reaction of hydrochloric acid and potassium carbonate is written as follows: 2 HCI(aq)+ K,CO,(aq)2 KCI(aq)+H2O0) CO.(g) to its neutral form (Fe? to Fe in equation ) and H' to H2 in equation 7), so is being reduced. 2 AI(s) 3 Fe(NO3)2(aq)3 Fe(s) 2 AI(NO3) (aq) Zn(s) + 2 HBr(aq) ZnBr2(aq) H2(g) As with precipitation reactions, one can write single replacement equations for any combi-

Answer 1

2. The information in the part A is insufficient. However, the reaction given in Part a is a precipitation reaction. This reaction is applied to test the presence of SO₄^2- ions in any given unknown salt.

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Section 3

4. The acid base reactions

Ca(OH)₂ + 2HCl ---------> CaCl₂ + 2H₂O

Hear Ca(OH)₂ is strong base and HCl is strong acid.

Ca(OH)₂ + HCl -------------> CaCl₂ + H₂O is molecular equation

OH^- + H⁺ ---------------> H₂O is ionic euation

2OH^- + 2H⁺ ---------------> 2H₂O is net ionic equation

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NaOH + CH₃COOH ------------------> CH₃COONa + H₂O   it self a molecular equation

OH^- + H⁺ ---------------> H₂O is ionic and net ionic equation.

here, NaOH is strong base and acetic acid CH3 COOH is weak acid.

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2HCl + K₂CO₃ ------------------> 2KCl + H₂O + CO₂

HCl + K₂CO₃ ------------------> KCl + H₂O + CO₂ molecular equation

here HCl is strong acid and K2CO3 is strong base

H⁺ + CO₃^2- ---------------> H₂O + CO₂ ionic equation

2H⁺ + CO₃^2- ---------------> H₂O + CO₂ net ionic equation

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Al + Fe(NO₃)₂ --------------> Fe + Al(NO₃)₃ is molecular equation

here Al is oxidizing from 0 oxidation state to +3 oxidation state. and Fe is reducing from +2 to 0

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Zn + HBr -----------------> ZnBr₂ + H₂ molecular equation

Here Zn is oxidizing from 0 to +2 oxidation state. and Hydrogen H+ is reducing from +1 to 0 oxidation state.