Use solubility rules to predict whether the following substances are soluble ins

Question

Use solubility rules to predict whether the following substances are soluble insoluble in water: K2CrO4, NiSO4, Cu(OH)2, Pb(C2H3O2)h, Ag2CO3, Al2S on 1. 2. In the following equations identify the substances oxidized and reduced K2Cr2O,(aq)+3SnCl2(aq) +14HCl(aq)2CrC(a)+3SnC1(aq)+7H O() + 2KCl(aq) s a net ionic equation. rite the above equation as a total ionic equation and a Predict if the following reactions will occur in aqueous solution and if so, write the products: 3. a. Al(s) +3NaCl(aq) -> b. Cl2(g) +2NaB(aq)-> c. Co(s) +NiC2(aq) Write formulas for the following substances as they would appear in a total ionic equation: 4. a. Aqueous calcium chloride b. Aqueous sulfuric acid c. Gaseous hydrogen sulfide d. Aqueous acetic acid e. Solid lithium carbonate f. Aqueous ammonia g. Aqueous sodium dihydrogen phosphate

Explanation / Answer

1. Let me put you the solubility rules, so you can have a guide and the explanation of my choice:

Rule 1. All compounds of Group IA elements (the alkali metals) are soluble.

Rule 2. All ammonium salts (salts of NH4+) are soluble.

Rule 3. All nitrate (NO3-), chlorate (ClO3-), perchlorate (ClO4-), and acetate (CH3COO- or C2H3O2-, sometimes abbreviated as Oac-) salts are soluble.

Rule 4. All chloride (Cl-), bromide (Br-), and iodide (I-) salts are soluble except for those of Ag+, Pb2+, and Hg22+.

Rule 5. All sulfate ( SO4=) compounds are soluble except those of Ba2+, Sr2+, Ca2+, Pb2+, Hg22+, and Hg2+, Ca2+ and Ag+ sulfates are only moderately soluble.

Rule 6. All hydroxide (OH-) compounds are insoluble except those of Group I-A (alkali metals) and Ba2+, Ca2+, and Sr2+.

Rule 7. All sulfide (S2-) compounds are insoluble except those of Groups I-A and II-A (alkali metals and alkali earths).

Rule 8. All sulfites (SO3=), carbonates (CO3=), chromates (CrO4=), and phosphates (PO43-) areinsoluble except for those of NH4+ and Group I-A (alkali metals)(see rules 1 and 2).

According to all of these rules, I'll list the substances that are soluble in water:

K2CrO4, NiSO4, Pb(CH3COO)2. The rest are insoluble in water

2. K2Cr2O7(aq) + 3SnCl2(aq) + 14HCl(aq) ----------------------------> 2CrCl3(aq) + 3SnCl4(aq) + 2KCl(aq) + 7H2O(l)

Total ionic equation:

2K+ + 2Cr2O72- + 3Sn2+ + 6Cl- + 14H+ + 14Cl- -----------> 2Cr+3 + 6Cl- + 3Sn+4 + 12Cl- + 2K+ + 2Cl- + 7H2O

Total net equation:

2Cr2O72- + 3Sn2+ + 14H+ -----------> 2Cr+3 + 3Sn+4 + 7H2O

Now from the net equation, you can see that Sn2+ goes to Sn4+, this means that is losing electrons, therefore it's oxidating; the Cr2O72- goes from the oxidation state of Cr that is 6+, to 3+. so it's gaining electrons, therefore, it's reducting.

3. a) Al(s) + 3NaCl(aq) ----------> AlCl3(s) + 3Na+(aq)

This will occur because according to solubility rules (rule 4) all chlorides, are soluble.

b) Cl2(g) + NaBr(aq) This will not occur, because the chlorium it's not strong enought to displace the Bromide ion in solution.

c) Co(s) + NiCl2(aq) -----------> CoCl2(s) + Ni2+(aq) See rule 4.

For question 4, I'll answer it if you post it in a new question. However all you have to do is put the elements and compounds as I put them in question 2. If you urgently need this question answered asap, tell me in a comment. If not, put it in a new question.

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