a On the basis of the general solubility rules, which choice explains why sodium sulfide would be expected to be appreciably soluble in water. Most sulfide (S²- ) salts are only slightly soluble. Most salts of Na+ are insoluble. Most sulfide (S²) salts are soluble. Most salts of Na+ are soluble. bon the basis of the general solubility rules, which choice explains why iron(II) nitrate would be expected to be appreciably soluble in water. O Most nitrate salts are soluble. Most salts of Fe²+ are soluble. Most nitrate salts are insoluble. O Most salts of Fe2+ are insoluble.

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The solubility rules listed in table below.
General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C.
1. Most nitrate (NO3¯) salts are soluble.
2. Most salts of Na+, K+, and NH4+ are soluble.
3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂.
4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4.
5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and
KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble.
6. Most sulfide (S²-), carbonate (CO3²), and phosphate (PO4³-) salts are only slightly soluble.*
*The terms insoluble and slightly soluble really mean the same thing: such a tiny amount
dissolves that it is not possible to detect it with the naked eye.
a on the basis of the general solubility rules, which choice explains why sodium sulfide would be expected to be appreciably soluble in water.
Most sulfide (S²-) salts are only slightly soluble.
2-
Most salts of Na+ are insoluble.
Most sulfide (S²-) salts are soluble.
Most salts of Na+ are soluble.
bon the basis of the general solubility rules, which choice explains why iron (II) nitrate would be expected to be appreciably soluble in water.
Most nitrate salts are soluble.
Most salts of Fe²+ are soluble.
Most nitrate salts are insoluble.
Most salts of Fe²+ are insoluble.
Transcribed Image Text:The solubility rules listed in table below. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3¯) salts are soluble. 2. Most salts of Na+, K+, and NH4+ are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide (S²-), carbonate (CO3²), and phosphate (PO4³-) salts are only slightly soluble.* *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. a on the basis of the general solubility rules, which choice explains why sodium sulfide would be expected to be appreciably soluble in water. Most sulfide (S²-) salts are only slightly soluble. 2- Most salts of Na+ are insoluble. Most sulfide (S²-) salts are soluble. Most salts of Na+ are soluble. bon the basis of the general solubility rules, which choice explains why iron (II) nitrate would be expected to be appreciably soluble in water. Most nitrate salts are soluble. Most salts of Fe²+ are soluble. Most nitrate salts are insoluble. Most salts of Fe²+ are insoluble.
On the basis of the general solubility rules, which choice explains why ammonium sulfide would be expected to be appreciably soluble in water.
Most salts of NH4+ are soluble.
Most sulfide salts are only slightly soluble.
Most sulfide salts are insoluble.
Most salts of NH4+ are insoluble.
dOn the basis of the general solubility rules, which choice explains why cesium sulfate would be expected to be appreciably soluble in water.
Most salts of Cs are only slightly soluble.
Most sulfate salts are soluble.
Most salts of Cs+ are insoluble.
Most sulfate salts are insoluble.
e On the basis of the general solubility rules, which choice explains why iron(II) chloride would be expected to be appreciably soluble in water.
Most salts of Fe²+ are insoluble.
Most chloride salts are soluble.
Most salts of Fe²+ are soluble.
Most chloride salts are insoluble.
Transcribed Image Text:On the basis of the general solubility rules, which choice explains why ammonium sulfide would be expected to be appreciably soluble in water. Most salts of NH4+ are soluble. Most sulfide salts are only slightly soluble. Most sulfide salts are insoluble. Most salts of NH4+ are insoluble. dOn the basis of the general solubility rules, which choice explains why cesium sulfate would be expected to be appreciably soluble in water. Most salts of Cs are only slightly soluble. Most sulfate salts are soluble. Most salts of Cs+ are insoluble. Most sulfate salts are insoluble. e On the basis of the general solubility rules, which choice explains why iron(II) chloride would be expected to be appreciably soluble in water. Most salts of Fe²+ are insoluble. Most chloride salts are soluble. Most salts of Fe²+ are soluble. Most chloride salts are insoluble.
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