![Basic Chemistry (5th Edition)](https://www.bartleby.com/isbn_cover_images/9780134138046/9780134138046_largeCoverImage.gif)
Concept explainers
(a)
Interpretation:
The net ionic equation of the given reaction should be determined.
Concept Introduction:
The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of
transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble. - The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(b)
Interpretation:
The net ionic equation of the given reaction should be determined.
Concept Introduction:
The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(c)
Interpretation:
The net ionic equation of the given reaction should be determined.
Concept Introduction:
The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(d)
Interpretation:
The net ionic equation of the given reaction should be determined.
Concept Introduction:
The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 12 Solutions
Basic Chemistry (5th Edition)
- Nonearrow_forward4. Draw and label all possible isomers for [M(py)3(DMSO)2(CI)] (py = pyridine, DMSO dimethylsulfoxide).arrow_forwardThe emission data in cps displayed in Table 1 is reported to two decimal places by the chemist. However, the instrument output is shown in Table 2. Table 2. Iron emission from ICP-AES Sample Blank Standard Emission, cps 579.503252562 9308340.13122 Unknown Sample 343.232365741 Did the chemist make the correct choice in how they choose to display the data up in Table 1? Choose the best explanation from the choices below. No. Since the instrument calculates 12 digits for all values, they should all be kept and not truncated. Doing so would eliminate significant information. No. Since the instrument calculates 5 decimal places for the standard, all of the values should be limited to the same number. The other decimal places are not significant for the blank and unknown sample. Yes. The way Saman made the standards was limited by the 250-mL volumetric flask. This glassware can report values to 2 decimal places, and this establishes our number of significant figures. Yes. Instrumental data…arrow_forward
- 7. Draw a curved arrow mechanism for the following reaction. HO cat. HCI OH in dioxane with 4A molecular sievesarrow_forwardTry: Convert the given 3D perspective structure to Newman projection about C2 - C3 bond (C2 carbon in the front). Also, show Newman projection of other possible staggered conformers and circle the most stable conformation. Use the template shown. F H3C Br Harrow_forwardNonearrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)