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Both the solubility product and ionic product are applicable to all types of solutions.
  • a)
    true
  • b)
    false
Correct answer is option 'B'. Can you explain this answer?
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Both the solubility product and ionic product are applicable to all ty...
Solubility of the product is only applicable to the saturated solutions, whereas an ionic product is applicable to all types of solutions. It is because the formation of a precipitate is dependent on the solubility product.
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Both the solubility product and ionic product are applicable to all ty...
Explanation:

The statement "Both the solubility product and ionic product are applicable to all types of solutions" is false.

Solubility Product:
The solubility product (Ksp) is a specific type of equilibrium constant that is used to describe the dissolution of a sparingly soluble salt in water. It represents the equilibrium between the solid salt and its dissociated ions in a saturated solution. The solubility product is only applicable to sparingly soluble salts and does not apply to all types of solutions.

Ionic Product:
The ionic product (Q) is a general term used to describe the product of the concentrations (or activities) of the ions in a solution. It is similar to the solubility product, but it is not limited to sparingly soluble salts. The ionic product can be used to determine the extent of ionization in a solution, regardless of whether the solute is a sparingly soluble salt or a strong electrolyte. However, it is important to note that the ionic product is not a constant like the solubility product.

Differences:
1. Applicability: The solubility product is only applicable to sparingly soluble salts, while the ionic product can be used for any type of solution.
2. Equilibrium Constant: The solubility product is a specific type of equilibrium constant, while the ionic product is not a constant but a measure of the ion concentrations in a solution.
3. Calculation: The solubility product is calculated based on the concentrations of the dissociated ions at equilibrium, while the ionic product can be calculated at any point in the reaction.

In conclusion, the solubility product and ionic product are not applicable to all types of solutions. The solubility product is specific to sparingly soluble salts, while the ionic product can be used for any type of solution.
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Two scientists wanted to test the solubility of different substances. Solubility is a measure of how many moles of a given substance (known as the solut e) can dissolve in a given volume of another substance (known as the solvent). The solvent can also be thought of as the substance present in greater amount, while the solute can be seen as the substance present in lesser amount. The scientists performed the following experiments to investigate this property.Experiment 1The scientists tested the number of moles of several substances that could be completely dissolved in 50mL of water at various temperatures. They made their solutions by slowly adding amounts of each substance to beakers sitting on a hot plate containing water and a stirring rod until no more of the substance dissolved in the solution. The beakers were weighed before and after the additions and the difference in mass was calculated to be the added mass of the substance. The researchers then calculated the number of moles that dissolved for each trial using the molecular mass and the recorded mass for each trial. Results are recorded in Table 1.Table 1Experiment 2In this experiment, the scientists wanted to test the solubility of NaCl in a variety of liquids at several temperatures. Their procedure was similar to that of Experiment 1, but with a range of liquids and only one solid. The results are compiled in Table 2.Table 2Q.Which of the following correctly ranks the solutes from Experiment 1 in decreasing order of solubility in water at 50C?

Two scientists wanted to test the solubility of different substances. Solubility is a measure of how many moles of a given substance (known as the solut e) can dissolve in a given volume of another substance (known as the solvent). The solvent can also be thought of as the substance present in greater amount, while the solute can be seen as the substance present in lesser amount. The scientists performed the following experiments to investigate this property.Experiment 1The scientists tested the number of moles of several substances that could be completely dissolved in 50mL of water at various temperatures. They made their solutions by slowly adding amounts of each substance to beakers sitting on a hot plate containing water and a stirring rod until no more of the substance dissolved in the solution. The beakers were weighed before and after the additions and the difference in mass was calculated to be the added mass of the substance. The researchers then calculated the number of moles that dissolved for each trial using the molecular mass and the recorded mass for each trial. Results are recorded in Table 1.Table 1Experiment 2In this experiment, the scientists wanted to test the solubility of NaCl in a variety of liquids at several temperatures. Their procedure was similar to that of Experiment 1, but with a range of liquids and only one solid. The results are compiled in Table 2.Table 2Q.In Experiment 2, which of the following combinations of temperature and solvent dissolved the greatest number of moles of NaCl?

Directions:Read the passages and choose the best answer to each question.PassageCertain preservatives known as sulfites are often added to fruit products to keep the fruit fresher longer. Use of sulfites is controversial because studies have linked sulfites to severe reactions in some asthmatics. Students performed 2 experiments to measure sulfite levels.Experiment 1Four solutions, each containing a different amount of sulfite dissolved in H2 O were prepared. A coloring agent was added that binds with sulfite to form a red compound that strongly absorbs light of a specific wavelength, and each solution was diluted to 100 mL. A blank solution was prepared in the same manner, but no sulfite was added. A colorimeter (a device that measures how much light of a selected wavelength is absorbed by a sampl e) was used to measure the absorbance of each solution. The absorbances were corrected by subtracting the absorbance of the blank solution from each reading (see Table 1 and Figure 1).Experiment 2A 100 g fruit sample was ground in a food processor with 50 mL of H2O and the mixture was filtered. The food processor and remaining fruit were then washed with H2O, these washings were filtered, and the liquid was added to the sample solution. The coloring agent was added and the solution was diluted to 100 mL. The procedure was repeated for several fruits, and the absorbances were measured (see Table 2).Q.If Experiments 1 and 2 were repeated using a different coloring agent that produces a different color when it binds with sulfite, which of the following changes in procedure would be necessary?

Directions:Read the passage and choose the best answer to each question.PassagePeople use many different chemicals each day for common household tasks such as cleaning and food preparation.Since the inception of consumer protection laws, chemicals come with toxicity warning labels, directions about proper use, and cautions about the hazards of improper use. Some household chemicals can be quite dangerous, especially when mixed together. One such example is the reaction that occurs when mixing household bleach (NaOCl) with ammonia (NH3). The by-products of the reaction vary depending on the concentrations of the reactants. The following experiments were conducted to determine the levels at which certain by-products resulted from mixing bleach and ammonia.Experiment 1A known by-product of the reaction of bleach and ammonia is chlorine gas (Cl2). Chlorine gas has an intensely disagreeable suffocating odor, and is very poisonous. To determine the quantities of bleach and ammonia that, when mixed together, produce chlorine gas, a varying quantity of bleach was added to eight different ammonia–water solutions and the resulting chlorine gas from each mixture was collected and measured. A solution of 1.0 mole (mol) of NH3 in 1 kg of water was used in each trial. A certain quantity of NaOCl was added to each of the solutions; the amount added was gradually increased for each trial. The amount of chlorine gas produced in each trial was recorded and graphed in Figure 1.Experiment 2Another known by-product of the reaction of bleach and ammonia is nitrogen trichloride (NCl3). Nitrogen trichloride is a yellow, oily, pungent-smelling liquid, often found as a by-product of chemical reactions between nitrogen containing compounds and chlorine. It is highly explosive.To determine the quantities of bleach and ammonia that, when mixed together, produce NCl3, again a varying quantity of bleach was added to eight different ammonia–water solutions and the resulting NCl3 from each mixture was measured. A solution of 1.0 mole (mol) of NH3 in 1 kg of water was used in each trial. A certain quantity of NaOCl was added to each solution; the quantity addedwas gradually increased for each trial. The amount of nitrogen trichloride produced in each trial was recorded in see Table 1.Experiment 3In yet another reaction, bleach and ammonia combined under certain conditions produce a compound known as chloramine. Chloramine (NH2Cl) is a toxic substance commonly used in low concentrations as a disinfectant in municipal water systems as an alternative to chlorination.To determine the mixture of bleach and ammonia at which NH2Cl is produced, a varying amount of ammonia was added to eight different bleach–water solutions and the resulting chlorine gas from each mixture was collected and measured. A solution of 1.0 mole (mol) of NaOCl in 1 kg of water was used in each trial. A certain quantity of NH3 was added to each solution; the quantity of ammonia added was gradually increased for each trial. The amount of chloramine produced in each trial was recorded in Table 2.Q.In Experiment 2, different quantities of NaOCl were added to the ammonia solution resulting in the production of nitrogen trichloride. The amounts of nitrogen trichloride produced for 3.00, 3.50, and 4.00 mol of NaOCl added were approximately the same. Which of the following best explains why the production of NCl3 was limited, based on this observation and the results of the experiment?

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Both the solubility product and ionic product are applicable to all types of solutions.a)trueb)falseCorrect answer is option 'B'. Can you explain this answer?
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