The 16 Solution Pdf

[Jens Loco]

Inchemistry, a solution is a special type of homogeneous mixture composed of two or more substances. In such a mixture, a solute is a substance dissolved in another substance, known as a solvent. If the attractive forces between the solvent and solute particles are greater than the attractive forces holding the solute particles together, the solvent particles pull the solute particles apart and surround them. These surrounded solute particles then move away from the solid solute and out into the solution. The mixing process of a solution happens at a scale where the effects of chemical polarity are involved, resulting in interactions that are specific to solvation. The solution usually has the state of the solvent when the solvent is the larger fraction of the mixture, as is commonly the case. One important parameter of a solution is the concentration, which is a measure of the amount of solute in a given amount of solution or solvent. The term "aqueous solution" is used when one of the solvents is water.[1]

Homogeneous means that the components of the mixture form a single phase. Heterogeneous means that the components of the mixture are of different phase. The properties of the mixture (such as concentration, temperature, and density) can be uniformly distributed through the volume but only in absence of diffusion phenomena or after their completion. Usually, the substance present in the greatest amount is considered the solvent. Solvents can be gases, liquids, or solids. One or more components present in the solution other than the solvent are called solutes. The solution has the same physical state as the solvent.

If the solvent is a gas, only gases (non-condensable) or vapors (condensable) are dissolved under a given set of conditions. An example of a gaseous solution is air (oxygen and other gases dissolved in nitrogen). Since interactions between gaseous molecules play almost no role, non-condensable gases form rather trivial solutions. In the literature, they are not even classified as solutions, but simply addressed as homogeneous mixtures of gases. The Brownian motion and the permanent molecular agitation of gas molecules guarantee the homogeneity of the gaseous systems. Non-condensable gaseous mixtures (e.g., air/CO2, or air/xenon) do not spontaneously demix, nor sediment, as distinctly stratified and separate gas layers as a function of their relative density. Diffusion forces efficiently counteract gravitation forces under normal conditions prevailing on Earth. The case of condensable vapors is different: once the saturation vapor pressure at a given temperature is reached, vapor excess condenses into the liquid state.

Body fluids are examples of complex liquid solutions, containing many solutes. Many of these are electrolytes since they contain solute ions, such as potassium. Furthermore, they contain solute molecules like sugar and urea. Oxygen and carbon dioxide are also essential components of blood chemistry, where significant changes in their concentrations may be a sign of severe illness or injury.

The ability of one compound to dissolve in another compound is called solubility.[clarification needed] When a liquid can completely dissolve in another liquid the two liquids are miscible. Two substances that can never mix to form a solution are said to be immiscible.

All solutions have a positive entropy of mixing. The interactions between different molecules or ions may be energetically favored or not. If interactions are unfavorable, then the free energy decreases with increasing solute concentration. At some point, the energy loss outweighs the entropy gain, and no more solute particles[clarification needed] can be dissolved; the solution is said to be saturated. However, the point at which a solution can become saturated can change significantly with different environmental factors, such as temperature, pressure, and contamination. For some solute-solvent combinations, a supersaturated solution can be prepared by raising the solubility (for example by increasing the temperature) to dissolve more solute and then lowering it (for example by cooling).

Usually, the greater the temperature of the solvent, the more of a given solid solute it can dissolve. However, most gases and some compounds exhibit solubilities that decrease with increased temperature. Such behavior is a result of an exothermic enthalpy of solution. Some surfactants exhibit this behaviour. The solubility of liquids in liquids is generally less temperature-sensitive than that of solids or gases.

The physical properties of compounds such as melting point and boiling point change when other compounds are added. Together they are called colligative properties. There are several ways to quantify the amount of one compound dissolved in the other compounds collectively called concentration. Examples include molarity, volume fraction, and mole fraction.

The properties of ideal solutions can be calculated by the linear combination of the properties of its components. If both solute and solvent exist in equal quantities (such as in a 50% ethanol, 50% water solution), the concepts of "solute" and "solvent" become less relevant, but the substance that is more often used as a solvent is normally designated as the solvent (in this example, water).

In principle, all types of liquids can behave as solvents: liquid noble gases, molten metals, molten salts, molten covalent networks, and molecular liquids. In the practice of chemistry and biochemistry, most solvents are molecular liquids. They can be classified into polar and non-polar, according to whether their molecules possess a permanent electric dipole moment. Another distinction is whether their molecules can form hydrogen bonds (protic and aprotic solvents). Water, the most commonly used solvent, is both polar and sustains hydrogen bonds.

Salts dissolve in polar solvents, forming positive and negative ions that are attracted to the negative and positive ends of the solvent molecule, respectively. If the solvent is water, hydration occurs when the charged solute ions become surrounded by water molecules. A standard example is aqueous saltwater. Such solutions are called electrolytes. Whenever salt dissolves in water ion association has to be taken into account.

Polar solutes dissolve in polar solvents, forming polar bonds or hydrogen bonds. As an example, all alcoholic beverages are aqueous solutions of ethanol. On the other hand, non-polar solutes dissolve better in non-polar solvents. Examples are hydrocarbons such as oil and grease that easily mix, while being incompatible with water.

Example: Make 2 g/100mL of NaCl solution with 1 L water. The density of the resulting solution is considered to be equal to that of water, statement holding especially for dilute solutions, so the density information is not required.

Chemists often make concentrated stock solutions that may then be diluted as needed for laboratory applications. Standard solutions are those where concentrations of solutes are accurately and precisely known.

All the words, pages, roles, activities, and artifacts in SAFe exist for one purpose and one purpose only: to help Agile teams continuously deliver solutions that provide value to the Customer and the Enterprise. In turn, that enables customers to achieve their goals.

To build desirable products that connect with customers and address their needs, solution builders apply a Customer-Centric mindset. Some customers are direct, end-users of the solution. Others are indirect customers who pay for and specify the solution but are not users. To understand and empathize with all customers, Solution builders apply Design Thinking to ensure the solution is desirable to all.

Rapid technology innovations continue to disrupt operational environments. Machines are quickly automating many steps in the Operational Value Stream (OVS), performing them faster and more reliably while reducing costs.

Most organizations build and deliver products in their domains. Automotive companies provide transportation solutions, and banking organizations offer financial solutions. However, digital disruption allowed businesses to enter and disrupt new markets. For example, Apple outsold the entire Swiss watch industry just four years after launching the Apple Watch. To compete in the digital age, organizations must have the technical knowledge to build innovative solutions and evolve them to meet changing customer and market demands rapidly.

Building innovative solutions require a diverse range of skills and technical resources. Organizations need the right technical teams, strategic relationships with the right partners, and economic models that ensure that solutions remain feasible over their lifecycles.

To leverage values and practices that continually encourage individuals to increase their knowledge and competence, Lean-Agile enterprises adopt a Continuous Learning Culture. Organizations may partner with suppliers, cultivate competence internally, or both, to fill in gaps. Partnering with suppliers brings domain knowledge, practical experience, and pre-existing solution components to the teams. Note: Organizations are less likely to partner when the supply chain innovates too slowly to support the business strategy or the technology is strategically important. In these cases, competence is developed internally through training, hiring, and strategic acquisition.

Modular designs that communicate through defined interfaces allow ARTs and teams to evolve their parts of the solution independently and accelerate value delivery. Some solutions provide direct value to an end-user; others are modules (also called components or subsystems) that are parts of a larger solution. Solutions are often built from other solutions to help accelerate value delivery, reduce development costs, and improve quality. Those other solutions come from various sources, including internal and external suppliers and open-source communities (Figure 3).

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