Concentration of solution
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A saturated solution contains as much solute as can dissolve at a given temperature, an unsaturated solution contains less, and a super-saturated solution contains more. The maximum amount of solute that can dissolve in a specified amount of solvent at a set temperature is known as the solute's solubility in that solvent at that temperature. Solubility is expressed as the amount of solute that dissolves in 100 grams of solvent. The concentration of a solution refers to the amount of solute present in a given quantity of the solution and can be expressed as a percentage by mass or volume.
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Solution concentration
This document discusses key concepts related to solution concentration including:
- Solutions are homogeneous mixtures with a solvent as the major component and solute as the minor component.
- Concentration can be expressed in various ways such as percentage by weight or volume, molarity, and parts per million or billion.
- Dilute solutions have low concentrations while concentrated solutions have high concentrations.
- Molarity calculations allow converting between moles, liters, and grams of solutes and solvents in solutions.
- Dilution decreases concentration by adding more solvent while maintaining the same amount of solute.
Molarity
This document discusses molarity, which is defined as the number of moles of solute per liter of solution. Molarity is calculated by taking the moles of solute and dividing by the total liters of solution. The document provides an example calculation of molarity using 0.40 moles of NaCl dissolved in 0.250L of water, and gives a sample problem of calculating the molarity of 58.44 grams of NaCl dissolved in 2.00L of solution. Two practice problems are included at the end to test the reader's understanding of calculating molarity.
MOLARITY
Molarity is a measurement that expresses the concentration of a solute in a solution as moles of solute per liter of solution. It is calculated by taking the moles of solute and dividing by the total liters of solution. Several examples are provided to demonstrate how to calculate molarity from mass, moles, or volume information and how to determine moles or mass of a solute given the molarity and volume of a solution.
Chemistry of solutions
This document discusses chemistry of solutions. It defines key terms like solute, solvent and solution. It explains that a solution is a homogeneous mixture of two or more substances. The solute is dispersed uniformly throughout the solvent. Factors that affect solubility are also discussed, like temperature, pressure, molecular size and polarity. Henry's law is introduced, which states that the solubility of a gas is directly proportional to its partial pressure.
Molarity vs Molality
Molarity vs Molality What is molarity? Molarity is also known as molar concentration, it is the ratio of moles of substance to volume in liter. Where mole is weight in gram divided by molecular weight. Molarity is chemistry terminology. Molarity... read more at https://chemistrynotesinfo.com/molarity-vs-molality/
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Molarity and dilution
The document discusses molarity, which is a measurement of concentration that expresses the number of moles of solute per liter of solution. It provides examples of calculating molarity when given the mass of a solute and volume of solution. It also covers diluting solutions, where the moles of solute stay the same but the concentration decreases as volume increases. Molarity can be used to determine the moles, mass, or volume of a solution component when any two pieces of information are known.
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Solution concentration
This document discusses key concepts related to solution concentration including:
- Solutions are homogeneous mixtures with a solvent as the major component and solute as the minor component.
- Concentration can be expressed in various ways such as percentage by weight or volume, molarity, and parts per million or billion.
- Dilute solutions have low concentrations while concentrated solutions have high concentrations.
- Molarity calculations allow converting between moles, liters, and grams of solutes and solvents in solutions.
- Dilution decreases concentration by adding more solvent while maintaining the same amount of solute.
Molarity
This document discusses molarity, which is defined as the number of moles of solute per liter of solution. Molarity is calculated by taking the moles of solute and dividing by the total liters of solution. The document provides an example calculation of molarity using 0.40 moles of NaCl dissolved in 0.250L of water, and gives a sample problem of calculating the molarity of 58.44 grams of NaCl dissolved in 2.00L of solution. Two practice problems are included at the end to test the reader's understanding of calculating molarity.
MOLARITY
Molarity is a measurement that expresses the concentration of a solute in a solution as moles of solute per liter of solution. It is calculated by taking the moles of solute and dividing by the total liters of solution. Several examples are provided to demonstrate how to calculate molarity from mass, moles, or volume information and how to determine moles or mass of a solute given the molarity and volume of a solution.
Chemistry of solutions
This document discusses chemistry of solutions. It defines key terms like solute, solvent and solution. It explains that a solution is a homogeneous mixture of two or more substances. The solute is dispersed uniformly throughout the solvent. Factors that affect solubility are also discussed, like temperature, pressure, molecular size and polarity. Henry's law is introduced, which states that the solubility of a gas is directly proportional to its partial pressure.
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Molarity vs Molality What is molarity? Molarity is also known as molar concentration, it is the ratio of moles of substance to volume in liter. Where mole is weight in gram divided by molecular weight. Molarity is chemistry terminology. Molarity... read more at https://chemistrynotesinfo.com/molarity-vs-molality/
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
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The document discusses molarity, which is a measurement of concentration that expresses the number of moles of solute per liter of solution. It provides examples of calculating molarity when given the mass of a solute and volume of solution. It also covers diluting solutions, where the moles of solute stay the same but the concentration decreases as volume increases. Molarity can be used to determine the moles, mass, or volume of a solution component when any two pieces of information are known.
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This document discusses concentration of solutions in chemistry. It defines molarity as moles of solute per liter of solution. It provides an example problem calculating the molarity of a solution made by dissolving 5 grams of nickel chloride hexahydrate in 250 mL of water. It also discusses molality, defined as moles of solute per kilogram of solvent, and provides an example problem calculating the molality of a sodium chloride solution. Finally, it discusses the process of diluting solutions through calculations that conserve the number of moles while changing the volume.
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This document discusses key properties and concepts related to solutions. It defines a solution as being made up of a solvent and one or more solutes. The solvent is the substance that exists in the greatest quantity, while solutes are all other substances present. Solutions can be solid, liquid or gas depending on the state of the solvent. The document also discusses concentration, solubility, factors that affect solubility like temperature and pressure, and how to increase the rate at which a solute dissolves.
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Solution
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
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This document defines pure substances and mixtures. A pure substance is homogeneous and has definite properties, while a mixture contains two or more substances mixed together without chemical change. Solutions are homogeneous mixtures where particle size is molecular. Suspensions are heterogeneous mixtures where particle size is larger, allowing settling. Colloids have intermediate particle sizes that do not settle. The document discusses types of mixtures and their distinguishing characteristics.
Metals and non_metals
The document discusses the differences between metals and non-metals. It states that metals account for about two thirds of all elements and 24% of Earth's mass. Metals have properties like strength, conductivity, and high melting points. Non-metals do not conduct electricity or heat well and are very brittle. Non-metals exist as gases and solids at room temperature, unlike metals which are typically solid, and do not have a metallic luster. The document then provides a table comparing various properties of metals and non-metals.
Physical & chemical changes
A physical change alters physical properties like state, texture, or color but does not change molecular composition, and can typically be reversed. A chemical change alters molecular composition to form new substances and cannot be reversed. Examples of physical changes include loss of water of crystallization and melting of candle wax. Examples of chemical changes include burning of magnesium ribbon and formation of curds from milk.
Purification of water
The document discusses water purification methods used by city water works. It describes the process of removing undesirable chemicals, biological contaminants, suspended solids, and gases from contaminated water to produce drinking water. Common purification methods include physical processes like filtration and sedimentation, biological processes such as slow sand filters, chemical processes like chlorination, and electromagnetic radiation such as ultraviolet light. Sedimentation is used in potable water treatment to allow particles to group into larger flocs that settle faster, removing suspended solids and settling colloids.
Reflection of light
Reflection is defined as light bouncing back into the same medium when it strikes a surface. The image formed by a plane mirror is virtual, erect, and the same size as the object. The image does not appear different from the object and is located behind the mirror.
Compound n mixture
A compound is a pure chemical substance consisting of two or more elements chemically combined in a fixed ratio. A compound has a homogeneous structure and properties that are different from its constituent elements. In contrast, a mixture is made up of two or more substances mixed together without chemical bonding. The constituents of a mixture can be separated physically and retain their original properties. Mixtures have a heterogeneous structure and the ratio of constituents can vary.
Polynomials review
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Concentration of solution
- 1. Saturated solution:- A solution, which at a given temperature dissolves as much solute as it is capable of dissolving is said to be a saturated solution. Unsaturated solution:- When the amount of solute contained in a solution is less than the saturation level, the solution is said to be an unsaturated solution. Super-saturated solution:-A solution which contains more of the solute than required to make a saturated solution is called a super- saturated solution.
- 2. The maximum amount of a solute which can be dissolved in 100gms of a solvent at a specified temperature is known as the solubility of that solute in that solvent at that temperature. While expressing the solubility of a substance , we have to specify the temperature also.
- 3. Problem on solubility:- 12gms of potassium sulphate dissolves in 75gms of water at 600C. What is its solubility in water at that temperature. Amount of solute X 100 Solubility = Amount of solvent = 12 x100 75 = 16gms
- 4. Concentration of a solution It is defined as the amount of solute in a given quantity of the solution .it is expressed in percentage of solute in the solvent . Concentration of solution in terms of mass of solute : Concentration of solution = mass of solute in grams x 100 mass of solution in grams Concentration of solution in terms of volume of solute : Concentration of solution = volume of solute in ml x 100 volume of solution in ml
- 5. Concentration of a solution •A solution is made by dissolving 25g of sugar in 175g of water. Calculate the concentration of sugar solution. •A solution is made by dissolving 50g of potassium nitrate in 250 g of water. Calculate the concentration of potassium nitrate solution. •How much water should be added to 50g of glucose, so as to obtain 12% glucose solution? •How much water should be added to 80g of common salt, so as to obtain 20% salt solution?
- 6. •A solution contains 50ml of acetic acid and 250ml of water. Calculate the percentage (by volume) of acetic acid. •Calculate the mass by volume percentage of copper sulphate if 20g of copper sulphate is present in 250ml of solution. •A solution contains 30g of glucose and 20g of sugar in 500ml of water. Calculate the mass percent of glucose and sugar.( density of water= 1g/ml) •During an experiment the students were asked to prepare a 10% solution of sugar in water. Ramesh dissolved 10g in 100g of water while Sarika prepared by dissolving 10g of sugar in water to make 100g of solution •Are the two solution of the same concentration •Compare the mass % concentration of the two solution.