Scientists mix 100 milliliters of hexane with 100 milliliters of water. Why is this the case? (A) Because hexane molecules are heavy and water molecules are light

(C) Because hexane molecules and water molecules are both nonpolar. (D) Because hexane molecules are nonpolar and water molecules are polar

In this question, we must explain why hexane and water are not miscible. Miscible means forming a homogeneous mixture when added together

Solutions are homogeneous mixtures of two or more pure substances. For our purposes, we will generally be discussing solutions containing a single solute and water as the solvent

That is to say if you had a liter of salt and 2 grams of water. In that case, the salt would be the solvent and the water the solute

When we do place solutes and solvents together, there is what we call the solution process. You can think of it as being similar to what you would experience if you tried to squeeze into an already packed elevator

Questions 1-10 Questions 11-20 Questions 21-30 Questions 31-40 Questions 41-50. 42 Hexane (C 6 H 14 ) and water do not form a solution

Which arrow represents the activation energy of the forward reaction?. 47 Which ion has the same electron configuration as an atom of He?

NaOH base, so it conducts electricity well and turns pht. Questions 1-10 Questions 11-20 Questions 21-30 Questions 31-40 Questions 41-50

Solutions are homogeneous mixtures of two or more pure substances. For our purposes, we will generally be discussing solutions containing a single solute and water as the solvent

That is to say if you had a liter of salt and 2 grams of water. In that case, the salt would be the solvent and the water the solute

When we do place solutes and solvents together, there is what we call the solution process. You can think of it as being similar to what you would experience if you tried to squeeze into an already packed elevator

|Unit I: Atoms Unit II: Molecules Unit III: States of Matter Unit IV: Reactions Unit V: Kinetics & Equilibrium. Unit VI: Thermo & Electrochemistry Unit VII: Nuclear Chemistry

When a solute dissolves, its individual atoms, molecules, or ions interact with the solvent, become solvated, and are able to diffuse independently throughout the solution (part (a) in Figure 9.2.1). If the molecule or ion happens to collide with the surface of a particle of the undissolved solute, it may adhere to the particle in a process called crystallization

(For more information about vapor pressure, see Section 7.4) We can represent these opposing processes as follows:. \( solute+solvent \rightleftharpoons crystallization \; dissolution \; solution \tag{9.2.1} \)

We explored the general properties of gases, liquids, and solids in Chapter 10 “Gases”, Chapter 11 “Liquids”, and Chapter 12 “Solids”, respectively. Most of the discussion focused on pure substances containing a single kind of atom, molecule, or cation–anion pair

Some are heterogeneous mixtures, which consist of at least two phases that are not uniformly dispersed on a microscopic scale; others are homogeneous mixtures, consisting of a single phase in which the components are uniformly distributed. (For more information about homogeneous mixtures, see Chapter 1 “Introduction to Chemistry”, Section 1.3 “A Description of Matter”.) Homogeneous mixtures are also called solutionsA homogeneous mixture of two or more substances in which the substances present in lesser amounts (the solutes) are dispersed uniformly throughout the substance present in greater amount (the solvent).; they include the air we breathe, the gas we use to cook and heat our homes, the water we drink, the gasoline or diesel fuel that powers engines, and the gold and silver jewelry we wear.

Oil is insoluble in water because the intermolecular interactions within the solute (oil) and the solvent (water) are stronger than the intermolecular interactions between the solute and the solvent.. Many of the concepts that we will use in our discussion of solutions were introduced in earlier chapters

An understanding of bond dipoles and the various types of noncovalent intermolecular forces allows us to explain, on a molecular level, many observable physical properties of organic compounds. In this section, we will concentrate on solubility, melting point, and boiling point.

In the organic laboratory, reactions are often run in nonpolar or slightly polar solvents such as toluene (methylbenzene), hexane, dichloromethane, or diethylether. In recent years, much effort has been made to adapt reaction conditions to allow for the use of ‘greener’ (in other words, more environmentally friendly) solvents such as water or ethanol, which are polar and capable of hydrogen bonding

It is critical for any organic chemist to understand the factors which are involved in the solubility of different molecules in different solvents.. You probably remember the rule you learned in general chemistry regarding solubility: ‘like dissolves like’ (and even before you took any chemistry at all, you probably observed at some point in your life that oil does not mix with water)

Solutions are homogeneous mixtures of more than one substance. The word homogeneous implies that the mixture is a single phase where the properties will be the same no matter where a sample is taken.

If we can see through the mixture (Clear) then it is most likely a single phase, which means a solution. If the mixture is opaque then there are likely two or more phases that do not mix with each other and hence, scatter the light, making it cloudy

We can see this better if we leave unhomogenized milk sit a while. The cream (oils) will rise to the top, leaving a more translucent liquid (mostly water with some suspended solids, called butter milk) below

A solvent (from the Latin solvō, “loosen, untie, solve”) is a substance that dissolves a solute, resulting in a solution. A solvent is usually a liquid but can also be a solid, a gas, or a supercritical fluid

Major uses of solvents are in paints, paint removers, inks, and dry cleaning.[2] Specific uses for organic solvents are in dry cleaning (e.g. tetrachloroethylene); as paint thinners (toluene, turpentine); as nail polish removers and solvents of glue (acetone, methyl acetate, ethyl acetate); in spot removers (hexane, petrol ether); in detergents (citrus terpenes); and in perfumes (ethanol)

When one substance is dissolved into another, a solution is formed.[3] This is opposed to the situation when the compounds are insoluble like sand in water. In a solution, all of the ingredients are uniformly distributed at a molecular level and no residue remains

In chemistry, 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

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

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]

A colligative property is a property of a solution that is dependent on the ratio between the total number of solute particles (in the solution) to the total number of solvent particles. Colligative properties are not dependent on the chemical nature of the solution’s components

The four colligative properties that can be exhibited by a solution are given below:. The word “colligative” has been adapted or taken from the Latin word “colligatus” which means “bound together”

A dilute solution containing non-volatile solute exhibits some properties which depend only on the number of solute particles present and not on the type of solute present. These properties are called colligative properties, and they are mostly seen in dilute solutions.

iRespond Question F Multiple Choice A.) K+ is the solute and Cl- is the solvent B.) Cl- is the solute and K+ is the solvent C.) KCl is the solute and water is the solvent D.) Water is the solute and KCl is the solvent E.). At STP, which of these substances is most soluble in H2O?

The solubility of KClO3(s) in water increases as the. iRespond Question Multiple Choice Solids are more soluble at higher temperatures, which is why you use hot water when washing dishes A.) temperature of the solution increases B.) temperature of the solution decreases C.) pressure on the solution increases D.) pressure on the solution decreases E.) Pressure does not effect the solubility of solids

iRespond Question F Multiple Choice A.) decreases B.) increases C.) remains the same D.) Increasing pressure makes gases more soluble, just like putting a cap on a bottle of soda keeps is carbonated longer E.). Which statement explains this phenomenon? iRespond Question F Multiple Choice A.) Hexane is polar and water is nonpolar