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“Do all substances dissolve?”, : - Coggle Diagram
“Do all substances dissolve?”
What are substances?
A substance is a matter with a distinct composition and contain specific properties that ensure they can't be separated using physical processes into its chemical composition.
What are different types of substances?
Organic Substances
Organic compounds are the basic levels of compounds that contain carbon atoms covalently bonded to hydrogen atoms. Therefore organic compounds are formed from chains of covalently bonded carbon atoms attaches to a hydrocarbon backbone. (3.1: Organic Compounds 2019)
Proteins
Lipids
Carbohydrates
Sugars
Glucose
Surcrose
Starch
fructose
Polymers
Polymers are long chain, giant organic molecules are assembled from many smaller molecules called monomers. Polymers consist of many repeating monomer units in long chains, sometimes with branching or cross-linking between the chains.
Nylon
PVC
Polypropylene
polyethylene
Pure Substances
Examples
Copper
Gold
Oxygen
Diamond
Salt
Baking Sodia
Pure substance is a substance that consists of only one type of atom or one type of molecule. It comes in two forms, elements and compounds, where elements are made up of one type of atom by itself or bonded together to create a molecule. Compuds, are molecules composed of simpler substances and made from more than one atom chemically bonded together.
(Study.com, 2021)
Inorganic Substances
Inorganic comunds are substances that have two or more chemical elements that are usualy other than carbon.
(Inorganic compound | Definition & Examples | Britannica 2023)
Sulfate
Salts
table salt (sodium chloride)
Baking soda
Calcium Carbonate
sodium bisulfate
Acids
Bases
Phosphate
Possible Variables:
Independant Variable
The type of solvent used: For example using different types of solvents including water, methanol, acetone and Benzene at the type of solute used. manipulating the:
Polarity: using different solutes or solvents with different polarities to highlight the relationship between polar and non-polar molecules and how they dissolve.
Temperature: This can be manipulated by testing the solubility of the solution when changing the temperature and if it does affect rate which it can dissolve.
Molecule size: can be measured through choosing different solutes for example sugat with different molecular weight and size. This observes how larger particles are generally less soluble
Method of mixing/ speed
(Factors affecting solubility. What does solubility depend on? 2023)
Dependant Variable
Measuring the solubility of each substance through observing the per cent of substance dissolvec by pre and post-testing.
subjective observations by analysing the mixture for any solute left over in the mixture.
Optimal temperature at which the substance dissolves at
Time to dissolve the substance
Controlled Variable
The type of solvent (if not IV)
The type of solute (if not IV)
Method of meausurment
Person measuing solubility of substance
Location
Number of trials
Mixing time
Volume of the solvent
Mass of the solute
-
Temperature
Equipment used
What does dissolve mean?
What is solubility
Solubility is the extent to which a solute dissolves in a solvent to form a solution. Solubility form new bonds between solute molecules and solvent molecules and is categorised into being highly soluble, sparingly soluble or insoluble. Highly soluble substances will dissolve completely yet other substances with lower solubility, take longer to dissolve and mix with the solvent or not dissolve. (Greene 2022)
Factors that effect solubility: INDEPENDANT VARIABLE
Temperature
As temperatue increases, the solbility between the solute and solvent is effected. For example ionic solids, increaseing the temperauture increases the rate which the solution can be produced. The temperature increases teh kenetic energy, for the particles in the solid move faster, impacting the chances of interacting with more solvent particles thus impacting the amount of solute that can be dissolved. (Greene 2022)
pH
pH affects solubility for ionic compounds with the basic anions, the solubility increases when the pH of the solution decreases, this is more prevalent if the ions in the compound are slightly acidic or basic. For example acid salts are more soluble within basic solutions but less soluble in acidic solutions. Basic salts however are more soluble in acidic solutions and less soluble in basic solutions. Neutral salts however have a solubility that is not effected by any change in the pH levels. (pH Effects on Solubility (Le Chatelier’s Principle) - Chad’s Prep® 2022)
Pressure
Pressure can influence solubility of gases as pressure and solubility are directly related. This means when particle pressure increases, so deos the solubility due to the increased collision frequency. The oppostie effect happens when the pressure decreases.
Polarity
Polarity can affect solubility depending on the bonds and the intermolecular forces between different substances and the molecules. The "like dissolves like" is the term to describe how polar solutes dissolve in polar solutes whilst non-polar solutes dissolve in non-polar solvents. The stronger the intermolecular forces between solute molecules and solvent molecules has greater solubility of the solute in the solvent. (Greene 2022)
Molecular size
Solubility decreases as the molecular size increases as the larger the size of the solute, the harder it is for the solvent molecules to wrap around and dissolve them. Solvent molecules are able to wrap around molecules of smaller size more effectively, increasing the solubility (What factors affect solubility? | AAT Bioquest 2022).
The most effective solvent that dissolves solutes the best is water, a "universal solvent" that contains harmful and postive charges to attract many differnt molecules. The bent structure of water, with the partial positive charges on the hydrogen and partial negative charge on the oxygen, reflect the polar substance's greater electronegativitye. This means that water is good at dissolving polar molecules, and poor at dissolving non-polar molecules. (Khan Academy, 2023)
What is a solute?
The substance that is dissolved in the solvent (fluids) or part of fluid solutions, the solute is present in smaller quantities than the amount of solvent. This produces a homogenous mixture.
. (Helmenstine, 2020)
Examples of Solutes:
Gaseous · Liquid · Solid.
Sadium Chloride (NaCl) and other salts
Sugars
Selected independant variable:
Glucose
-Sucrose
-Starch
Lactose sugar
Gucose
Lactose
Starch
Lactose Sugar
Surcose
Brass ( various metals mixed into copper)
Carbon dioxide in carbonated drinks
Dyes
Calcium Carbonate -CaCO3
Sodium Sulfide
Magnesium Sulfide
Aluminium Sulfide
Heterogeneous vs Homogenous:
Homogenous is uniform in structure as well as composition as the particles are evenly distributed in the solution. Heterogeneous mixtures include a uniform composition and the components of a mixture remain separate from each other(Mazurek 2022)
What is a solvent ?
A solvent is any substance, usually liquid, which is capable of dissolving one or several substances, thus creating a solution. One of the most common examples of solvents is water, which is generally used for dissolving polar molecules. (Solvent Meaning & Definition | EcoOnline, 2023)
Examples:
Solvents can come in gaseous and solid phases, but are most commonly in liquid state. .Polar solvents are made up of molecules containing bonds with atoms that have different electronegativity. Molecules that are non-polar have bonds with similar electronegativity your the same.
Examples of solvents include water (H2O), methanol, acetone, Benzene, and Hexane. (Shafi 2021)
What makes a substance soluble in a solvent?
Dissolve meaning
Dissolving is the process where a solute in a solid, liquid or gaseous stage dissolves in a solvent to forms a solution. Individual solute particles become surrounded and separated by the sovlent particles. (Jue Xi Lu, Tupper & Murray 2022).
Limitations
Solutes or solvents may be haxodous when reacting
Observing solubility can lead to more potential errors (visibility)
Limiitations include how much solute can dissolve within a solvent
(12.3: Solubility Limit and Saturation 2016)
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