SOLUBILITY
The solubility of a substance in a solvent represents the maximum amount of a soluble substance in a solvent. A solubility is generally expressed in grams / L or mol / L.
If some of the salt of the kitchen is dissolved into water and some is insoluble, the solution is a saturated solution. If the NaCl saturated solution is added again NaCl, the added NaCl will precipitate as a NaCl solid. Thus, the concentration of the solution is equal to the solubility of NaCl in water.
If some of the salt of the kitchen is dissolved into water and some is insoluble, the solution is a saturated solution. If the NaCl saturated solution is added again NaCl, the added NaCl will precipitate as a NaCl solid. Thus, the concentration of the solution is equal to the solubility of NaCl in water.
FACTORS AFFECTING THE FIGHT
The amount of solubility of a substance is influenced by several factors, among others:
The amount of solubility of a substance is influenced by several factors, among others:
1. Type of solvent
Polar compounds (having poles of charge) will be readily soluble in polar compounds, such as alcohols and all acids are polar compounds so easily soluble in water which is also a polar compound. In addition to polar compounds, ionic compounds such as NaCl also readily dissolve in water and decompose into ions. Nonpolar compounds will readily dissolve in nonpolar compounds, eg fat soluble in oil. Polar compounds are generally insoluble in nonpolar compounds, such as insoluble alcohols in kerosene.
2. Temperature
The solubility of solids in water will be higher if the temperature is increased. This is due to the heat that will result in the increasing spacing between molecules in the solid. Reducing the distance between molecules in solids molecules makes the force of force between molecules become weak so easily released by the influence of gravity of water molecules. The graph below shows the effect of temperature on the solubility of some solids.
Polar compounds (having poles of charge) will be readily soluble in polar compounds, such as alcohols and all acids are polar compounds so easily soluble in water which is also a polar compound. In addition to polar compounds, ionic compounds such as NaCl also readily dissolve in water and decompose into ions. Nonpolar compounds will readily dissolve in nonpolar compounds, eg fat soluble in oil. Polar compounds are generally insoluble in nonpolar compounds, such as insoluble alcohols in kerosene.
2. Temperature
The solubility of solids in water will be higher if the temperature is increased. This is due to the heat that will result in the increasing spacing between molecules in the solid. Reducing the distance between molecules in solids molecules makes the force of force between molecules become weak so easily released by the influence of gravity of water molecules. The graph below shows the effect of temperature on the solubility of some solids.
In contrast to solids, a rise in temperature will cause the solubility of gas in water to decrease. This is because the increased temperature causes the dissolved gas in the water to be released from water.
Thus the article on solubility, may be useful ... ..
Source:
Sudarmo, U. (2013). CHEMISTRY: For SMA / MA Class XI, Mathematics and Natural Sciences. Erlangga: Jakarta
Thus the article on solubility, may be useful ... ..
Source:
Sudarmo, U. (2013). CHEMISTRY: For SMA / MA Class XI, Mathematics and Natural Sciences. Erlangga: Jakarta
BalasHapusAnything that affects the amount of solubility of a substance?
1 Factors Affecting Solubility
Hapus1.0.1 a. Temperature
1.0.2 b. Concentration
1.0.3 c. Influence of Adding Ion Name
1.0.4 d. Properties of Solvent
1.0.5 e. Effect of pH
1.0.6 f. Effect of Hydrolysis
1.0.7 g. Complex Effects
1.0.8 Ca (OH) 2 (s) ↔ Ca2 + (aq) + 20H- (aq)
A. Temperature
HapusThe rise in temperature will provide an additional energy to disconnect the ions from the electrolyte compound. Therefore, the higher the temperature, the easier the soluble electrolyte.
B. Concentration
The greater concentration of ions present in solution will increase the product of the concentration of ions in the solution. The multiplication of the concentrations of these ions if they are able to pass through the Ksp price, the electrolyte will be easily settled and difficult to dissolve.
C. Influence of Adding Ion Name
Electrolytes consisting of the same metal ions as AgCI, AgNO3, Ag2CrO4, AgBr, and Ag3PO4 are said to have the namesake ion, the silver ion (Ag +). Likewise, AgCI, NaCl, CaCI2, and AICI3 are also said to have ion names ie chloride ions (Cl-).
D. Properties of Solvent
Organic salts are more soluble in water than inorganic salts.
E. Effect of pH
The solubility of salts derived from weak acids depends on the solution. An example of oxalic acid, when dissolved into water will release H + ions and C2O24- ions. The H + ion from water will join the oxalate ion C2O24 - forming oxalic acid back H2C2O4 so as to increase salt solubility.
F. Effect of Hydrolysis
If a salt of a weak acid is dissolved into water, it will produce H + ions so that the amount of H + ions in water increases. The cation of the salt undergoes hydrolysis thus increasing the solubility of the salt.
G. Complex Effects
The solubility of a slightly soluble salt in another solution can produce complex compounds. This complex compound is formed from the salt cation with the central atom of another compound, eg as in the following reaction equation.
AgCI (s) + 2NH4OH (aq) → Ag (NH3) 2CI (aq) + 2H2O (ℓ)
Ag (NH3) 2CI is a complex compound formed from AgCI. AgCI is slightly soluble in water. When AgCI is united with NH4OH form Ag (NH3) 2CI, the solubility of AgCI becomes increased because in the complex the concentration is increased.
An electrolyte, in its solution, forms an equilibrium. The existence of the addition of ion names into the electrolyte solution will result in a shift in equilibrium of ions in the solution toward the formation of molecules again. This shift results in the reduction of ions in the solution. With the fewer ions, the electrolyte is difficult to dissolve.
Example:
Ca (OH) 2 (s) ↔ Ca2 + (aq) + 20H- (aq)
If into the electrolyte there is added a solution having an ionic ion with an OH-ion such as NaOH, the OH-ion concentration will increase. Based on the Le-Chatelier principle, the equilibrium will shift towards the formation of the soluble (OH) 2 molecule of Ca (OH) 2.
The presence of similar ions in solution causes the concentration of one of the ions to increase so that the other ion concentration is more, small. This causes the solubility product equal to its Ksp. Ksp is the maximum limit of the product ion concentration in a soluble saturated electrolyte solution in water.
Hai Iin
BalasHapuswhy Polar compounds (having poles of charge) will be readily soluble in polar compounds??
Polar and non polar compounds
HapusThe characteristics of polar compounds:
Soluble in water and other polar solvents
Have poles + and poles -, due to not
The uniform distribution of electrons
-have a free electron pair (when the molecular shape is known) or have different electronegativity
Example: alcohol, HCl, PCl3, H2O, N2O5
The polar compound is described as
Characteristics of non-polar compounds:
Insoluble in water and other polar solvents
It has no poles + and poles -, consequences
The uniform distribution of electrons
-not have a free electron pair (when the molecular shape is known) or its electronegativity is the same
Example: Cl2, PCl5, H2, N2
Non-polar compounds are described as
QUANTITATIVE SIZE OF THE POINT OF THE CENTRAL COMPOUND
* Polar compound boiling point higher than non-polar compounds
Boiling point sequence, hydrogen bond> dipole-dipole> non polar-non polar or hydrogen bond> Van der Waals> london style
When equally polar / non polar, the bigger Mr. boiling point
For the same Mr. carbon compound, the C chain extends the boiling point> branched chain (round)
DIFFERENCES OF POLAR COMPOUND WITH NON POLAR
POLAR COMPOUND
Can dissolve in water
Has a free electron pair (symmetrical shape)
Ends odd, except BX3 and PX5
Cth: NH3, PCl3, H2O, HCl, HBr, SO3, N2O5, Cl2O5
NON POLAR COMPOUND
Insoluble in water
Have no free electron pairs (symmetrical shape)
Ended even
Cth: F2, Cl2, Br2, I2, O2, H2, N2, CH4, SF6, PCl5, BCl3
Which boiling point is higher?
1. F2 or N2?
2. CH4 or C3H8?
3. H2O or H2S?
4. NH3 or XeF4?
5. HF or HI?
6. PCl5 or PCl3?
7. n-pentane or 2,2-dimethyl propane?
The pair of electrons used together in the formation of a covalent bond between the two nuclei of the atom will be drawn by the two bonded nuclei. The result will affect the distribution of electrons between the two bonded nuclei. The ability to attract electrons toward itself depends on the electronegativity of each bonded element.
8. For elemental molecules, such as H2, Cl2 and N2 the 100 percent covalent bond is covalent. This is because both nuclei have the same ability to draw electrons toward itself, so that the bonding electrons will be distributed evenly between the two nuclei, as shown in Fig. A bond formed with the ability to attract an equally strong pair of electrons is called a non-polar covalent bond.
What is meant by saturated solution
BalasHapusSaturated solution
HapusThat is a solution where the solute is in equilibrium with solid phase. Saturated solution is a solution where the solute (molecule or ion) has a maximum at a certain temperature. For soluble elektroit substances, the saturated solution is characterized by the Ksp value. At a given temperature a saturated solution mixed with an insoluble solute is another example of dynamic equilibrium.