PRACTICAL REPORT OF DEVELOPMENT LABORATORY
SOLUTION
Lecture: Purwanti Widhy
Arranged by:
Tri Sulis Setyowati (09312241027)
C. Nulat Panggayuh (09312241035)
Sunjani (09312244033)
M. Ihzatul Faqih (09312244025)
Endah Dani (09312244034)
SCIENCE EDUCATION PROGRAM
MATHEMATICS AND SCIENCE FACULTY
YOGYAKARTA STATE UNIVERSITY
2010
SOLUTION
I. Purpose
Knowing how to make a solution
II. Basic theory
Solution is a homogenous mixture. A mixture is said homogeneous if there is no field of inter-component boundaries so that no longer distinguishable despite using ultra microscope. In addition, the homogenous mixture has the same composition in each part.
Solution consisting of solvent (solvent) and solutes (solutes). Typically, the most amount component which is considered as a solvent, but if the liquid solution, then the fluid is considered as a solvent. For example syrup, which is a mixture that contains more sugar than water, is considered as a solution in the sugar.
Solution concentration is the amount of solute contained in a certain amount of solution. Molarity concentration expressed as the number of moles of solute in 1 L solution. Dilution is the process of adding solvent to a solution, which will reduce the concentration (molarity) solution without changing the total number of moles of solute contained in the solution.
In chemistry, a solution is a homogeneous mixture consisting of two or more substances. A smaller number of substances in solution is called (substances) dissolved or solutes, whereas substances that amount more than other substances in solution is solvent or solvents. The composition of the solute and solvent in solution is expressed in concentration of the solution, while the mixing process of the solute and solvent form a solution is called dissolution or solvation. Example of a common solution is the solids dissolved in liquids, such as salt or sugar dissolved in water. Gas also can be dissolved in a liquid, such as carbon dioxide or oxygen in the water. In addition, the fluid can also be dissolved in another liquid, while gas dissolved in another gas. There is also a solid solution, such as alloy (mixed metal) and certain minerals. Concentration Solution concentration expressed in quantitative composition of the solute and solvent in the solution. Concentrations are usually expressed in comparison with the amount of the total amount of solute substance in solution, or in comparison with the total amount of solute solvent. Examples of some unit of concentration is a molar, molal, and parts per million (parts per million, ppm). Meanwhile, qualitatively, the composition can be expressed as a dilute solution (low concentration) or concentrated (high concentration).
Dissolution
Sodium ion solvated by water molecules. Molecular components interact directly in a state of solution mixed. In the process of dissolution, the pull of pure component between particle fragmented and replaced with the attraction between the solvent with the solute. Especially if the solvent and solute are both polar, will form a solvent structure around the solute; this allows the interaction between the solute and solvent remained stable.
When the solute component is added continuously into the solvent, at a point component that is added will not be late again. For example, if the substance fused a solid and a liquid solvent, at some point can not be dissolved solids again and formed sediment. The amount of solute in the solution is maximal, and the solution was called as a saturated solution. The point of the achievement of being saturated solution is strongly influenced by various environmental factors, such as temperature, pressure, and contamination. In general, the solubility of a substance (ie the amount of a substance that can be dissolved in certain solvents) is proportional to the temperature. This is especially true in solids, although there are exceptions. Liquid solubility in other liquids are generally less sensitive to temperature than the solubility of solids or gases in liquids. Gas solubility in water is generally inversely proportional to temperature.
Ideal solution
When the intermolecular interaction of components of the solution together with intermolecular interaction components in pure state, it becomes an idealization that is called an ideal solution. Ideal solution obey the Raoult law, namely that the vapor pressure of solvent (liquid) with a straight right versus mole fraction of solvent in the solution. Solution is really ideal does not exist in nature, but some solutions meet the Raoult law to certain limits. Examples which may be considered ideal solution is a mixture of benzene and toluene.
Another feature is that the volume is an ideal solution is an appropriate summation of the volume of constituent components. In non-ideal solution, the sum of the volume of pure solute and pure solvent is not the same with the volume of the solution.
Another feature is that the volume is an ideal solution is an appropriate summation of the volume of constituent components. In non-ideal solution, the sum of the volume of pure solute and pure solvent is not the same with the volume of the solution.
Nature koligatif solution
Dilute aqueous solution shows properties that depend on the collective effect of the number of solute particles, called koligatif properties (from the Latin word colligare, "gather together"). Koligatif properties include vapor pressure drop, increasing the boiling point, freezing point depression, and symptoms of osmotic pressure.
Types of solution
Solution can be classified for example according to the phase of the solute and solvent. The following table shows examples of solutions based on the phase components.
Sample solution of dissolved substances
Sample solution of dissolved substances
Solid Liquid GasSolvents Air Gases (oxygen and other gases in nitrogen)
Water vapor in the air (humidity)
The smell of a solid arising from the dissolution of these solids in the air molecules
Carbonated water fluid (carbon dioxide in water) ethanol in water; a mixture of various hydrocarbons (petroleum)
Sucrose (sugar) in water, sodium chloride (table salt) in water; gold in mercury amalgam
Solid hydrogen is soluble in metals, such as platinum
Water in the active charcoal; moisture in wood
Alloy metals such as steel and duralumin
Based on its ability to conduct electricity, a solution can be distinguished as a solution of electrolyte and non-electrolyte solution. Electrolyte solution containing an electrolyte that can conduct electricity, while the non-electrolyte solution can not conduct electricity.
Solution is a homogeneous mixture (same composition), all the same (particle size), there is no boundary between the solvent with the solute (can not distinguish directly between the solvent-solute), the constituent particles of the same size (both ions, atoms, or molecules) from two or more substances. In the liquid phase solution, the solvent (solvent) is a liquid, and dissolved substances in it called solutes (solutes), can form solid, liquid, or gas. Thus, the solution = solvent (solvent) + solutes (solutes). Especially for the liquid solution, the solvent is the largest volume.
There are 2 reactions in solution, namely:
a. exothermic, the process releases heat from the system to the environment, the temperature of the reaction mixture will rise and the potential energy of chemical substances in question will fall.
b. endothermic, which absorbs heat from the environment into the system, the temperature of the reaction mixture will decrease and the potential energy of chemical substances in question will rise.
Solution can be divided into 3, namely:
a. An unsaturated solution is a solution containing solutes (solute) is less than that required to make a saturated solution. Or in other words, the solution of which the particles are not exactly run out to react with the reagent (still can dissolve substances). Unsaturated solution when the time occurs when the ion concentration
b. Saturated solution is a solution containing a number of solutes which dissolve and hold equilibrium with solid solute. Or in other words, the solution of which the particles are exhausted to react with appropriate reagents (substances with a maximum concentration). Saturated solution occurs when when the ion concentration = Ksp appropriate means saturated solution.
c. The solution was saturated (too saturated) is a solution that contains more solutes than is necessary for the solution saturated. Or in other words, the solution can no longer dissolve the solute resulting in sediment. Highly saturated solution occurs when the ion concentration when the product> Ksp means supersaturated solution (precipitate).
Based on the extent of the solute, the solution can be divided into 2, namely:
a. The concentrated solution is a solution containing relatively more solutes than the solvent.
b.Aqueous solution is a solution of relatively fewer solutes than the solvent. In a solution, the solvent can be water and without water.
Concentration of Solution
Concentration of the solution can be distinguished qualitatively and quantitatively. Qualitatively, the solution can be divided into a concentrated solution and dilute solution. In dilute solution, a solution of mass equals the mass of the solvent because of the density of the solution equal to the density of the solvent. Quantitatively, solution concentration is distinguished by the unit. There are several dissolution process (principle of solubility), namely:
a. Fluids
Liquid solubility in liquids is often stated "Like dissolver like" meaning liquid substances which have similar structures will be mutually dissolve each other in every comparison. Examples: hexane and pentane, water and alcohol => H-OH with C2H5-OH. Polarity difference between the solute and solvent effect is not big on solubility. For example: CH3Cl (polar) with CCl4 (non-polar). The solution is due to the occurrence of inter-action style, through dispersion forces (the events in the spread of the solute in solvent) is strong. Here solution events, namely the events surrounding solvent particles (confined) particles dissolved. For the solubility of the liquids is influenced also by hydrogen bonding.
b.Solid-liquid.
Solids generally have limited solubility in this fluid due to attractive force between molecules solids with solids> solids with liquids. Solids non-polar (slightly polar) great solubility in low polarity liquid. Examples: DDT has a structure similar to DDT CCl4 so easy to dissolve in non-polar (eg coconut oil), not easily soluble in water (polar).
c. Gas-liquid
There are 2 principles that affect the solubility of gases in liquids, namely:
The higher the melting point of a gas, liquid has come closer to an attractive force between molecules. Gas with higher melting point, solubility is greater.
The best solvent to a gas is an attractive force between the solvent molecules are very similar to the one owned by a gas. The boiling point of the noble gases from the top down in a periodic system, the higher, and greater solubility.
Effect of temperature (T) and pressure (P) against the solubility, ie temperature increase profitable endothermic process, whereas temperature lowering favorable exothermic process. The process of solid solubility in liquids generally lasts endothermic solubility consequently raise the temperature rise. The process of gas solubility in liquid lasted exothermic effect increases temperature lower solubility.
There are 2 principles that affect the solubility of gases in liquids, namely:
The higher the melting point of a gas, liquid has come closer to an attractive force between molecules. Gas with higher melting point, solubility is greater.
The best solvent to a gas is an attractive force between the solvent molecules are very similar to the one owned by a gas. The boiling point of the noble gases from the top down in a periodic system, the higher, and greater solubility.
Effect of temperature (T) and pressure (P) against the solubility, ie temperature increase profitable endothermic process, whereas temperature lowering favorable exothermic process. The process of solid solubility in liquids generally lasts endothermic solubility consequently raise the temperature rise. The process of gas solubility in liquid lasted exothermic effect increases temperature lower solubility.
Dissolution process is considered the equilibrium
III. Tools and Materials
- Measuring cup
- Balance analytical
- Glass watches
- Pipette drops
- Beaker glass
IV. Work Steps
a. Make 100 ml of HCl 37 % 2 M
Known:
ρHCl : 1,16 kg/L = 1,16 *1000 g/L
Mr HCl: 36,5
So,
nHCl 37% = (0,37 * 1,16 * 1000) / ( 36,5)
= 11,76 mol.
M HCl 37% per Liter = (11,76 mol)/(1L)
= 11,76 M
To make HCl 2M for the quantity of 100 mL is :
V1.M1 = V2.M2
11,76 M. V1 = 2M. 100 mL
V1 = ( 2M.100 mL ) / (11,76M)
= 17,01 mL.
1. Take 17,01 ml of HCl 11,76 M with a pipette
2. Enter in a measuring cup
3. Add the water, until the volume to 100 ml
b. Make 25 ml of HCl 0.1 M of HCl 2 M
V . M = V’ . M’
V = 0,025 L
M = 0,1 M
M’ = 2 M
0,025 L . 0,1 M = V’ . 2 M
0,0025 = 2 V’
0,00125 L = V’
V’ = 1,25 ml
1. Take 1.25 ml of HCl 2 M with a pipette
2. Enter in a measuring cup
3. Add the water, until the volume to 25 ml
c. Make 25 ml of NaOH 1 M
Mr NaOH = 23+16+1 = 40
volume NaOH = 25 mL = 0,025 L
mol
Molaritas = ---------------
volume NaOH = 25 mL = 0,025 L
mol
Molaritas = ---------------
volume
mol NaOH = molaritas x volume = 1 x 0,025 = 0,025 mol
massa
mol = --------------
Mr
massa = mol x Mr = 0,025 x 40 = 1 gram
mol NaOH = molaritas x volume = 1 x 0,025 = 0,025 mol
massa
mol = --------------
Mr
massa = mol x Mr = 0,025 x 40 = 1 gram
1. Consider 1 gram of NaOH with balance analytical
2. Input it to the measure cup
3. Add the water, until the volume to 25 ml
d. Make 25 ml of NaCl 0,5 M
c = n / V
c = molarity (M)
n = mol
V = volume (L)
n(NaCl) = c(NaCl) x V(NaCl) = 0.5 M x (25/1000)L
n(NaCl) = 0.0125 mol
So, use the formula;
n = m / M
n = mol
c = molarity (M)
n = mol
V = volume (L)
n(NaCl) = c(NaCl) x V(NaCl) = 0.5 M x (25/1000)L
n(NaCl) = 0.0125 mol
So, use the formula;
n = m / M
n = mol
m = mass (g)
M = molar
m(NaCl) = n(NaCl) x M(NaCl) = 0.0125 mol x 58.5 gmol^-1
m(NaCl) = n(NaCl) x M(NaCl) = 0.0125 mol x 58.5 gmol^-1
m (NaCl) = 0,73125 g
1. Consider 0,73125 gram of NaCl with balance analytical
2. Input it to the measure cup
3. Add the water, until the volume to 25 ml
V. Data
Solution of Solution of
Solution of
VI.Discussion
Pada praktikum pembuatan larutan ini, bertujuan untuk mengetahui cara pembuatan larutan. Diantaranya larutan HCl 37 % 2 M, HCl 0.1 M, NaOH 1 M, dan NaCl 0,5 M. namun karena di laboratorium tidak tersedia HCl pekat maka dalam pelaksanaan praktikum tidak dibuat HCl 37% 2 M. Solution is a homogenous mixture. A mixture is said homogeneous if there is no field of inter-component boundaries so that no longer distinguishable despite using ultra microscope. In addition, the homogenous mixture has the same composition in each part.
Larutan pertama yang dibuat adalah HCl 0,1 M, yang dibuat dari HCl 2 M. dengan langkah kerja sebagai berikut take 1.25 ml of HCl 2 M with a pipette, and then enter in a measuring cup and add the water, until the volume to 25 ml. Prinsip yang digunakan pada pembuatan larutan ini adalah pengenceran, dimana yang digunakan sebagai bahan pembuatan larutan adalah larutan yang sama namun memiliki molalitas yang lebih besar, untuk menentukan banyaknya HCl @ m yang dibutuhkan, kita perlu menggunakan persamaan sebagai berikut,
V . M = V’ . M’
V = 0,025 L
M = 0,1 M
M’ = 2 M
0,025 L . 0,1 M = V’ . 2 M
0,0025 = 2 V’
0,00125 L = V’
V’ = 1,25 ml
Dari persamaan dia atas kita dapat menentukan banyaknya HCl 2 M yang dibutuhkan, yaitu sebanyak 1,25 ml.
HCl 2 M HCl 0,1 M
Larutan kedua yang dibuat adalah 25 ml of NaOH 1 M, dengan langkah kerja sebagai berikut consider 1 gram of NaOH with balance analytical, then input it to the measure cup and add the water, until the volume to 25 ml. penentuan banyaknya NaOH yang digunakan, berdasarkan pada rumus berikut,
Mr NaOH = 23+16+1 = 40
volume NaOH = 25 mL = 0,025 L
mol
Molaritas = ---------------
volume NaOH = 25 mL = 0,025 L
mol
Molaritas = ---------------
volume
mol NaOH = molaritas x volume = 1 x 0,025 = 0,025 mol
massa
mol = --------------
Mr
massa = mol x Mr = 0,025 x 40 = 1 gram
mol NaOH = molaritas x volume = 1 x 0,025 = 0,025 mol
massa
mol = --------------
Mr
massa = mol x Mr = 0,025 x 40 = 1 gram
Dari persamaan di atas kita dapat menentukan bahwa untuk membuat 25 ml of NaOH 1 M dibutuhkan 1 gram NaOH padat.
NaOH padat
Larutan terakhir yang dibuat adalah 25 ml of NaCl 0,5 M, dengan langkah kerja sebagai berikut pertama consider 0,73125 gram of NaCl with balance analytical, then input it to the measure cup and add the water, until the volume to 25 ml. Dalam penentuan banyaknya NaCl yang dibutuhkan dalam pembuatan larutan ini, kita menggunakan persamaan berikut,
c = n / V
c = molarity (M)
n = mol
V = volume (L)
n(NaCl) = c(NaCl) x V(NaCl) = 0.5 M x (25/1000)L
n(NaCl) = 0.0125 mol
So, use the formula;
n = m / M
n = mol
c = molarity (M)
n = mol
V = volume (L)
n(NaCl) = c(NaCl) x V(NaCl) = 0.5 M x (25/1000)L
n(NaCl) = 0.0125 mol
So, use the formula;
n = m / M
n = mol
m = mass (g)
M = molar
m(NaCl) = n(NaCl) x M(NaCl) = 0.0125 mol x 58.5 gmol^-1
m(NaCl) = n(NaCl) x M(NaCl) = 0.0125 mol x 58.5 gmol^-1
m (NaCl) = 0,73125 g
Dari persamaan di atas dapat kita tentukan banyaknya NaCl yang dibutuhkan, yaitu sebanyak 0,73125 g.
NaCl powder
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