report

Title: Electrolyte and nonelectrolyte solutions
Day / Date: Monday, 6 february 2017
Objective: 1.  can observe electrical conductivity symptoms of various solutions in water.
                    2. Can Know any solution that has the ability to light up.

Benefits: 1. to be able to observe electrical conductivity symptoms of various solutions in water.
                 2. to be able to know which solutions have the ability to light up.


Theoretical basis

The solution is a homogeneous mixture of two or more substances which dissolves and each of its constituents is physically distinguishable. Substances that are fewer in solution are called soluble substances or solutes, while substances that are more numerous than other substances in solution are called solvents or solvents. The solute and solvent composition in this solution is expressed in solution concentration, while the process of mixing solutes and solvents to form a solution is called dissolution or solvation.
Electrolyte solution is a solution that can conduct electrical current. Svante Arrhenius, the famous chemist from Sweden, proposed the theory of electrolytes in 1884. According to Arrhenius, the electrolyte solution in water dissociates into positively and negatively charged electric particles called ions (positive ions and negative ions) The amount of positive ion charge will Equal to the amount of negative ion charge, so that the charge of ions in the neutral solution '' Ion-ion is the duty mengahantarkan electrical current.
This solution gives a symptom of flashing a lamp or the incidence of a gas bubble in solution. The electrolyte solution contains charged particles (cations and anions). This solution may be sourced from an ionic compound (a compound having an ionic bond) or a polar covalent compound (a compound having a polar covalent bond)
A strong electrolyte solution is a solution that can conduct an electric current well. This is because the solute will decompose completely (degree of ionization = 1) into ions so that in the solution contains many ions. Because many ions can conduct an electric current, the conductivity is strong.
For example: NaCl
A weak electrolyte solution is a solution which can conduct a weak electrical current. This is because the solute will partially decompose (degrees of ionization = 0 <α <1) into ions so that in the solution it contains a little ion. This is because not all decompose into ions (imperfect ionisation) so that in the solution there are only few ions that can conduct electrical current.
For example: ordinary water, and NH3
In a non-electrolyte solution, the molecules are not ionized in solution, so that no charged ions can conduct an electric current. (Degree of ionization = 0)
Examples: urea, and glucose

Tools and materials

- Tools
1. big battery
2. 1 lamp
3. Cable + and -
4. Crocodile clamps + and -
5. Paper sandpaper
6. 2 large battery cathode
7. Triplect
 

   - ingredients
1. Rain water and battery water
2. Sugar water (4 spoons)
3. Salt water (salt box)
4. Soap water (4 scoops of detergent)
5. Vinegar
6. Urea (3 spoons)
7. Alcohol 70%

Work procedures

1) Run the electrolyte test kit.
2) Check if the electrolyte tester works properly or not if the two electrodes are connected, the lamp can be on.
3) Insert one of the solutions to test its electric conductivity strength with 2 cathodes into the beaker halfway up. Notice not to touch.
3) Record and check what happens to the appliance, whether the light is on or off, has a bubble or not.
4) Clean the two cathodes / electrodes with sandpaper.
      5) Repeat activities 3-5 until all of the solutions are addressed. .

No	material	Formula	Observation		Type of Electrolyte
			Lamp	Electrode
1	Rain water	-	no flame	No bubbles	Non-electrolyte
2	Salt water	NaCl	bright	There are bubbles	Strong electrolyte
3	Sugar water	C12H22O11	no flame	There are bubbles	Weak electrolyte
4	Urea	CO(NH2)2	no flame	There are bubbles	Weak electrolyte
5	vinegar acid	CH3COOH	dim	There are bubbles	Weak electrolyte
6	Etahnol	C2H5OH	no flame	There are bubbles	Weak electrolyte
7	Sulfuric acid	H2SO4	bright	There are bubbles	Strong electrolyte
8	soap water	-	bright	There are bubbles	Strong electrolyte
9	Ammonia	NH3	dim	There are bubbles	Weak electrolyte
10	Hydrochloric Acid (HCl)	HCl	bright	There are bubbles	strong electrolyte
11	Aquades	-	no flame	No bubbles	Non-electrolyte

Discussion1) Rainwater is supposed to be non-electrolyte because, no bubbles are tested and lights are not lit, but in our test solutions lights are dimmed, this may be because our electrolyte test kits are dirty or even wrong.2) The salt water should be brightly lit and has a lot of bubbles and includes a strong electrolyte, but in our experiments the solution is not lit but there are bubbles and are classified as weak electrolytes, this may be due to an error in our electrolyte test kit.3) Sugar water including weak electrolytes, lights are not lit and have bubbles, but the labs we do show no lights and no bubbles, this may be because our electrolyte test equipment is dirty or even wrong.4) Vinegar acids should be dimmed and there are bubbles, but the results of our test shows lights are not lit, this may be due to fault / damage of the test equipments.5) Ethanol (alcohol) should not light on, there is a bubble but our test results lights are not lit and no bubbles. This may be because our tool error or test tool is dirty.6) Sulfuric acid (battery water) is actually lights are bright and there are bubbles, but the test solution that we do produces that lights turn red. Maybe this is because our test equipment is less clean.7) The soapy water is basically a brightly lit lamp and there is a bubble, but our lab results show the light is not on. It may be due to an error in our electrolyte test kit.8) Urea includes weak electrolytes, no lights on but no bubbles.9) Ammonia supposedly lights are dim and there are bubbles, but our lab results show no lights on and no bubbles. This may happen because our electrolyte test equipment is dirty or even wrong.10) Hydrochloric acid should be brightly lit and there are bubbles, but the results of our lab show lights are dimmed. This may happen because our electrolyte test equipment is dirty or even wrong.11) The aquades include non-electrolyte solutions because the lights are not lit and there are no bubbles.

Post-practice questions1. What symptoms indicate the conductivity of electricity through the solution?Answer:The presence of many gas bubbles.2. Among the materials tested, which material is a strong electrolyte solution, weak electrolyte, and nonelectrolyte?Answer:Strong electrolysis = HCl and NaOH, weak electrolyte = vinegar and NH4OH, Nonelectrolyte = Sugar, urea, tea water.3. Name the characteristics of the strong electrolyte and weak electrolyte solution that can be observed from the experiment!Answer:Powerful electrolyte = lights on and many gas bubbles. The electrolyte is weak = the light is not lit but there is little gas bubble.Conclusion• Strong electrolytes have the characteristic of lights on and there are many gas bubbles.• The weak electrolyte has a characteristic that is the light is not lit and there is little gas bubble.• Nonelectrolytes have no light features and no gas bubbles.Denngan know the conductivity of the solution along with electrical conductivity symptoms in the solution, we can group the solution into electrolyte and nonelectrolyte solution.
Bibliography

- Ministry of National Education.2006. Standart Isi 2006, Chemistry Pursuit SMA / MA.Jakarta: Curriculum Center- Purba, Michael and Soetopo Hidayat. 2000. Chemistry 2000 for SMA class 1. Volume I B. Jakarta: Erland- Parning and Horale. 2003, Chemistry IB for grade 1 high school. Second Edition. Jakarta Yudhishthira- Purba, Michael. 2007. Chemistry for class X. Jakarta ErlanggAttachment