Softening Hard Water With Sodium Carbonate
Prediction
----------
In a preliminary experiment, we discovered that adding 1g. Na2CO3 to
hard water softened it slightly. We tested both tap water and
distilled water with the sodium stearate and discovered that tap water
was far harder than distilled water, we then tested tap water that 1g
of Na2CO3 had been applied to. This solution was softer than the
original tap water. The exact results were;
Type of water
Soap solution required
1st attempt
2nd attempt
Average
Distilled
0.5
0.5
0.5
Tap
4.5
5.0
4.75
Tap with 1g. Na2CO3
3.5
3.0
3.25
This tells us that Na2CO3 softens hard water. However 1g Na2CO3 did
not render it as soft as distilled water. Now our aim is to determine
whether increasing the quantity of Na2CO3 added to the hard water
softens it more effectively. We are measuring the hardness of the
water by the volume of soap solution required to produce a lather.
Thus, the less soap solution required to form a lather, the softer the
water, and the more successful the Na2CO3.
We know that 1g Na2CO3 did not fully soften the water. My prediction
is that as the quantity of Na2CO3 is increased, the water will become
softer. Thus requiring less soap to form a lather. Additionally I
predict that after a certain point the Na2CO3 will become less
effective at softening the water until finally it will not effect the
softness of the water if more Na2CO3 were to be added.
Water is made hard by dissolved calcium ions, Ca2+, when placed into a
solution Na2CO3 splits up into Na+ ions and CO32- ions, the CO32- ions
combine with the dissolved calcium ions to create calcium carbonate,
this is a solid precipitate that doesn't alter the softness of the
water. The sodium ions stay dissolved in the water, but they don't
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
The purpose of this experiment was to determine the amount of water in Epsom Salt and determine whether the amount of water is equal to the theoretical value, when the chemical formula is MgSO4・7 H2O. To check the amount of water in epsom salt, 3g of epsom salt in each crucible 1, 2, and 3 were heated on 495℃. While the epsom salt was heated, white water vapor came out from the crucibles and disappeared in the air. According to the Table 1, as the epsom salt were heated, the mass keep decreased and when those were heated 5th and 6th times, 50 minutes and 60 minutes, there were no significant change in mass. From the Table 2, the leftover amount of anhydrous epsom salt in each crucibles were equal. There were 1.46g of MgSO4 in the crucible after the last heating and 1.54g of H2O was vaporized. Since the result of each trials are same, the standard deviation shows up as 0. By using the molar mass of each compound, MgSO4 got 0.0121mol and H2O got 0.0855mol, which the ratio of MgSO4 and H2O is 1:7.07. The mol ratio shows that when there are one MgSO4, there are 7 H2O. According to the chemical formula of epsom salt, which is MgSO4・7 H2O, the experiment shows that the experiment and the theoretical values are almost same. The random errors of the mass and mol for MgSO4 and H2O are 1.3699% and
When Alka-Seltzer comes in contact with water, a chemical reaction immediately occurs that releases carbon dioxide gas. This reaction creates a lot of bubbles and fizz like a soda, and like a soda, the bubbles are carbon dioxide gas (CO2).
To begin the experiment, we measured 5cc of water and 5g of NaCl and added them to a test tube. Next, we stoppered the test tube and shook vigorously for two or three minutes. After we observed that the solution was saturated and massed an evaporating dish (18.89g) and poured most of the solution into it, while being careful not to pour any undissolved solid into the dish. Next, we massed the evaporating dish with the solution and found it to be 23.32g. The next step was to slowly evaporate the solution in the evaporating dish using a hot plate. Once the liquid was evaporated from the solution, to the best of our ability, we massed the remaining solid in the dish, which we found to be 20.32g. This was the last step of the physical portion of the experiment, and we proceeded to the calculations. First, we found the mass of the remaining solid by subtracting the mass of the evaporating dish from the mass of the solid and evaporating dish, which we found to be 1.43g. To find the mass of the evaporated water we subtracted the mass of the solid and evaporating dish from the mass of the solution and evaporating dish, which we found to be 3g. Because the density of water is 1g/1cc, the mass is the ...
The third titration was performed by making a solution of Sodium Bicarbonate with 0.336 grams of Sodium Bicarbonate and 50 mL of deionized water. Three drops of methyl orange indicator were added to 10 mL of HCl inside of a flask in which the Sodium Bicarbonate solution was added to. Three trials were performed and averaged to calculate the molarity of the baking soda along with the percent yield of the reaction. In the final titration of the experiment commercially purchased vinegar was used with NaOH. 10 mL of the vinegar was added with 40 mL of deionized water as the original bottle solution was too acidic to be neutralized with small amounts of NaOH. Four drops of the phenolphthalein indicator was added to 10 mL of the now further diluted acetic acid solution which was also titrated with NaOH. Three trials of this titration was performed to determine the actual molarity of the commercial vinegar compared to its advertised
Investigating the Solubility of Table Salt in Distilled Water at Different Temperatures The aim of this essay is to explain and discuss the drug cannabis and its effects in relation to biochemical, behavioural and psychological factors. The introduction will outline a brief history relating to the drug and include both the medicinal and recreational purposes of its use. The main discussion will explain how the drug chemistry affects the nervous system emphasising what neurotransmitter is effected and also what behavioural and psychological implications this has on the user.
The goal of this experiment was to: create a dilute NaCl solution and calculate molarity, molality, and parts per million, experimentally determine the molarity of the same dilute NaCl solution through Mohr chloride precipitation technique, then, evaluate the accuracy by comparing the actual value to the experimental one. The actual molarity was calculated using the average density of three trials, mass of NaCl in solution, and molarity formula to be 0.0140 mol/L, the molality was calculated to be 0.0143, and the PPM was calculated to be 833. The experimental value for molarity, obtained through titration using AgNO3 as a titrant with Ag2CrO4 as an indicator, was averaged over three trials to be .01523 mol/L. Comparing experimental and actual values gave an estimated standard deviation of 0.00032 M with a confidence interval of +0.00079 at 95% and +0.0018 at 99%. The percent error for molarity was 8.8%. The experimentally determined molarity was functionally close to the actual molarity, however, some significant error in accuracy was observed. The amount of precision achieved with reasonable accuracy suggests this experiment could be used in testing salinity of separate bodies of water for comparison. The high % error inaccuracy, however, also suggests this should not be used in comparing minute changes in salinity in a single body of water.
There is also a small standard error of the mean compared to the size of the standard deviation which indicates some uncertainty in the accuracy of the results. The concentrated solutions used may have been contaminated from the source and therefore all collaborated results would be inaccurate due to the solutions not being of the correct percentage concentration of sodium chloride. The results would be inaccurate as they would not be correctly collaborated to the correct concentration in which they are being graphed for. Another systematic error is that the eggs are not all exactly the same size and effects such as surface area to volume ratio can impact how much water enters or exits the egg at any point in time. There was also still traces of shell left on some eggs which would have affected the rate of osmosis as not all membrane was available to be utilised in the diffusion of water. However, a larger sample size will eliminate the effect of this error. The reaction may have not reached equilibrium in the time frame of 10 minutes and this may be needing to be extended. For an equilibrium to be reached between the water and solute in the egg and in the solution. The strength of the experiment included the efficiency in which the practical was completed placing 2 eggs within a solution each at the one time as well as collaborating results with other experimenters in order to achieve an average overall for a larger sample size. Yet it could still be improved by further increasing the sample size of the experiment to counteract and possibly eliminate the effects of errors on the
Bottled water,more expensive choice than tap water for your houseplants,might improve the condition of your plants.Water from softeners often contains sodium (salt)in amounts that are harmful to houseplants.
Buying a case of bottled water every week at the store is something people do out of habit, however most people are not aware of how much plastic is piling up. Some people think that bottled water will not cause a problem if you dispose of the bottles correctly however, others think that they can hurt the environment even if you dispose of them properly. Environmentalists think bottles water should be banned because they are probably worse quality than your tap water, they can be very expensive, and they are very bad for the environment.
Is bottled water a wise consumer choice? No bottled water is not a wise consumer choice because it costs to much money, people have to worry about chemicals, and the extraction plants are annoying for the people around them.
My hypothesis was supported because each experiment did what I thought it would. The salt sank when it was inside of the hot and cold water. When salt was placed inside of the hot and cold water, it sank because of it weighing more than the cold and hot water. We can look at it in this way, salt water weighs more than fresh water. The weight of a cubic foot of salt water is 64.1 lbs. On the other hand, a cubic foot of fresh water only weighs 62.4 lbs. The numbers are different because the salt water has a higher density compared to fresh water. When salt is added to water then the molecules in water are different because they are really together and tight around the salt molecules. Adding salt also increases the volume of water by less than
The government should restrict water use for the following reasons. A interesting fact is, the state of California, is trying new ways to conserve and save water. The people of California are now tying waste water into sum what clean what, that is purified. There are a couple places in California using a different technique called desalination. This tactic is using the water from the Pacific Ocean, taking all the salt out of it then, making it water others can use. The tactic is harmful to the sea life because when you desalitize the water, you have left over salt that gets dumped right back into the ocean. Even more compelling is, the people of California are using ground water as there water supply. From a news report a statement was made
Many people do not pay much attention or care about what condition their water is in. According to www.cleanwater.com, when water comes in contact with the air, it absorbs carbon dioxide, making it more acidic. Therefore, unfiltered water can be very dangerous. Your body's acidity becomes higher due to the amount of unfiltered water you drink. This can lead to rapid breathing, fatigue, headache, lack of appetite, increased heart rate, and even confusion.
For the solid sodium chloride, using distilled water will make it an aqueous solution. Just like before using red and blue litmus paper will only indicate that the sodium chloride is neutral. The same can be done for sodium carbonate since it is soluble in distilled water, making it easy to determine whether it is an acid or base when using litmus paper. In this case, sodium carbonate is a base so red litmus paper will turn blue when the solution of sodium carbonate is dripped on to it.