Alkali Metal Carbonate Lab Report

For our hypothesis we thought that the seltzer would dissolve the alka seltzer the fastest, because the seltzer was already carbonated. After doing the experiment we found out that the seltzer was the 2nd fastest at dissolving the tablet, and the water dissolved the alka seltzer 6 seconds faster than the seltzer. This being said our hypothesis turned out to be wrong because the water (fastest to dissolve the alka seltzer) has fewer chemicals, so it dissolved the tablet faster. We thought the less chemicals the slower the alka seltzer would dissolve. Although after conducting the experiment we found through data that the more chemicals in the liquid, the slower the tablet would dissolve in them.

either barium (Ba 2+ ) or calcium (Ca 2+ ). Part C consisted of a series of cation flame tests using metal

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

The purpose of this experiment was to mix Alka-Seltzer with Hydrochloric acid in order to analyze Sodium Bicarbonate as an active ingredient in the Alka-Seltzer. The mixture will contain hydrochloric acid to only see the composition of Sodium Bicarbonate in the tablet once it reacts. The amount that reacted allowed us to determine how much of it is present in the tablet. The amount of sodium bicarbonate will be measure by using the ideal gas law PV=nRT. The experiment will be conducted in the lab, therefore we are going to use room temperature which ranges from 15 to 26 degrees celsius. At room temperature pressure ranges from 12.8 to 25.0 millimeters mercury according to its corresponding room temperature.In the ideal gas equation R is 0.08206latm/mol k which is a constant. Once we have those values we can calculates the number of moles that reacted in the mixture by solving for the missing value. With the number of moles we are able to find the mass in grams which is what will potentially tell us the composition of Sodium Bicarbonate in a tablet of Alka-Seltzer.

The white color implies that chlorine is within the mineral oil, thus did not react. Since chlorine did not react, it means that bromide isn’t a possible anion, leaving chlorine as the anion. In procedure 5, the unknown compound produced water on the watch glass indicating it could be a hydrate. The hydrate test was inconclusive because the number of waters of hydration shown in Table 5 was half way between being lithium chloride monohydrate and lithium chloride 2. The percent error, shown in Table 5, between the expected percent of water in lithium monohydrate and the accepted value, was high at 40% which meant that the unknown could not be properly identified as a hydrate. Repeating the hydrate test produced a similar percent which is shown in Table 7. The reason for these high percent errors is because lithium chloride and lithium monohydrate are both hygroscopic. In addition, Table 6 shows an increase in mass when unknown #42 was left outside, which suggest that the unknown compound is

The compound was tested for the presence of ammonium, carbonate, sulfate, chloride, and nitrate, as seen in Table 2. The nitrate test produced a precipitate, indicating the presence of the nitrate ion in the compound. At this point it was hypothesized that our unknown compound was calcium nitrate.

The purpose of this experiment was to identity, analyze and synthesize an unknown white compound. The identity of the unknown compound was determined by a flame and ion test to identify the cation and anion present in the compound. To confirm the identity, an ammonium test and conductivity test was conducted. After, the unknown compound, which was identified as Calcium(II)Nitrate, was synthesized in an acid-base reaction between Nitric Acid and Calcium Carbonate. The increments used were done so in order to obtain a theoretical yield of 1.0 gram of Ca(NO3)2.

On average the Alka Seltzer tablet dissolved faster in hot water in comparison to ice cold water and room temperature water. The beaker with ice cold water caused the Alka Seltzer tablet to dissolve the slowest. The three beakers containing different temperatures of water, all produced carbon dioxide bubbles; however, the beaker containing hot water produced the bubbles more rapidly.

Alka Seltzer is a medical drug used for pain relief and used for relieving indigestion. For example, if you have a stomachache or some indigestion problems, Alka Seltzer may help neutralize the stomach acidity. Not only that, Alka Seltzer is also used for cleaning household items, such as vases or jewelry. Alka Seltzer contains citric acid and sodium bicarbonate, which makes it dissolve and release carbon dioxide gas when dropped in water. In this experiment, my lab partner, Rebecca, and I are trying to find a way to make Alka Seltzer dissolve faster in water. Rebecca and I both decide that if we increase the temperature of the water or make the water hotter, then the Alka Seltzer will dissolve faster because I know when salt and sugar dissolve in hot water, they dissolve faster. I predict that this same result would apply to this experiment.

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

There are significant differences in chemical and physical properties between beryllium and magnesium and the group members from calcium onwards, which traditionally led to "alkaline earth metal" only applying to the latter group. This classification is mostly not in in English-language sources, but is still used in other countries such as Japan. As a result, comparisons with strontium and barium are more germane to calcium chemistry than comparisons with magnesium. Calcium metal burns hot if ignited, and it reacts violently with water to form the strongly-alkaline calcium hydroxide that can cause chemical

An unknown material can be determined by using simple chemical tests and separations which is called as inorganic qualitative analysis. The separation of cations depends on the difference in their propensity to form precipitates. Separation scheme is used to classify cation into five groups on the basis of their physical and chemical behavior opposed to some reagents. Classification is based on whether there is formation of precipitates or not when metal cations react with the reagent. The five groups of cations and the characteristics of these groups are as follows:

The amount of soda ash needed for the experiment was calculated using the following equation: sample weight of unknown=0.1103M (18ml×150.99)/(10×2× %〖Na〗_2 〖CO〗_3 ) An analytical balance was used to weight the calculated amount of soda ash. A piece of weighing paper instead of a weighing boat was used. The mass was recorded. The weighed soda ash was transferred into a 250 mL beaker, then the sample was dissolved in approximately 70 mL of water. The pH meter and electrode was obtained, rinsed with DI water, and calibrated using pH 7 and pH 4 buffer. A burette was obtained, mounted on a ring stand, and filled with the standardized HCl solution, that was prepared in Experiment 2. Since magnetic stirring bars and stirring plates were not available, the students

Calcium, Na, is a metal located the 20th element in the periotic tablet and has an atomic mass of 40.078. It is located in period 4 group 2 and is a alkaline earth meatal. These metals are shiny, and most are white or silvery in color, physically they are soft, they react with water to produce hydrogen gas and the metal hydroxide. Due to their high levels of reactivity, the alkaline earth metals rarely appear by themselves in nature.

The reaction characteristics of basic copper carbonate 〖mCuCO〗_3⋅n〖Cu(OH)〗_2 were observed by changing the reaction mole ratio. The reaction mole ratio of sodium carbonate to copper chloride (II) was controlled from 1.08 to 1.68. Fig. 1 shows the XRD patterns of copper carbonate powder. At a reaction ratio of 1.08, paratacamite (Cu_2 Cl(OH)_3 ), beside alkali copper carbonate, was formed because of incomplete reaction at a copper content of 53.9 wt%. Lack of sodium carbonate may cause incomplete reaction with copper chloride (II) because of low pH (6.0) of the solution [12]. The copper content according to the reaction mole ratio were 57.7, 50.5, 58.8, 59.3, and 59.8 wt% at the reaction mole ratios of 1.20, 1.32, 1.44, 1.56, and 1.68, respectively.