H2In-3 (aq) + M2+ (aq) MIn- (aq) + 2H+ (aq)
Blue pink
As you add EDTA solution from a buret, the metal ions preferentially
The calcium dissolved really quickly and there were bubbles and foams formed. We then heated the beaker with a hot plate for 2 to 3 minutes, equally distributed the supernatant solution into two test tubes, but avoid pouring the solid. After centrifuging the samples, we added extra HCl solution into the test tubes, there wasn’t any bubbling occurs, so we could continue and put the mixtures into the centrifuge again. And then put the NaCO3 solution into the beaker and wait to allow the CaCO3 precipitate to form. We then tested whether the supernatant solution is still acidic with a piece of red litmus paper, filter the liquid and we had some CaCO3. Dried the filter paper and CaCO3 in the oven, then we broke the CaCO3 into small particles with a glass rod, and dried it one more time. Let it cool and repeat heating, cooling and weighing it until the masses differ between two results are less than…
A 50-mL buret, a 250-mL volumetric flask, and 25- and 50-mL pipets were obtained from stockroom. The 0.5 g of calcium carbonate was weighted in a small 50-mL beaker. Approximately 0.4 g of the carbonate was transferred to a 250-mL beaker. 25 mL of distilled water was poured to the large beaker and 40 drops of 6 M HCl were added. Then, solution was heated until it just begins to boil. After boiling 50 mL of distilled water was added to the beaker. The flask was stoppered and mixed thoroughly by inverting the flask. The buret was filled with the EDTA solution. The blank was prepared by adding 25 mL distilled water, 5 mL of the pH 10 buffer to a 250-mL Erlenmeyer flask. Small amount of solid Eriochrome Black T indicator was added. EDTA was added to the solution until the last tinge of purple just disappears. Three 25-mL portions of the Ca2 + solution were drawn separately into clean 250-mL Erlenmeyer flasks. To each flask add 5 mL of the pH 10 buffer, a small amount of indicator, and 15 drops of 0.03 M MgCl2 were added. The solution was titrated in one of the flasks until its color matches that of your reference solution.…
Experiment and Observations: As I performed the lab, I had to retrieve all my equipment’s from my labpaq. As I started to setup, I had to weigh out 1.0 gram of CaCl2*2H2O on the digital scale. After it was weighed, it was added to the 100 mL beaker and 25 mL of distilled was added and stirred. Next, I had to figure out the amount of the second reactant, so that it can be added to the solution. I had to perform stoichiometry to figure out the amount of Na2CO3 is needed to make a precipitate of calcium carbonate. After the calculations, I arrived at .72 grams of Na2CO3 and rounded to the nearest tenth to mix with 25 mL of distilled water. After both of the reactants were mixed separately with distilled water, they both were clear color. As soon as you added the solution of Na2CO3 to CaCl2*2H2O the color of solution changed to a cloud white color. When both solutions are mixed, the paper filter that was provided with the lab must be weighed and recorded. Then you pour the solution into the paper filter to filter out the precipitate and dry the filter to weigh the mass of the precipitate when it dries. After it dried, it was weighed and stoichiometry was performed to see what the…
Water is to be considered “hard” if it contains unusually high levels of dissolved magnesium, and calcium ions. This can be an issue for some people because hard water reacts with soap and it forms an insoluble salt or curds, which then in turn may leave your clothing looking yellow. Hard water can be softened by filtering your water through a household water softener to remove some of the excess magnesium…
Primarily, hard water consists of magnesium and calcium. Therefore the ratio of magnesium to calcium ions was inferred to be 50/50. The average molar mass of the molar mass of Magnesium (24.305 g/mol) and the molar mass of Calcium (40.078 g/mol) was calculated to be 32.192 g/mol. This calculated average molar mass was used as the molar mass of the metal that was present in the sample. The concentration of metal that was present in the TAP water was solved by the following calculations:…
When water is heated limescale deposits can form, especially in machines such as fully automatic coffee makers, espresso machines and all hot water units. In this context you often hear about hard and soft water. The hardness of the water indicates the proportion of limescale. Your water supply company will provide more information about hardness of your water. If your groundwater flows through calcareous rock layers, eroded magnesium and calcium carbonate will cause limescale deposits in your water.…
A) The first source of error had to do with the precipitation section of the lab. Not only is possible, but it is almost guaranteed that the CaCO3 did not precipitate to its fullest extent. Attaining a precipitate that is 100% pure and is…
Total hardness of tap water was 120 mg/l and bottle water combined had a total hardness of 50 mg/l…
(1)Hard water is any water containing an appreciable quantity of dissolved minerals. (2) Some of the minerals come from chalk, limestone or marble, which the water may have flowed over or through. (4) Hard water contains calcium or magnesium ions. Limestone, marble or chalks are insoluble in pure water however they will dissolve slowly in acidic rain. If your water has emerged through limestone or chalk (calcium carbonate) it will be hard. (1) Soft water is gratification water in which the only cation (positively charged ion) is sodium. The minerals in water give it an idiosyncratic taste. Some natural mineral waters are highly desired for their flavour and the health benefits they may converse. (3) Extremely hard water affects plumbing such as pipes and the performance of certain cleaning agents. When the water is heated the carbonates precipitate out of solution, forming scale in pipes and kettles.…
In this experiment a titration using a standardized HCl solution will be used to determine the solubility product of the dissolution of calcium hydroxide in water. The following chemical equation can explain the…
Sacramento tap water reveals ion concentrations of various different dissolved minerals such as calcium (Ca2+) and magnesium (Mg2+). These concentrations are a result of mineral deposits in local lakes and rivers. Perma Pure, a gas conditioning products manufacturing company, simplifies the mechanism of ion exchange by explaining that water is a solvent that dissolves most ionic bonds when exposed to compounds ("The Mechanism of Ion Exchange"). Therefore, as tap water passes through rocks it will pick up several different minerals resulting in hard water. As reported by the USGS water science school, calcium carbonate concentrations from 0 to 60 parts per million (ppm) are considered soft, while 61 to 120 ppm is medium, and anything past 121 ppm is classified as hard water (Perlman). In this experiment, a sample of Sacramento tap water was tested for its ion concentrations of Ca2+, Mg2+, chloride (Cl-), nitrate (NO3-), and sulfate (SO42-), which will give insight on potential negative and positive effects of using the tap water. If the concentrations of…
Purpose: The purpose of this investigation is to find the solubility product (Ksp) of Ca(OH)2 by titrating the hydrochloric acid with calcium hydroxide and using their entities to find the concentration of Ca2+ and OH- ions.…
concentration of these ions is said to be soft. The hardness of water can be measured as…
chen,Yueh-huey, and Jing-Fun Young, Alka Seltzer fizzing-determination of percent by mass of NaHCO3 in alka seltzer tablets, J.Chem. Educ., 79, (July 2002), 848-850.…
EDTA is a hexaprotic acid, meaning that each of the amines nitrogen’s and each of the acid’s oxygen’s can donate one electron pair. There are four carboxylic acid groups and two amine groups, allowing a total of six attachments points, hence it being ‘hexa’protic. EDTA is a chelating agent, which works by ‘binding’ with metal ions, forming complexes.…