h) A way to make hard water softer is to put an sodium nitrate and create a precipitate to mellow out the reaction. Another way of making it softer is by removing the calcium ions one way of doing that is by boiling the solution to take out some of the ions. Conclusion: Overall, we determined that sodium carbonate, Na2CO3, is the anion that can be used to precipitate the most metal cations. Also, we learned that the anion sodium chloride, NaCl, could be used to remove silver ions from solutions. The stuff that I found interesting was that how many colours you can get when you mix the cations and anions
This particular reaction is a strong acid and a strong base which means that when the reaction reaches the equivalence point, the moles of the acid and the base are equal and the solution is neutral so the pH should be around 7.0 depending on the final volume of each solution. To get this data, we will titrate an HCl solution with NaOH solution of which is a known concentration. We will record the initial and final reading of the NaOH while we record the pH of the titrated solution in the beaker. We will repeat this process with a solution of acetic acid which is a weak acid with NaOH and record the initial and final reading of NaOH and the pH of the solution in the beaker. Procedure Preview Calibrate the pH meter.
Write a hypothesis on what you think will happen when mixed. 3. Combine the substances; record observations. Hydrochloric Acid and Magnesium 1. Add hydrochloric acid to a test tube.
This is evident because the substance tested positive for both the acid test and the base test for zinc hydroxide. Observations of the zinc and iodine reaction without acetic acid: After swirling, the solution starts off to be yellow, than changes to orange. During swirling becomes dark brown- reddish. The tube feels warm, which means that the reaction is exothermic. Soon, the dark red changes into black and then eventually lighter and lighter becomes colorless.
The Cover Sheet to the Confidence Report South Street Seaweed Seaport Tabulated test Results Name of Test Requirements Result Test for Iodine If the mineral oil turns a shade of purple (either dark, or light such as pink), then the Tincture is positive for iodine. The solution became light lavender/pink. This shows that the tincture is positive for iodine. Test for Iodide ion A few things can happen: 1) A white precipitate only, indicating chloride ion is present predominantly (Na Cl in salt water). 2) A yellow precipitate only, indicating iodide ion is present predominantly.
Objectives: The purpose of this lab is to observe the reaction of crystal violet and sodium hydroxide by looking at the relationship between concentration and time elapsed of the crystal violet. CV+ + OH- CVOH To quantitatively observe this reaction of crystal violet, the rate law is used. The rate law tells us that the rate is equal to a rate constant (k) multiplied by the concentration of crystal violet to the power of its reaction order ([CV+]p) and the concentration of hydroxide to the power of its reaction order ([OH-]q). Rate = k[CV+]p[OH-]q To fully understand the rate law, concentrations of the substances must be looked at first. The concentration is measured in molarity.
For the sulfate anion test, 1 mL of 6M HCl and 1 mL of 0.1M BaCl2 react with 1 mL of the test solution to form a white precipitate product. This indicates the presence of sulfate (SO4¬2-). Sulfate anion equation: H2SO4 (aq) + BaCl2 (aq) → HCl(aq) + BaSO4 (s). The chloride anion test involves mixing 1 mL of the test solution and 1 mL of 0.1M AgNO3. White precipitate shows the presence of chloride (Cl-).
| | | An Activity Series 1/9/13 Makieya DunhamPartners: Jasmine Lewis and Danielle Anderson | | | Problem Statement: In this lab we determined the activity series for five metals and for three halogens. In the first part of the lab we used a microscale technique to rank the metals that reacted with the other metal nitrates from most reactive to least reactive. The metal that reacts with another metal nitrate, then the solid metal have reduced the other metal ion and is the more reactive metal of the two. In the second part of the lab we used the solvent extraction technique to derive an activity series for the halogens. Safety Precautions: When in the lab we wore goggles, an apron, and gloves the entire time.
Chemistry: Molarity and Stoichiometry Directions: Using the definition of molarity, the given balanced equations, and stoichiometry, solve the following problems. Please submit your work via the link provided. 1. Calcium hydroxide (“slaked lime”) and sulfuric acid react to produce calcium sulfate and water according to the following balanced equation: Ca(OH)2(aq) + H2SO4(aq) ⋄ CaSO4(s) + 2 H2O(l) a. How many liters of 0.2 M calcium hydroxide do you need in order to have 6.0 moles of calcium hydroxide?
In the experiment, toluene was alkylated with 2-chloropropane to synthesize isomers of isopropyltoluene in 47% yield, weighing 2.66g. The final product had a purity of 91.8% while the appearance was a colourless clear liquid with a strong odour. The results suggest that although the product yield was low, the experimental design led to the production of isopropyltoluene in high purity. REFERENCES 1. Smith R, McKee J, Zanger M. The electrophilic bromination of toluene: Determination of the ortho, meta, and para ratios by quantitative FTIR spectrometry.