After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid. Place another dry test tube in a 50mL beaker and weigh it. Find a bottle of barium iodide and record the name and molar mass. Then, weight out either anhydrous barium iodide or barium iodide dehydrate into this test tube and dissolve is it in 2 mL of deionized water. Pour the contents of one of the test tubes into the other and a reaction should occur and you should see a white precipitate of barium sulfate form.
Cylinder was rinsed with distilled water. * * 2. 2.0 ppm standard: 2.00 mL of 10.0 ppm phosphate solution was placed in a 25 mL graduated cylinder and diluted to exactly the 10 mL mark with distilled water then poured into a plastic cup labeled 2. Cylinder was rinsed with distilled water. * 3.
c. Prepare the solution by dissolving 38.90 grams of ZnI2 with 500 mL of water. d. 0.0125/0.25 = 0.05 L = 50 mL. This produces 0.0125 moles of ZnI2 5. Exercise 5: a. (0.125)(0.1) = 0.0125 moles of solute b. Pour 50 mL of the stock solution to get the number of moles needed.
Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 0.250 g H2SO4 x 1 mole x 1 L = 0.0102 L 98.12 g 0.250 mole 5. 1.50 g of NaCl is dissolved in 100.0 mL of water. Calculate the concentration. 6.
These tests consisted of a wafting test, a solubility test in deionized water, and a pH test. The unknown’s characteristics, discovered through the physical tests, were then compared with known cations: Sodium, Potassium, Calcium, Ammonia, and Magnesium. Flame tests were performed in order to classify the unknown cation. A small amount of the solid unknown ionic compound was placed on a watch glass. A wet swab was used to collect a small sample of the compound.
A) How many mosm solute will 1 gram of NaCl yield? Show your calculations. (1gNaCl/1)*(1000mg/1gNaCl)(2/58mg)=34.5mOsm. 3. Mixed Solutions: If 1 mmole of glucose (180mg=1mOsm) and 1 mmole of NaCl (58mg=2mmOsm) are put into a beaker and distilled water added to make 1 liter, the osmolarity is 3 mOSm/L.
The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel. The peak of the line is used to find Vmax of Fe2+. Vmax is used to find the moles of Fe2+ and ligand. The unknown n is a ratio of moles ligand divided by moles Fe2+. Results and Discussion For the first part of the experiment (Part A), five different 100 mL volumetric flasks were each filled with 1,2,3,4 and 5 mL of iron (II) solution.
Hydrate Lab The purpose of this lab is to analyze the percent water in a crystalline hydrate and to indentify the hydrate from a list of possible unknowns. The solid hydrate will be heated to remove the water, and the percent can be found by measuring the mass of the solid before and after heating. The hydrate will be indentified by comparing the percent water in the hydrate with the percent water calculated for the possible unknown. Before the lab there are pre-lab questions: 1. Describe the three general safety rules for working with a Bunsen burner.
Stoichiometry is a section of chemistry that involves using the relationships between reactants or products in a chemical reaction to determine the desired quantitive data. 4. Using the balanced chemical reaction between Sodium carbonate and Calcium Carbonate given in page 92 of your lab manual (first paragraph of procedure), find the mass of Sodium Carbonate (in grams) needed in reaction? Na2CO3(aq)+CaCl22H20(aq)-CaCO3(s)+2NaCl(aq)+2H2O Date:_____3/30/2015____________ Name______Chloe Flake______________ 1. Title: 1pt Stoichiometry Of A Precipitation Reaction 2.
[7.7(10-12 mol/L] 2. How many milligrams of PbI2 can you dissolve in 300 mL of water at 25(C? Ksp of PbI2 is 1.4(10-8 [210 mg] 3. Calculate the solubility product constant, Ksp, of SrCl2 if 8.0 mg dissolves in 200 mL to form a saturated solution at 25(C. [6.4(10-11] 4. Seawater is saturated with AgCl.