The purpose of the experiment was to do a solution, which molarity is 0.20 mol/l, from water and an ionic compound. Our ionic compound was zinc sulfate (ZnSO4). Our task was to make one hundred milliliters (100 ml) of the solution. Materials To execute the experiment we used the following equipment: - a beaker - a volumetric flask - a plastic spoon - a scale - a pipette - a funnel - a cork cap We also used solid zinc sulfate (ZnSO4), and distilled and deionized water to make the solution. Calculations To figure out the amount of zinc sulfate that we had to add to the water, so that the molarity of the solution would be 0.20 g/mol, we did the following steps: First we calculated the amount of the zinc sulfate to add in moles.
If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium. 2 HI (g) === H2 (g) + I2 (g) Ke = 1.84(10-2 [H2]=[I2]= 1.07(10-2 mol/L, [HI]=7.86(10-2 mol/L 6. A 1.00 L reaction vessel initially contains 9.28(10-3 moles of H2S. At equilibrium, the concentration of H2S of 7.06(10-3 mol/L. Calculate the value of Ke for this system.
Single Replacement Reaction Laboratory Modified from Glencoe Chemistry - Matter and Change, Glencoe McGraw-Hill, 2002 Objectives Observe a single replacement reaction Measure the masses of iron and copper Determine the mole ratios and the limiting reactant Chemicals Iron filings (Fe) – 20 mesh Copper(II) sulfate pentahydrate, (CuSO4·5H2O) Distilled water Materials Stir rod 100-mL beaker 250-mL beaker 25-mL graduated cylinder Weigh paper Balance Hot plate Beaker tongs Wire mesh insulated pad screen Distilled water wash bottles |Lab Data - Reaction of Copper(II) Sulfate and Iron | | Mass of empty 100-mL beaker |(g) | | | Mass of 100-mL beaker
Part C: Density of Sodium Chloride (NaCl) Solution, a sample of NaCl was obtained and measured using a 100mL beaker and a 10mL pipet to determine the concentration of the solution. In order to obtain the appropriate result, a calibration graph and density measurement was used to determine the concentration of the sodium chloride solution. In conclusion, based on the water temperature of 21.8°C in part A’s graduated cylinder experiment obtained, it was determined that the average density was .0973g/mL with a percentage error of 2.5%. When graphed the measurement was equal to Y=0.988x. Part B: The graduated pipet’s average density at 22.3 °C was determined to be 0.9785g/mL with a percentage error of 1.89% shows the graduated pipet to be more accurate and precise.
(4 points) n = 125 4. If magnesium was the limiting reactant in this lab, calculate the theoretical yield of the gaseous product. Show all steps of your calculation. (4 points) Moles of Mg: (0.0281 g)(1 mole / 24.305 g) = 1.156 x 10^-3 moles 5. Determine the percent yield of this reaction, showing all steps of your calculation.
n (3) Solutions of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride. co NaOH(s) → Na+(aq) + OH–(aq) ∆H1 = ? Chemistry with Vernier py In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. One of the reactions is the same as the combination of the other two reactions. Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the sum of the heats of reaction for the other two.
What is the weight percent of each element in ammonium sulfate? C. Empirical and Molecular Formulas 1. Empirical Formula - shows the number of atoms in the smallest possible ratio a. may be calculated from percent composition data b. may or may not show the true number of atoms of each kind in the molecule 2. Molecular Formula - shows the true
Conclusion 10 Grams of Potassium chlorate when decomposed produces 3.915576 grams oxygen gas and 6.083363 grams potassium chloride Atomic Weight of Magnesium Introduction In this lab we will determine the atomic weight of magnesium by measuring the amount of hydrogen gas evolved when hydrochloric acid reacts with magnesium. The reaction is as follows: Mg + 2HCl -> H2 + Mg2+ (aq) + 2Cl- (aq) There is a one to one relationship between the number of moles of hydrogen gas evolved and the
The chemical reaction used to find this constant is as follows: MgC2O4 (s) ↔Mg(aq)2++ C2O4 (aq)2- Kc= Mg2+[C2O42-][MgC2O4] Ksp=Mg2+[C2O42-] The solid salt magnesium oxalate is prepared through the following precipitation reaction: Mg(SO4)(aq)+NaC2O4 (aq) → MgC2O4 (s)+NaSO4 (aq) Next, the concentration of the Mg2+ and C2O42- ions is found through a redox titration. This redox titration uses a standardized potassium permanganate solution. The potassium permanganate solution is standardized by titrating it with samples of iron(II)ammonium sulfate hexahydrate . The end point is reached when the solution has turned light purple which is a result of excess amounts of MNO4-. This reaction can be summed up using the following formula: 5Fe2++8H++MnO4- →5Fe3++Mn2++4H2O After standardization, the potassium permanganate solution is then titrated with 3 different magnesium oxalate solutions.
Section 3: The titration of an unknown concentration of HCl with the standard solution of NaOH. Section 4: Use the HCl solution titrate a commercial basic product and determine the quantity of active ingredient. -Section1: Preparation of a Standard Sodium Hydroxide Solution Materials 250-mL volumetric flask Weigh scale Weighing bottle, or watch glass for NaOH sample, Glass funnel Dropper pipette 100 ml beaker Deionized water NaOH solid Procedure 1. Weigh approximately 1 gram of NaOH in a weighing bottle. Record the actual mass (1.01 grams weighed) in the results table.