Place 10 drops of copper (II) sulfate into A5 of the 24 well plate. 7. Use the tweezers to pick and carefully insert a piece of magnesium into the sodium sulfate. Record your observations. 8.
Gravimetric Analysis of a Metal Carbonate Post Lab TABLE Mass of Crucible + M2CO3 14.8145g Mass of Crucible + M2CO3 (1st weighing) 14.7915g Mass of Crucible 12.9405g Mass of M2CO3 1.851g Mass of filter paper + CaCO3 3.8025g Mass of filter paper 1.8120g Mass of CaCO3 1.9905g Moles of CaCO3 0.019887 mol Molar mass of M2CO3 93.08 g/mol Identity of M2CO3 Na2CO3 Percent Error 12.18% error ANALYSIS QUESTIONS 1. Calculate the moles of precipitated calcium carbonate, CaCO3. Enter this value in the Data Table. 1.9905g CaCO3 x 1 mol CaCO3 = 0.019887 mol CaCO3 1 100.09g 2. Calculate the molar mass of the unknown carbonate.
The pre-1983 penny was made of an alloy of copper and zinc. An alloy is “a substance that has metal characteristics and consists of two or more different elements”. (Coordinated Science, pg.1005) Our objective is to find the metal used inside a post-1983 penny. The accepted value of the density of a post-1983 penny is 7.05g/cm3. “Density is the mass per unit volume of a material”.
Real World Applications of Number Theory A. Rounding and Truncation 1. Student 1 received a score of 299 out of a possible 334 points for a term in an unknown class. To find what percentage the student received, one must take the score received and divide it by the total amount of points possible, and then multiply the quotient by 100. In this particular case, the teacher chose to use rounding to attain the final grade of the student. To round to the nearest whole number, one must consider the value in the tenths place.
Once the reaction of sodium hydrogen carbonate takes place, carbon dioxide gas is released, as well as water vapor. When the compound is under heat, the crystalline power bubbles, and stirs around as the carbon dioxide gas is released. Over time powder is heated, the entire compound gradually decreases noticeably in size and weight as the water vapor escapes as well. The crystalline powder (solid) never changes state, and after
The tip of the inner blue flame is the hottest portion. 4. How will you know in this experiment when the hydrate BaCl2*2H20 has been completely dehydrated? It will be completely dehydrated when the difference in successive weights of the crucible, cover, and residue (after cooled to room temp.) is 0.0020 g or less.
Contents Page Experiment 1 Calibration of a 25-mL Pipette 1 Experiment 2 Volumetric Analysis 3 Experiment 3 Experiment 4 Experiment 5 Gravimetric Determination of Nickel Sodium Acid Salt of Heptaoxodiphosphoric Acid Synthesis and Stoichiometric Analysis of Hexaamminenickel(II) Chloride 5 6 9 Experiment 1: Calibration of a 25-mL Pipette Background The graduation mark on a pipette being usually made at 20°C (whereas room temperature is much higher than this), the volume of the pipette must be calibrated before any volumetric analysis is carried out. Otherwise, the error in the graduation mark may exceed the error allowed in a measurement. A pipette is designed to deliver only one fixed volume of a liquid and it is calibrated for this volume only. Accuracy to two decimal places in mL is generally possible. The pipette is calibrated by weighing distilled water in it at room temperature, and then calculating the volume from the weight of water in air.
The purpose of this lab was to perform a titration on 10.000 mL of sodium hydroxide solution with 0.10 mol/L sulfuric acid solution. In this lab we performed numerous trials to find the amount of sulfuric acid solution that would neutralize 10.0 mL of sodium hydroxide solution and averaged the trials to find the amount; this data could then be used to find the concentration of the sodium hydroxide solution through solution stoichiometry. To do this we used a burette with the capacity of 50.00 mL with an uncertainty of 0.04 mL, a pipette of 10.000 mL with an uncertainty of 0.015 mL, a clamp stand, a titration flask(an Erlenmeyer flask) and bromothymol blue indicator. The apparatus was set up like so; 0.00mL (graduation at top) Burette contains 0.10M H2SO4(aq) 50.00mL (graduation at bottom) Erlenmeyer flask contains 10.000mL of NaOH (aq) as well as bromothymol blue indicator (10.000mL was measured with a pipette) Evidence Table 1: Raw Data collected from the Titration Lab showing the initial and final burette readings of the titrant of 0.10M ± 0.005M H2SO4(aq) Qualitative Observations Before any sulfuric acid was added, the solution was colourless and clear. After adding three drops of brymothymol blue indicator, the solution was now a clear blue colour.
The equilibrium is of dynamic nature; means that both the forward and backward processes are taking place even at the equilibrium point but with the same speed. The equilibrium involving gases can be attained only in closed containers. At equilibrium, the concentrations of different substances involved in the process become constant at constant temperature. The equilibrium involving a solid dissolved in a liquid at a particular temperature is represented by the saturated solution. Question 3 The solubility of a gas in a liquid is given by Henry's law.
All matter may exist in any of three physical states of matter.In the graphic on the left the solid and liquid forms of water - ice are shown. | | Physical Changes:A physical change takes place without any changes in molecular composition. The same element or compound is present before and after the change. The same molecule is present through out the changes. Physical changes are related to physical properties since some measurements require that changes be made.Melting Point: As solid matter is heated it eventually melts or changes into a liquid state at the melting point.