Section 1: Introduction and Guiding Question Atoms are tiny particles that compose to make up matter. The atoms combine to create bonds. The bonds are substances that can go through physical and chemical changes. Chemical reactions can happen when two substances combine. Different mixtures of substances create different types of reactions. When reactions happen, the atoms rearrange and break apart. The atoms never get misplaced or taken away, due to the law of conservation of mass. The law of conservation of mass explains how mass cannot be created or destroyed in a physical or chemical change. How does the total mass of the substance formed as a result of a chemical reaction compare to the total mass of the original substance? Scientists are trying …show more content…
The materials used during the experiment included Sodium Hydroxide, Copper Nitrate, a beaker, a pipette, a test tube, a graduated cylinder, a digital scale, gloves, and goggles. The scientist put the goggles and gloves on for safety and the scientist began the experiment. First, the scientist set the graduated cylinder on the digital scale. Then, the scientist pressed zero on the digital scale. While the graduated cylinder is still on the digital scale, the scientist measured ten milliliters of Sodium Hydroxide into the graduated cylinder. The scientist recorded the mass of the Sodium Hydroxide in the data table. After the mass gets recorded, the scientist takes the graduated cylinder off the scale, while the Sodium Hydroxide remains in the graduated cylinder. Next, the scientist took the beaker and the test tube and placed the two materials on the digital scale. The scientist pressed the zero on the digital scale to zero out the scale. While the materials stay on the scale, The scientist took the pipette and filled the pipette up with Copper Nitrate. The scientist poured the Copper Nitrate into the test tube
A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved.
This experiment investigated the properties of metals by seeing the reactivity of metals. The metals used in this experiment were lithium, sodium, potassium, magnesium, and calcium. What was the first chemical change observed in the lab? Explain.
All matter is made of particles called atoms. An atom is smallest unit of matter. A matter can be solid, liquid or gas. When a group of atoms bond together this makes a molecule. The molecule is the base of chemical compounds that is involved in chemical reactions.
For this experiment, the materials needed include an
Covalent bonding occurs when atoms share pairs of electrons. Another type of bonding is called a metallic bond. A metal bond is different form covalent and ionic bonds,
First, the group was assigned an amount of copper sulfate. Then, one group member measured out the copper sulfate while another member retrieved a beaker; it was filled with water. Both items were taken to the lab counter where a beaker was already placed. The copper sulfate was poured into the beaker. Afterwards, the beaker was placed on the hot plate.
The acid was allowed to be poured for a little longer before the flask was removed and taken to a lab bench with a buret that contained 0.1 M sodium hydroxide, and the amount of acid used was recorded. The sodium hydroxide was added into the flask in small amounts
Tare the scale. 4. Measure out 2g of NaOH pellets into the glass beaker. 5. Determine the mass of the beaker and NaOH together.
3) Distilled water was added to dissolve it. 4) The two electrodes were placed in the water while making sure that they were immersed in the solution but not touching each other or the surface of the beaker. 5) After about 10 seconds, the average of the readings were taken and recorded.
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
They were given the labels of “HCl”, “Na2S2O3”, and “water”, as was done to the beakers. The “water” syringe was then used to extract 2 mL of water from the “water” beaker. The syringe was examined to verify that no air bubbles were made in the syringe. The water was then translated into Well #3. Next, the “HCl” syringe was used, taking 1 mL of HCl from the “HCl” beaker, and then translated into Well #3 as well.
The buret is filled to a point above the "0" mL mark with NaOH solution. In order to fill the tip of the buret with liquid, the solution is drained out of the bottom until the meniscus lies between the "0" and "1" mL marks. The initial buret reading can now be recorded to the nearest 0.01 mL. If you have any doubts as to your ability to read the buret correctly, ask your instructor to check your initial reading. Standardization of NaOH solution Accurately weigh out a sample of approximately 0.3-0.4 g of primary standard potassium hydrogen phthalate, KHPh, which has been previously dried at 120°C.
The point of the experiment was to test how accurate and precise five pieces of lab glassware--an erlenmeyer flask, a pipette, a buret, and a graduated cylinder, and a 50mL beaker-- were for measuring water volume (mL). The tools used to determine the precision and accuracy were an electric scale, the provided 5 pieces of glassware, an extra beaker, a calculator, and 10 mL of H2O or water (distilled) per trial. The way to test the accuracy of a tool was to find how close the experimental volume of water in the given glassware was to the given theoretical volume, 10mL. Volume can be calculated with the formula mass/density = volume with the knowledge that water has a theoretical density of 0.997 g/mL under the lab conditions provided. To find
During a chemical reaction, atoms are rearranged, but they do not break apart, nor are they created or destroyed. Three is all atoms of a given element are identical in mass and other properties. four is the atoms of different elements differ in mass and other properties. The last is the Atoms of one element can combine with atoms of another element to form compounds. In a given compound, however, the different types of atoms are always present in the same relative
17) The outcome was cataloged. 18) The left and the right beaker are emptied and cleaned to execute the next test. 19) 18 millimolar of Na⁺Cl⁻ was put inside of the left beaker. 20) Deionized Water was poured into the right beaker.