Sodium silicate Essays

reaction would be higher. Those factors would affect the speed and the amount the atoms are moving at therefore effecting the amount that the particles collide and hence impacting the rate of reaction. The two reactants involved in the experiment are Sodium Thiosulfate

Objective: I will be combining calcium carbonate with hydrochloric acid as a case study to measure the rate of chemical reaction. This gives us the equation CaCO3 + 2HCl  H2O + CaCl2 + CO2 Background Information: Several factors are already known which increase (or decrease) the rate of reaction. An increase in concentration of the acid allows for a greater number of hydrochloric acid molecules colliding into those of calcium carbonate. Although not every single particle would result in a successful

Procedures 1.First thing needed is a plastic bag open the plastic bag and take about a teaspoon of calcium chloride, put the calcium chloride in one corner of the bag. Then take about a half teaspoon of sodium bicarbonate and put it in the opposite corner of the bag. Then lay the bag flat on the table use about 5 mL of phenol red. Once the phenol red is in quickly lift your bag and put all the substances in one corner. Then observe 2.Reference procedure one for first step.Lay bag down and add about

Nonosmotic Sodium Accumulation and Salt Sensitive hypertension As we discussed earlier, high sodium diet causes water retention and increases the blood pressure by increasing extracellular fluid volume. In contrast to this traditional view, Heer et al. 2000 performed an experiment in which they showed that consumption of high dietary sodium causes a relative shift of fluid from interstitial compartment to intravascular space. They selected 32 healthy male subjects and provided them with a diet rich

Conclusion: In Station 1- reaction 2, Station 3- reaction 1, Station 4-reaction 1, Station 5 reaction 1, Station 6-reaction 1 and 2, and Station 7- 1 and 2 there was chemical reaction because all of those mixed ionic compounds created a precipitate. However some solutions did not become insoluble and produce precipitates such as: Station 1- BaCl2 (aq) + KNO3 (aq) , Station 2- KNO3(aq) + AgNO3(aq) and KNO3(aq) + CaSO4(aq), Station 3- Na2CO3(aq) + KNO3(aq) , Station 4- NaPO4(aq) + KNO3(aq)

Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction:

In this lab, a total of 9 reactions were complete, mixing 3 powders and 3 liquids. The powders were baking powder, baking soda, cornstarch. The liquids were water, iodine solution, and acetic acid. Of these experiments, 5 were chemical reactions and 4 were only physical changes. Of the powders, baking powder was the most reactive because it chemically reacted with all 3 liquids. Baking soda and cornstarch both reacted with 1 out of the 3 liquids. Baking soda reacted with acetic acid. Cornstarch reacted

Introduction During this lab, students observed that not all substances dissolve at the same rate. Many factors involved including the independent and dependent variables affect how distinct substances dissolve. Overall, the chemical reaction, “the amount of reactant that changes the product in a given time”, played an important part in this experiment, when proven how a substance can change into another element by either emitting or absorbing energy. (Tro, 2018). Within the chemical reaction are

Factors affecting reaction rates (video) | Khan Academy (Khan Acadamey, n.d.) Research question: In the chemical reaction between 0.25m Sodium Thiosulfate solution and 1.0M of Hydrochloric solution, how will a variety of temperatures, between 10oC and 45oC the Sodium Thiosulfate solution, affect the time it takes for the chemical reaction to occur? Possible Hazard: Potential Risks: Control Measures: Hydrochloric Acid solution. -Potential skin

A safety audit for the gas-solid fluidization experiment was conducted. The following safety concerns were found when performing the audit: operating beyond the operational limits, spillage of the beads, risk of head injury from bending over to change the beads in the apparatus or from the low bar, and congestion of the workspace. One of the biggest safety concerns with this lab involved the small glass beads that acted as the solid in the experiment. If the gas flow rate goes below 50 standard cubic

Title : Determination of chemical formula of hydrate Aim To determine the chemical formula of hydrated Copper (II) sulphate, CuSO4 Research Background “When the chemical is heated the hydrate will convert to an anhydrous ionic compound (this means the water will leave it). The moles of H2O will be determined by assuming the amount of mass lost by heating is the mass of the evaporated H2O. The moles of the CuSO4 (the white substance after heating) can be calculated from the mass of the white crystals

Title: The effect of concentration on reaction rates Introduction: - The iodine clock reaction involves mixing two clear solutions and producing a new clear solution. Then, after several seconds, the solution turns dark blue. This can be used to measure how fast a reaction occurs which is known as chemical kinetics. The time taken for the reaction mix to turn blue can be measured with a stopwatch. The reactions that form the basis for the iodine clock reaction are shown below. Equation 1: H2O2 +

actual yield is 0.38 grams. So if 0.38 is divided by 0.49 and multiplied by 100 then the percent yield for Zinc Sulfide would be 77.6%. When it comes to Sodium Chloride, the theoretical yield is 0.58 grams and the actual yield is 0.45 grams. So when 0.45 grams is divided by 0.58 grams and multiplied by 100, the percent yield would be 77.5% of Sodium chloride. The actual yield is directly taken from the mass of the products in the experiment while the theoretical yield is determined by using stoichiometric

In cycle one, the double displacement reaction, Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) occurred, the result of the reaction was that the reaction mixture began to bubble with the copper filling dissolving and a vapor like substance leaving the reaction. Furthermore, when water was added, the color change, from brown to a blue color pigment. Then in Cycle two, another double displacement reaction occurred, Cu(NO3)2(aq) + 2NaOH(aq) → Cu(OH)2(s) + 2NaNO3(aq), which resulted in the reaction

If there is a change in concentration, temperature, volume, or total pressure the equilibrium will change in order to react to the change. This concept was shwon throughout the experiment by the adding of new reagents and temperature changes. This was shown by the mixing of NH4NCS and Fe(NO3)3. The two chemicals together produced a dark red FeNCS2+. Since the solution became a dark red, the concentration of FeNCS2+ had increased. The darker solution means that the products are more favored at equilibrium

The average concentration of my unknown Al3+ solution (#41) was 0.02372 0.00016 mol/L. My %RSD was 0.67%, which I would say is very good. This means my precision relative to my average was very good. When calculating the mass of the precipitate, my Trial #1 and #2 were both 0.271X, with Trial #3 being 0.27XX. Having Trial #1 and #2 being only 1 decimal place different from each other was very surprising to me, and indicated high precision. This led to a low standard deviation and a low %RSD. I think

The objective of the experiment was to try to figure out what the mystery powder was. I used a bunsen burner, four different types of liquids. We were given eight powders and one of these powders were our mystery powder. And each powder reacted different to the fire and the liquid. We had to go back into our notes and see what matched to what. Materials I used. Were a petri dish, scapula, liquids, burner, C-clamp, tongs, gas to start the flame, eight different types of powders, and the most importa

ADI Lab: Stoichiometry and Chemical Reactions The guiding question of this ADI lab was, “Which balanced equation best represents the thermal decomposition of sodium bicarbonate?” The goal of this lab was to use our knowledge of stoichiometry with the mole ratio to identify the correct chemical equation for the decomposition of sodium bicarbonate. Information that was given going into this investigation was the definition of the law of conservation of mass and the atomic theory which states that

Anthracene-9,10-bismethylmalonate (ADMA), Orange G and polystyrene (PS, Mw = 192,000 g/mol) were purchased from Sigma-Aldrich. Acetic acid (glacial), tetrahydrofuran (THF) and dimethylformamide (DMF) were purchased from Saarchem, while Rose Bengal was purchased from Fluka. Water collected from milli-Q water (Millipore corp., Bedford, MA, USA) was used for the preparation of all aqueous solutions. All solvents were dried prior to use using molecular sieves. BODIPY 1 was synthesized using the method

Stoichiometry of a Double Displacement Reaction The objective of this lab is to find the percent yield of a product of a double displacement reaction. Procedure: Refer to handout entitled “Stoichiometry of a Double Displacement Reaction” Materials: Refer to handout entitled “Stoichiometry of a Double Displacement Reaction” Data & Observations: Data Table Calculated Molar Mass of CuSO4•5H2O 249.677 g Calculated Molar Mass of CuO 79.545 g Starting mass of CuSO4•5H2O 2.050 g Mass of 100-ml beaker