Chapter 2 22. A student heats 0.5585 g of iron with 0.3550 g of sulfur. She reports that she obtains 0.8792 g of iron sulfide and recovers 0.0433 g of unreacted sulfur. Show by calculation whether or not her results obey the law of conservation of mass. Total mass initial = 0.5585 g + 0.3550 g = 0.9135 g Total mass final = 0.8792 g + 0.0433 g = 0.9225 g These two values should be equal by the law of conservation of mass. These results do not obey the law of conservation of mass. Possibly she
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Hydrogen Tartrate Wang Haina 1. Aim 1. To determine the solubility of potassium hydrogen tartrate (KHT) at various temperatures from 10°C to 50 °C‚ and determine the corresponding Ksp at these temperatures. 2. To obtain the changes in enthalpy and entropy of the dissolution of KHT from the dependence of Ksp on temperature. 2. Results and discussion 2.1 Collection of data A portion of KHT (1 to 1.5 g) was added into about 100 mL of deionised water to prepare a saturated KHT solution. Several
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the limiting reactant‚ also to find the percentage yield and percentage purity of the reaction that happens between Calcium Chloride and Sodium Carbonate. The other purpose was to know how the reaction can be balanced and created. Hypothesis: In this lab we are going to see a precipitation reaction. This is a reaction where two soluble salts Sodium Carbonate and Calcium Chloride are added together and the result is the precipitation of single Product while the other product remains in solution
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in enthalpy (H°) and the change in entropy (S°)‚ the equilibrium constant (Ksp) was determined for the dissolution of borax in water. In procedure one of the experiment‚ the temperature of the borax solution was varied and its saturation level was measured at different temperatures (10°‚ 30°‚ 40°‚ 50°). In procedure two‚ the concentration of the borate anion was measured through a titration with 1.00 M HCl. Equation 6: Ksp= [Na+]2 [[B4O5(OH)4]2-]= (s)(2s)2=
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CHEMICAL COMPOUNDS “Analytical chemistry -I” http://foricseandbeyond.blogspot.in/ metal oxide “Oxides of metals are generally stable to heat and they are considered to be most stable form of compound found in nature.” Oxides of potassium‚sodium‚calcium‚magnesium‚ aluminum ‚ zinc‚iron‚lead and copper are stable to heat uO C PbO Zn O http://foricseandbeyond.blogspot.in/ MERCURIC OXIDE “Mercury(II)oxide” “orange red” 2HgO 2Hg + O2 1.The amorphous powder changes to dark
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Reaction 4- My hypothesis for reaction 4 is that adding hydrochloric acid to solid calcium carbonate produces bubbles maybe. When burning the splint is placed on the test tube‚ the flame is extinguished. Reaction 5- My hypothesis for reaction 5 is that mozzy zinc in the test tube will make smoke come out of the tube Reaction 6 - My hypothesis for reaction 6 is that when you add the 0.5 M of copper (11) chloride and mix it with the 0.5 M of sodium phosphate they will
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CHE 151-50 Fall 2013 Lab report Isolating the Components of a Three Component Mixture The purpose of this experiment was to separate the component of three mixtures sand‚ sodium chloride and calcium carbonate then calculate the percentage by mass of each component recovered from the mixture. The other purpose of this experiment was to show us the students the concepts associated with physical and chemical properties of substances. Me and my lab partner‚ obtained a mixture of a un known
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PATHOPHYSIOLOGY FOR THE HEALTH PROFESSIONS CHAPTER 6: FLUID‚ ELECTROLYTE‚ AND ACID-BASE IMBALANCES Fluid Imbalance Review of Fluid Imbalance -Water carries nutrients into cells and removes wastes‚ transports enzymes in digestive secretions‚ and moves blood cells around the body. Fluid Compartments -Approximatley 60% of an adult’s body weight consists of water -Infant’s body weight is about 70% -Fluid is distributed between the intracellular compartment (ICF)‚ or fluid inside the
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mol) / 0.025L = 0.03785 mol/L Ksp = [K+][HC4H4O6-] = (0.03785 ÷ 1mol/L) x (0.03785 ÷ 1 mol/L) = 1.433 x 10-3 1/T = 1/(28+273.15) = 3.6 x 10-3 ln Ksp = ln (1.433 x 10-3 )= -6.548 1/Temperature(1/K) (10-3 ) | ln Ksp | 3.3 | -6.548 | 3.5 | -6.92 | 3.4 | -6.801 | 3.2 | -6.07 | 3.1 | -5.384 | Table 2: The inverse of different temperatures and the ln for their respective Ksp. Graph 1: Graph of ln Ksp against 1/T Graph 1 is a graph of ln Ksp against 1/T. It is a linear graph
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buffers Henderson-Hasselbach equation buffer capacity buffer range SA/SB titration curve WA/SB titration curve equivalence point pH at equivalence pt buffer region pH at midpoint solubility product constant insoluble Ksp slightly soluble Ksp soluble Ksp Short problems: (about 45 points) 1. Calculate [H3O+] and [OH-] for a KOH solution with pH = 9.36. ------------------------------------------------- ------------------------------------------------- [H3O+] =
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