An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. Identify the solid in the balanced equation. A) (NH4 )2 SO4 B) Pb(NO3 )2 C) PbSO4 D) NH4 NO3 E) There is no solid formed when the two solutions are mixed. ____ 11. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride.
White precipitate shows the presence of chloride (Cl-). Chloride anion equation: HCl(aq) + AgNO3 (aq) → HNO3 (aq) + AgCl(s). The nitrate anion test involves cooling a mixture containing 1 mL of test solution and 3mL 18M H2SO4. 2mL is poured down the inner test tube side and the presence of a brown ring shows nitrate (NO3-) to be present. The carbonate anion test mixes 1 mL of test solution and drops of 6M HCl.
Give an example of each of the following solutes: a. Ions/electrolytes sodium b. Colloids proteins c. Nonelectrolytes glucose 6. List the major extracellular and intracellular cations and anions a. Extracellular cations: sodium, potassium, calcium, & magnesium anions: bicarbonate, sulfate, phosphates, & chloride b. Intracellular cations: sodium, potassium, & magnesium anions: bicarbonate, sulfate, phosphates, & chloride 7. Within a fluid compartment, the total number of positive charges must be equal to the total number of negative charges. 8. Name four of the seven functions given for electrolytes: a. secondary active transport b. muscle contraction c. cofactors for enzymes d. action potentials 9.
Purpose: To investigate the physical and chemical properties of pure chemical substances. Observations and Experimental Data: Data Table 1: Solubility or Reaction Substance Name Color Odor Effect of Heat Cold H2O Hot H2O Litmus Test Dilute HCl Dilute NaOH Mg Silver odorless nothing bubbles bubbles No color change Bubble,fizz Slightly frothy cloudy No apparent change Cu Copper Odorless Turns darker black No apparent change No apparent change Lighter blue Holes in copper ball bubbles Dark spots on copper Zn Silver Odorless Liquid Solid Solid Lighter blue Bubbles fizzes No apparent change MgO white odorless Dark grey Cloudy Cloudy Lighter blue Fizzed bubbled Cloudy no bubbles CuCO3 green odorless pops Cloudy green h2o dissolved Turns dark green pops Blue-from pink Fizzed dissolved Turns blue Cu(NO3)2 blue odorless Melts boils Light green liquid Dissolved boils Blue-from pink Dissolved green liquid Blue bubbles NaCl white odorless crackesl Grain in h2o no bubbles Stays granular Lighter blue No apparent reaction bubbles Questions: A. Did you observe any chemical changes in this experiment? Yes. B.
For zinc ion to react, the NaEDTA must also be an ion in the solution which means that the large salt must be dissolved in water. Procedure 1) Weighed out 3.64 of NaEDTA on an electronic beam balance 2) Added this mass of NaEDTA using wide mouth funnel to a 250 mL volumetric flask. 3) Rinsed the funnel with a squirt bottle containing deionized water making sure none of the solid remained in the funnel. 4) Added about 100-200 mL of deionized water to the volumetric flask containing the solid NaEDTA. 5) Swirled the solution until the NaEDTA (s) dissolved entirely.
| Observations of Chemicals | Zinc Sulfate | Powder of a white solid | Barium Iodide | Powder of a white solid. | Deionized water | Liquid, transparent. | Trial # | BaI2 | ZnSO4 | Theoretical Yield of ZnI2 | Actual Yield | Percent Yield | 1 | .67g | .45g | .499820g | .52g | 104% | 2 | .67g | .45g | .499820g | .52g | 104% | 3 | .66g | .46g | .493117g | .48g | 97% | Calculations for Cost | Double Replacement | Synthesis | 0.48 grams of Zinc Sulfate - $0.02 | 1.00 gram Granular Zinc - $62.50 | 0.67grams of Barium Iodine Dihydrate - $0.886 | 2.00 gram Iodine - ($74.90 × 2) - $149.80 | 0.52 grams of Zinc Iodide - $0.906 | 1.00 gram zinc - $0.212 | 1000 grams of Zinc Iodide = $1,923.00 | 1000 grams of Zinc Ioidide = $212.30 | Focus Question Should chemists prepare Zinc Iodide, from its Elements or from a Double Replacement Reaction between Barium Iodide and Zinc Sulfate?
Acid test= solid + 3M Acetic acid cloudy + 6 ZnO ZnO + Heat yellow Zn Cooled White + ZnCO3 + heat yellow solid. Yellow solid cooled white solid + QUANTITATIVE DATA AND CALUCATIONS Desired Results Calculations Temperature of Water Bath 22.8oC Vapor Pressure (as
If the reaction is first order, its graphical representation is seen as ln[A] (natural log of concentration) vs. time, and the slope of its like is also the negative rate constant. Finally, for a second order reaction the graph is shown as 1/[A] (inverse of concentration) vs. time, and the slope of its given line is the positive rate constant. By understanding the rate law and finding the value of the correct rate constant with respect to the order of the reaction, one can determine the half-life of the crystal violet. This is because the crystal violet undergoes a decay reaction with the sodium hydroxide. According to Beer's Law, the absorbance of crystal violet is proportional to its concentration.
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. Part C: Density of an unknown NaCl solution was measured and a calibration curve used to determine the percentage of NaCl by mass in the solution. y=0.007x + 0.998 which concluded that the concentration of the sodium chloride solution was 3.14%. INTRODUCTION Anything that you can see, touch, taste or smell, occupies space and has mass, it is called matter. Matter can be a gas, a liquid,
Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3. The general formula of barium chloride hydrate is BaClg-nHZO, where n is the number of water molecules. Calculate the theoretical percent water for each value of n—divide the sum of the atomic masses due to the water molecules by the sum of all the atomic masses in the hydrate, and multiply the result by 100. Complete the table. | BaCl2 | BaCl2•H2O | BaCl2•2H2O | BaCl•3H2O | Sum of atomic masses (BaCl2) | 208.23 | 208.23 | 208.23 | 208.23 | Sum of atomic masses (nH2O) | 0 | 18.02 | 36.04 | 54.06 | Sum of atomic masses (hydrate) | 208.23 | 226.25 | 244.27 | 262.29 | Percent water in hydrate (theoretical) | 0% | 7.96% | 14.75% | 20.61% | In this lab we used a Balance, centigram