0.05mol/6M=8.3*10-3 L=8.3mL stock solution c. 100mL-8.3mL=91.7mLwater Add 91.7 water to 6M stock solution to prepare 0.5M acetic acid. Exercise 8: a. 42.35 - 0.55 = 41.8 mL b. The moles of EDTA4- : 0.0189M*(41.8*10-3)L=7.9*10-4mol c. Zn2+(aq)+EDTA4-(aq)—Zn(EDTA)2-(aq) The ratio Zn2+ and EDTA4- is 1:1 The moles of Zn2+= the moles of EDTA4-=7.9*10-4mol d. 7.9*10-4mol*65.39g/mol=0.0517g Zn e.
Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 0.250 g H2SO4 x 1 mole x 1 L = 0.0102 L 98.12 g 0.250 mole 5. 1.50 g of NaCl is dissolved in 100.0 mL of water. Calculate the concentration. 6.
CO(g) + H2O(g) ↔ CO2(g) + H2(g) Suppose you start with 1.00 mol each of CO and H2O in a 50.0 L vessel. How many moles of each substance are in the equilibrium mixture if the Kc is 0.58? Homework Page 472 #5,6 Problem Sheet Equilibrium Constant Problems 1. What is the equilibrium composition of a reaction mixture if you start with 0.055 mol each of H2 and I2 in a 1.0 L vessel? The reaction is a synthesis.
Procedure Step 1, Obtain acid, in a 100 ml Erlenmeyer flask add 35 ml of .2M HCl solution. Step 2, add an indicator to the acid, select the flask and add 2 drops of phenolphthalein indicator. Step 3, Fill buret with NaOH, obtain a 50 ml buret and fill with .2M NaOH solution.Step 4, Titrate NaOH into HCl until end point, record initial buret volume and add NaOH (quickly at first then slowly) until the HCl solution turns pink and record the final buret volume of NaOH in buret. Step 5, repeat steps 1-4 using pH meters, add a pH meter to the acid solution. Record several points of pH and NaOH added (especially near equivalence point) to be use later to prepare a titration curve.
Now to begin, pour 50 mL of the sodium phosphate buffer solution with a pH of 6.84 into the 150 mL beaker. From here on out, the sodium phosphate buffer solution will be referred to as simply the buffer solution. Next, locate the indicator called bromothymol blue (0.04%) and add 20 drops to your 150 mL beaker. The solution should then appear green. Next, obtain a 5 mL serological pipet and thoroughly rinse it with the buffer solution, then discard the buffer solution into the 250 mL beaker.
Filter by suction then collect the dark solid. ANALYSIS FOR % HALIDE (X-) IN A SYNTHESIZED COBALT COMPOUND Preparation of silver nitrate in 150 mL beaker. Mixed 1.7806 of silver nitrate with 50 mL of deionized water and 10 drops of nitric acid. Then used 250 mL beaker and added as well as mixed 0.250 cobalt compound, 150 mL of water and 10 drops of nitric acid. Boiled for 45 minutes gently to collect silver (unknown).
[7.7(10-12 mol/L] 2. How many milligrams of PbI2 can you dissolve in 300 mL of water at 25(C? Ksp of PbI2 is 1.4(10-8 [210 mg] 3. Calculate the solubility product constant, Ksp, of SrCl2 if 8.0 mg dissolves in 200 mL to form a saturated solution at 25(C. [6.4(10-11] 4. Seawater is saturated with AgCl.
29.4 atm B. 4.89 atm C. 25.1 atm D. 36.0 atm _____ 5. The vapor pressure of pure ethanol at 60 °C is 349 mm Hg. Calculate the vapor pressure at 60 °C of a solution prepared by dissolving 10.0 mol of naphthalene (nonvolatile) in 90.0 mol of ethanol. A.
Collect 6 grams of copper (II) sulfate on weighing paper. Weigh and record. 5. Collect 50 mL of distilled water into the beaker. 6.
Experiment 8 DETERMINATION OF % COMPOSITION OF PENNIES USING REDOX AND DOUBLE DISPLACEMENT (PRECIPITATION) REACTIONS Introduction: The main purpose of the lab is to determine the percent composition of pennies using oxidation reduction and double displacement reactions and titration techniques. The quantitative determination of zinc is conducted by precipitation followed by isolation and weighing of the Zn(OH)2 precipitate (gravimetric analysis). My expected results were that 97.5% of the penny would be zinc, and 2.5% would be copper. Experimental Procedure: 1. Obtain beaker filled with 250 mL of HCl and 5 pennies.