2. In mass balance calculation, non-steady & non-conservative conditions refer to: A. Change/Reaction 0, Input/Output #0 B. Change/Reaction # 0, Input/Output = 0 C. Change 0, Reaction/Input/Output # 0 D. Change #0, Reaction/Input/Output = 0 !! 3. Chemical thermodynamics CANNOT: A. predict direction of chemical reaction B. predict equilibrium concentrations C. calculate equilibrium constants D. predict reaction mechanisms 4. In chemistry, standard conditions refer to: A. T=25 °C, P=1 atm for gases, concentration 1 M for solutions B. T=0 °C, P = 1 atm for gases, concentration 1 M for solutions C. T= 25 °C, P = 1 bar for gases, concentration = 1 M for solutions D. T= 25 °C, P = 1 atm for gases, concentration =1 ppm for solutions 5. H,CO, +H* + HCO,, HCO, »H +CO; ,write the equilibrium equations [HCO J[H*] [H,CO,] А. Ка1 2; Ka,2 [HCO ][H*] %3D [HCO5] В. Ка1 2;Ka,2 [HCO,] [H2CO, ] Pe pH Diagram С. Ка, [HCO5][H*] ;Kaz [H,Co, ;Ka2 %3D [HCO] D. Ka1 = HCOJ[H*]. %3D [H,Co, J [HCO5] 6. When pH = pKa,1, which one is true? A. [H2CO3] > [HCO:] B. [H2CO3] = [HCO:] C. [H2CO3]< [HCO.] D. [H2CO3] = [CO?] 12

2. In mass balance calculation, non-steady & non-conservative conditions refer to: A. Change/Reaction 0, Input/Output #0 B. Change/Reaction # 0, Input/Output = 0 C. Change 0, Reaction/Input/Output # 0 D. Change #0, Reaction/Input/Output = 0 !! 3. Chemical thermodynamics CANNOT: A. predict direction of chemical reaction B. predict equilibrium concentrations C. calculate equilibrium constants D. predict reaction mechanisms 4. In chemistry, standard conditions refer to: A. T=25 °C, P=1 atm for gases, concentration 1 M for solutions B. T=0 °C, P = 1 atm for gases, concentration 1 M for solutions C. T= 25 °C, P = 1 bar for gases, concentration = 1 M for solutions D. T= 25 °C, P = 1 atm for gases, concentration =1 ppm for solutions 5. H,CO, +H* + HCO,, HCO, »H +CO; ,write the equilibrium equations [HCO J[H] [H,CO,] А. Ка1 2; Ka,2 [HCO ][H] %3D [HCO5] В. Ка1 2;Ka,2 [HCO,] [H2CO, ] Pe pH Diagram С. Ка, [HCO5][H] ;Kaz [H,Co, ;Ka2 %3D [HCO] D. Ka1 = HCOJ[H]. %3D [H,Co, J [HCO5] 6. When pH = pKa,1, which one is true? A. [H2CO3] > [HCO:] B. [H2CO3] = [HCO:] C. [H2CO3]< [HCO.] D. [H2CO3] = [CO?] 12

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 1P

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The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
By the use of Henderson Hasselbalch equation; pH = pKa + log{[acetate ion]/[acetic acid]} 4.5 = 4.75 + log{[0.10 M]/[acetic acid]} -0.25 = log{[0.10 M]/[acetic acid]} [Acetic acid] = 0.10 M/ 10-0.25 [Acetic acid] = 0.10 M/0.56 [Acetic acid] = 0.1786 M Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L = 0.025 mol Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow; w100% = 0.025 mol × 82.0343 g/mol = 2.051 g Weight (w) of sodium acetate (purity 99%) is calculate as follow; w99% = 2.051 g× (100/99) = 2.072 g What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.
An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.
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In lecture I mentioned that standard state is usually at 25oC; however, it can be at any specified temperature. In problems 9 and 10 you will calculate ΔGo from Ksp data. The Ksp range over the temperature range in these two problems is consistent with some actual solubility data; however, in order to allow each student to do their own calculation I have made this data for an "unknown" ionic solid. Calculate the value of ΔGo (kJ/mol) at 3.3oC for the dissolution of an ionic solid with a Ksp of 2.5 x 10-11 at 3.3oC. Your answer should have 2 sig figs.
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Phase equilibria data for the system water / acetone / trichloroethane phase equilibria data for the coexisting phases in mole% extract phase raffinate phase trichloroethane| acetone | water (trichloroethane| acetone water 80,18 o 0,07 59,01 . ) 0,10
The partition coefficient of ammonia between water and chloroform is wanted to be determined. The necessary quantities of ingredients are taken into the separation funnel, and the extraction process is applied. At the end of the extraction process, 5 mL portions of each of the water and chloroform phases are titrated with 0.1 M HCI in the presence of methyl orange indicator. If the volumes spent at the turning points are 7.2 and 5.1 mL, respectively, calculate the KSU, KLOROFORM (Dispersion coefficient) value.
. A solution was prepared by mixing 4.00mL of 2.00 x 10-3 M Fe(NO3)3 and 3.00mL of 5.00 x 10-3 M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture. [Hint: Use as many significant figures as you legitimately can in your calculations] my average you can find on the picture below PLS HELP ASAP!!
Calculate the solubility at 25°C of PbCO3 in pure water and in a 0.0110M PbNO32 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0110 M Pb(NO3)2solution: gL
1. Sodium carbonate is recovered as decahydrate from 1000kg of 5% solution of sodium carbonate in water. If it is desired that 95% of Na2CO3 is to be recovered as decahydrate by cooling to 278 K, determine the following: a) the mass of water evaporated (b) the mass of crystals obtained (Na2CO3 ∙ 10H2O). The solubility of Na2CO3 in water at 278K is 9.0% (weight) 2. A copra batch contains 44% oil and is to be extracted with n-hexane. The extracted meal contains 0.07 kg of oil/kg oil free matter and the mass fraction of n-hexane in it is 0.05. The extract contains 49% n- hexane. If 10,000 kg of copra are to be processed, how many kg of n-hexane are required and the determine the amount of extract. 3. Absorption of sulphur dioxide is carried out in a packed tower. Gas containing 14.8% sulphur dioxide and the rest inert gases enters the tower while the leaving gases contains 1% sulphur dioxide. Water flows at the rate of 1m3/min. The tower handles 7380 m3/hr of gas at 303K and 1 bar. Find…