Concept explainers
(a)
Interpretation:
To determine the composition of the crystalline product.
Concept introduction:
Crystallization is the process in which the solute particles are separated as a crystal in the solids in highly organized form which may retain suspended in the mother liquid. This process is generally utilized for the purpose of purification of impure sample.
(b)
Interpretation:
To estimate the required feed and vapor flow rates in kg/h, and the rate at which MgSO4 could be recovered from the crystals.
Concept introduction:
Crystallization is the process in which the solute particles are separated as a crystal in the solids in highly organized form which may retain suspended in the mother liquid. This process is generally utilized for the purpose of purification of impure sample.
Evaporation simply involves the conversion of a liquid to its vapor form.
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Chapter 6 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- We want to determine the purity of alum sample bought in a local pharmacy in Miagao. A Chem 28 student determined the purity gravimetrically of a sample of alum, K2SO4:Al2(SO4)3:24H20. A 1.5879-g sample was dissolved and the aluminum precipitated as Al(OH)3. The precipitate was collected by filtration, washed, and ignited to give a product Al203 weighing 0.1572 g. Show your calculation to determine the purity of the alum sample.arrow_forwardA quantity of methyl acetate is placed in an open, transparent, three-liter flask and boiled long enough to purge all air from the vapor space. The flask is then sealed and allowed to equilibrate at 30°C, at which temperature methyl acetate has a vapor pressure of 269 mm Hg. Visual inspection shows 10 mL of liquid methyl acetate present.(a) What is the pressure in the flask at equilibrium? Explain your reasoning.(b) What is the total mass (grams) of methyl acetate in the flask? What fraction is in the vapor phase atequilibrium?(c) The above answers would be different if the species in the vessel were ethyl acetate because methyl acetate and ethyl acetate have different vapor pressures. Give a rationale for that difference.arrow_forwardYou are required to prepare 5 L of a solution containing 1.000 x 103 mol/L of Cu2"(aq). Which of the following procedures would produce an appropriate solution? O Dissolve 0.0636 g of copper metal in nitric acid, add to a 5.000 Lvolumetric flask, dilute to the mark with deionized water and mix well. O Dissolve 1.248 g of CuSO.5H,0(s) in deionized water, add to a 5.000 L volumetric flask, dilute to the mark with deionized water and mix well. Dissolve 0.250 g of CUSO,.5H,O(s) in deionized water, add to a 5.000 L volumetric flask, dilute to the mark with deionized water and mix well.arrow_forward
- A 25mL volumetric pipet is used to deliver a sample of the stock solution marked “0.6000M X2SO4” into a 100mL volumetric flask. Distilled water is added to the flask until it is about 3/4thfull, the solution is mixed well, then more water is added to fill it up to the calibration mark, then it is mixed again. Calculate the concentration of X+ion in the dilute solution made above.arrow_forward4. (cont.) (e) CO2 (g) + H20 (1) → 5. Balance the following equations; write the ionic equations and the corresponding balanced net ionic equation with the proper phase symbols (if different from the ionic equation). H2SO4 (aq) + NaOH (ag) > Na2SO4 (aq) + H20 (1) (a) (b) Al203 (s) + HCl (aq) → AIC13 (aq) + H20 (1) (c) H2SO3 (aq) КОН (aq) > K2SO3 (aq) + H20 (1) (d) HC2H3O2 (aq) + Ca(OH)2 (aq) →. Ca(C2H3O2)2 (aq) +. H20 (1) 55arrow_forwardSO4 -two content in 7689mL of a water sample was precipitated as Na2SO4. The precipitated was filtered, washed and calcined in an empty crucible with a mass of 27.0234g. The mass of the crucible plus Na2SO4 (142g/mol) was 27.7708g. Calculate the %m/v of Na (23g/mol) and the concentration of Na in the sample in ppm.arrow_forward
- The % purity of a powdered crude sample of Na^2CO^3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What is the % purity of the sample to the nearest whole number?arrow_forwardThe % purity of a powdered crude sample of Na^2CO^3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. Write the balanced chemical equation of the reaction in your solutions sheet. What is the sum of all the coefficients of the balanced chemical equation? Determine the pressure of the trapped gas inside the eudiometer in mmHg. Determine the partial pressure of the collected CO^2 in mm Hg. How many millimoles of CO^2 was collected? What is the % purity of the sample to the nearest whole number?arrow_forwardA 600.0 mg sample consist only of CaC2O4 and MgC2O4 was heated at 500°C converting the two salts to CaCO3 and MgCO3. The resulting precipitate weighed 465.0 mg. If the sample had been heated at 900°C, the products would be CaO and MgO, what would the mixture of oxides weigh? (FW: CaC2O4=128.1; MgC2O4=112.3; CaCO3=100.1; MgCO3=84.31; CaO=56.08; MgO=40.31)arrow_forward
- 1)Please express the normal salt (NaCl) concentration in body fluid into molarity (mM).2) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9%. solution. Please convert it into molarity.3) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.4) The above reaction has the product Ammonia, which when dissolved in 650 mL ethanol makes an alkaline ethanolic solution. Find its molarity (M) 5) Calculate the adult dose as per the BW of the baby. (Child dose-50 mg and the BW of the baby is 48 lb (British pound) (1lb=0.453 Kg)arrow_forwardThe calcium (AW= 40.08 g/mol) from a sample of limestone weighing 607.4 mg was precipitated as calcium oxalate hydrate (CaC204.H20, FW 146.12 g/mol) and ignited to calcium carbonate (CaCO3, FW= 100.09 g/mol) weighing 246.7 mg. (c) If the precipitate had been ignited at a higher temperature giving calcium oxide (CaO, FW= 56.08 g/mol), what would be its weight?arrow_forward(a) The heat evolved upon dissolution of atmospheric ozone into water is determined to be +5 kcal/mol at 298 K. Given that ozone has a Henry’s constant of 9.4 × 10−3 mol/L/atm at 298 K, determine its Henry’s constant at 273 K. Note that the definition of Henry’s constant is for the process air to water. (b) If the atmospheric ozone concentration in a polluted air is 100 ppbv, what is the concentration in equilibrium with a body of water in that region at 298 K? Note that you need to assume no losses of ozone other than absorption into waterarrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
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