Calculate the molarity of a solution in which 360. grams of glucose, CSH12OS, are dissolved in enough water to make 250. mL of solution. (A) 1.0 M (B) 2.0 M (C) 4.0 M (D) 8.0 M
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A: Given: Normality of CaCO3 = 1.13 N And volume of solution = 1826 mL = 1.826 L…
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A: The given data contains, Volume = 3.00 L. Molarity = 0.500 M.
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A: Given, Concentration of NaCl solution = 0.87 M Volume = 500 ml = 0.5 L
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A: Given: The molar mass of KI=166 g/mol. The volume of the solution=125 mL=0.125 L. The molarity of…
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A: Given : Mass of water = 0.1151 Kg = 115.1 g…
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A: Molarity :- It is the number of moles of the solute dissolved per liter of the solution. It is…
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A: Given :- mass of NH3 = 6.50 g Volume of solution = 125 mL To be calculated :-…
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A: Given : Molality of sodium acetate = 0.500 m And moles of sodium acetate = 1.00 mol Since moles of…
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A: Answer is explained below. To calculate the molality of the aluminum phosphate solution first we…
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A: Given : Mass of CH3COONa i.e solute = 6.08 g And volume of solution = 0.750 L
Q: 4. How many grams of NaCl would you need to prepare 200.0mL of a 5M solution.
A: To determine the mass of NaCl dissolves in 200.0ml Given The molality of the solution is 5M The…
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A: Molarity (M) of a solution is defined as the number of moles of solute dissolved per volume of the…
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A: Given Mass of MgCl2 = 15.5 g Molar mass of MgCl2 = 95.2 g/mol Volume of solution = 250 ml = 250÷1000…
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Q: How many grams of water must be added to 48.8 g of NaOH in order to prepare a 5.46%(m/m) solution?
A: Mass of NaOH = 48.8 g % m/m = 5.46 % Calculation of mass of solution: % m/m=Mass of NaOHMass of…
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A: The given data: The mass of NaOH = 0.4 g. The volume of water = 100 cm3 = 100 mL. To determine = The…
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A: Answer :- -3.72 (°C) 2.00 m CH3OH(aq) solution freeze at -3.72 °C…
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A: Given details, Volume = 500 mL = 0.5 L Molarity = 0.2 M To calculate the mass in grams.
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A:
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A: %(w/v) = (100 x Mass of solute in g)/Volume of solution in mL %(w/v) = (100 x W)/V
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A:
Q: 7. Calculate the normality (N) of a 500 ml. solution containing 20 gms of NaOH (Mm 40 g/mole),
A: Molarity of the NaOH = ( mass of NaOH /molar mass of NaOH • volume of the Solution ) Molarity of…
Q: What mass of ammonium sulfate, (NH4)2SO4 must be added to prepare 200.0 g of a 3.5% solution of…
A: 3.5% Solution of (NH4)2SO4 means 100g solution of ammonium sulfate contains 3.5g (NH4)22SO4.
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A: Since you have posted multiple questions, we will solve the 1st one for you. Kindly post the other…
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Q: 2. How many mole of nickel(II) nitrate are required to prepare 5.00 L of a 0.025M solution?
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Q: How many grams of calcium chloride (CaCl2) must be added to 45.0 g of water to prepare a 8.80% (m/m)…
A: since % (m/m) is defined as the mass percent of solute in the solution i.e % (m/m) = mass of solute…
Q: what is the Freezing point oF an that boils at lo5Ĉs Jiven that aqueous Solution KF =1.86
A: Given: The boiling point of the solution, (Tb of solution)=1050C. The molal boiling point elevation…
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- Using the percent purity calculations, determine the percent yield of synthesis of aspirin. Part I Synthesis of Aspirin Mass of salicylic acid used (g) 2.029g Volume of acetic anhydride used (mL) 5ml Mass of acetic anhydride used (vol. × 1.08 g/mL) 5.4g Mass of aspirin synthesized (g) 3.256g Part II Melting Temperature Data Melting temperature (°C) 133°C Part III Salicylic Acid Standard Stock Solution Initial mass of salicylic acid (g) 0.210g Moles of salicylic acid (mol) 0.0147 mol Initial molarity of salicylic acid (M) 0.724 M Part III Beer’s Law Data for Salicylic Acid Standard Solutions Trial Concentration (M) Absorbance Water (mL) 1 10 0.301 0 2 7.5 0.219 2.5 3 5.0 0.163 5.0 4 2.5 0.074 7.5 Best-fit line equation for the salicylic acid standards Test of the Purity of the Synthesized Aspirin Initial mass of aliquot of product (g)…7. Consider a1Msolution ofNa3AsO4. Write the charge and mass balance equations for this system. (please type answer not write by hend)Determine the percentage Fe in a sample of limonite from the following data:Sample : 0.5000g ; KMnO4 used = 50.00 ml ; 1.000ml of KMnO4 is equivalent 0.005317 g Fe,FeSO4 used = 6.00 ml; 1.000ml FeSO4 is equivalent 0.009200 g FeO ( ans 44.59 %)
- Prepare 50ml of approximately 1000ppm Mn stock solution from MnCl2*4H2)You are supplied with the following: / Jy word voorsien van die volgende: NaCl(Mr= 58,443 g /mol) 2.5MTris-Cl, pH 8 solution /oplossing (1 Litre) EDTA,natriumsout(Mr= 380,2g/mol) 10% sodium dodecyl sulphate solution / natriumdodecyl sulfaat oplossing Proteïnase K solution / oplossing (50 mg dissolved / opgelos in 1 ml ddH2O) You need a digestion buffer consisting of the following: / Jy moet 'n verteringsbuffer op maak wat uit die volgende bestaan: 15m M NaCl 75 mM Tris-Cl,pH 8 16 mM EDTA,pH 8 0.8% sodium sulphate / natrium dodecyl sulfaat 0,75 mg/ml proteïnase K How will you prepare 500 ml of the digestion buffer? Show all your steps and calculations. Remember to explain exactly how you will make it up.Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices
- The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.The %purity of a powdered crude sample of Na2CO3 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. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole numberThe %purity of a powdered crude sample of Na2CO3 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 CASE does this experiment satisfy?
- show solutions pls. thanksHow to prepare the solutions listed below Solution 1) 25 mL 7 M sulfuric acid and the respective dilution of this solution to prepare 50 mL 2 M sulfuric acid in deionised water. Sulfuric acid Mw = 98.079 g mol-1 Sulfuric acid density = 1.84 g mL-1 Sulfuric acid purity = 98% Solution 2) 100 mL 0.02M potassium permanganate potassium permanganate Mw = 158.03 g mol-1 potassium permanganate purity = 99%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. 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?