Molarity of KMNO4 solution (M) from bottle Final reading of buret (KMNO4) (mL) Initial reading of buret (KMNO4) (mL) Volume of KMnO4 solution (mL) Moles of MnO4 used for titration (mL)
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Q: A student is in a hurry and all his trials are hot pink. Is his calculated molarity too high or too…
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Q: Refer to picture below. What is the pAg of the solution after addition of 5.00 mL AgNO3?
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Q: A. Dilution of Stock Solution Concentration of STOCK solution you prepared (M) 0.8 Volume of STOCK…
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Q: (1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she…
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Q: A 0.786 g sample of KHP is dissolved in 50 mL of water and titrated with KOH. The initial burette…
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Q: A stock solution will be prepared by mixing the following chemicals together: 3.0 mL of 0.00200 M…
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Q: What is the molarity of a sodium chloride solution where 5.65 g of NaCl is dissolved into 500.0 mL…
A: We have given that Initial molarity of NaCl = 0.650M Initial Volume of NaCl = 500mL If we add…
Q: Redox Titration 2 KMnO4 + 5 (COOH)2 + 3 H2SO4 -------> 10 CO2 + 2 MnSO4 + K2SO4 + 8 H2O
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Q: Question 4
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Q: In the laboratory you dissolve 19.2 g of zinc bromide in a volumetric flask and add water to a total…
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Q: Standardization of NaOH Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 0.785 0. l690g 0.8239 Mass of KHP…
A: The mass of KHP used in trial 1, trial 2 and trial 3 is 0.785 g, 0.690 g and 0.823 g, respectively.…
Q: A 50.0 mL sample of 0.108 M H2SO4 is diluted to 250.0 mL. What is its new molarity?
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Q: The molarity of 0.2N HClO4 is ___________ . Group of answer choices 0.05 0.2 0.4 0.1
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Q: KHP + NaOH—> KNaP +H2O Data of trial Mass of KHP : 0.8085 Initial buret containing NaOH reading:…
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- Which of the following methods of preparing 0.0010M HCl solution from 1.0M stock HCl Solution willyield the smaller overlall uncertainty? a. A one step Dilution that uses 1mL(±0.006) pipet and 1000mL(±0.30) Volumetric Flask, or b. A two-step dilution that uses 20mL (±0.03) pipet and a 1000mL(±0.30) volumetric flask and a25 mL (±0.03) pipet and a 500mL(±0.20) volumetric flask for second dilution.Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?The partial molar volumes of acetone and chloroform, in a solution in which the molar fraction of chloroform is 0.4693, are 74.166 cm3mol-1 and 80.235 cm3 mol-1, respectively. What is the volume of 1,000 kg of this solution? Data: M.M. (acetone) = 58.08 gmol-1; M.M. (chloroform) = 119.07 gmol-1.
- C7H21O4NHCl(aq) + NaOH(aq) ---> C17H21O4N(aq) + H2O (l) + NaCl(aq) When a 25mL of aqueous solution that contains 62.50g of the salt is treated with NaOH, the salt is converted to pure cocaine. How much water in litres is needed additionally to dissolve the formed pure cocaine?What would be the boiling point of 500 mL of chloroform if 10.50 grams of caffeine (molar mass = 194.19) was added? The normal boiling point of chloroform is 61.3oC, the density of chloroform is 1.49g/mL, and the Kb of chloroform is 3.63 oC/m. Only enter the numerical value for the answer. DO NOT include a unit.Submit a clean, dry, and properly labeled 50-mL reagent bottle for your unknown solution. Pipet 20.00 mL of the sample in 250-mL Erlenmeyer flask. Add 5 mL of buffer and 5 drops of indicator. Titrate the solution until it turns light blue. If the titration consumes more than 50 mL of the titrant, dilute the sample accordingly. Compute for ppm of CaCO3 using the following table. Mean Molarity = 2.487 x 10^-3 MBlank correction = 0.015 Formula = V (mL) titrant x Mean Molarity of Titrant x Molecular weight of CaCO3 x 1/V (L) sample
- 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.5-7: A 10.34 molal aqueous nitric acid solution was prepared. (Density of nitric acid = 1.51 g/mL, density of water = 1.0 g/mL, and the MW of nitric acid = 63 g/mol)5. How many grams of HNO3 were used to prepare the solution? 6. What is the Molarity of the solution? 7. What is the concentration (%v/v) of the solution? 8-10: An aqueous solution of HNO3 was prepared having a molal concentration of 6.29. (Atomic weights: H=1 amu, N=14 amu, O=16 amu, density of H2O = 1g/mL, density of HNO3 = 1.51 g/ml)8. How many grams of HNO3 was used to prepare the said concentration? 9. What is the molarity of the aqueous HNO3 solution? 10. The % v/v of the prepared HNO3 solution is __________.Prepare the following solutions: 100.0 mL 0.0500 M stock Ca2+ solution 50.0 mL 0.0050 M working standard Ca2+ solution from 0.0500 M Ca2+
- Calicheamicin gamma-1, C55H74IN3O21S4, is one of the mostpotent antibiotics known: one molecule kills one bacterialcell. Describe how you would (carefully!) prepare 25.00 mLof an aqueous calicheamicin gamma-1 solution that couldkill 1.0 x108 bacteria, starting from a 5.00 x 10-9M stocksolution of the antibiotic.12 g of unknown organic sample was dissolve in 706 mL of Dicloromethane (DCM). The boiling point of benzene was increased by 2.72oC. Determine the molecular weight of the unknown sample? Kb of DCM = 2.42oC/m Bb of benzene = 39.6 oC density of benzene = 1.33 g/mL at 25 °C Round your answer to the nearest whole number, no units required.When 1 mole of water is added to an infinitely large amount of an aqueous methanol solution having a mole fraction of methanol of .40, the volume of the solution increased by 17.35cm^3 and 25C. When 1 mole of methanol is added to such a solution, the volume increases by 39.01 cm^3. Calculate the volume of a solution containing .40 mole of methanol and .60 mole of water. What is the volume of .6 mole of water plus the volume of .4 mole of methanol before they are mixed? The densities of water and methanol at 25C are .998g/cm^3 and .791g/cm^3 respectivley.