You are a lab assistant preparing a solution of known concentration of phosphorus. You have pure trisodium phosphate (Na3PO4) towork with, and you weigh out 0.328 g of the solid and add it to a 1.00 L volumetric flask which is mostly full of DI water; you thenfill to the mark with DI water. The volumetric flask thus containsmg/L Na3PO4 solution.0.330.328O 328O none of the above Another source of phosphorus in water is known as organic phosphorus which commonly finds its way into natural bodiesof water from human and animal waste and food residues.If you wish to measure the phosphorus content due to organic matter in the water sample using thevanadomolybdophosphoric acid method, you must first "digest" the sample to convert the organic phosphorus toorthophosphate.O TrueO False

Hii there, As there are multiple question posted. we are answering first question. If you need…

You are a lab assistant preparing a solution of known concentration of phosphorus. You have pure trisodium phosphate (Na3PO4) to work with, and you weigh out 0.328 g of the solid and add it to a 1.00 L volumetric flask which is mostly full of DI water; you then fill to the mark with DI water. The volumetric flask thus contains mg/L Na3PO4 solution. O 0.33 O 0.328

You are a lab assistant preparing a solution of known concentration of phosphorus. You have pure trisodium phosphate (Na3PO4) to work with, and you weigh out 0.328 g of the solid and add it to a 1.00 L volumetric flask which is mostly full of DI water; you then fill to the mark with DI water. The volumetric flask thus contains mg/L Na3PO4 solution. O 0.33 O 0.328

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 20CR

See similar textbooks

Similar questions

Write an equatition for the reaction of methanol with sodium?
To analyze an aspirin sample, 0.3470 g of crushed tablets are weighed and treated with 50.00 mL 0.1155 M sodium hydroxide, boiling for 10 minutes. Under these conditions the acid acetylsalicylic (MW, 180) reacts according to: CH3COO-C6H4-COOH + 2 OH- → OH-C6H4-COO- + CH3COO- The excess NaOH is then titrated with 11.5 mL of 0.2100 M HCl. What is the purity of said show ?.
(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.
Dissolve 0.25g NaClI, 0.20g NaHCO3. 0.35g KCI, and 1.5g of glucose in 100 ml distilled water using a 250 mL capacity beaker. Use the formula to create a 60 mL ORS. Based on the given procedure, calculate the total amount of glucose in the prepared solution. (MW: Na: 23, K: 39, CI: 35, H: 1, C: 12, 0: 16) O 83.33 mmol/L 66.91 mmol/L 90.40 mmol/L 71.11 mmol/L O 23.81 mmol/L O 47.30 mmol/L
b) A carbonate of metal X has the formular X,CO3. The carbonate reacts with hydrochloric acid according to the following equation: X,CO3 + 2HC! → 0.25g of X,CO3 was found to neutralize exactly 23.6cm³ of hydrochloric acid of concentration 0.15moldm? ( RAM for C=12;0=16) i) Calculate the number of moles of hydrochloric acid 2XCl + CO2 +H,0 ii) Calculate the number of moles of X,CO3 iii) Calculate the relative molecular mass of X,CO3 iv) Calculate the relative atomic mass of X and hence deduce its identity c) Propanoic acid is a weak acid with an acid dissociation constant of 1.22x 10°moldm i) Write an equation for the ionization of propanoic acid -3 ii) Calculate the pKa for propanoic acid Lo iii) Sodium propanoate is made by the titration using 0.1M sodium hydroxide with propanoic acid A: Write an equation for the reaction B: Name a suitable indicator for this titration iv) A mixture of sodium propanoate and propanoic acid acts as a buffer solution. What is a buffer solution?
What is the chemistry behind fish fermentation process? Provide references and elaborate
Oral rehydration salts are stated to contain the following components: Sodium Chloride 3.5g Potassium Chloride 1.5g Sodium Citrate 2.9g Anhydrous Glucose 20.0g 8.342 g of oral rehydration salts are dissolved in 500 ml of water. 5 ml of the solution is diluted to 100 ml and then 5 ml is taken from the diluted sample and is diluted to 100 ml. The sodium content of the sample is then determined by flame photometry. The sodium salts used to prepare the mixture were: Trisodium citrate hydrate (C6H5Na3O7, 2H2O) MW 294.1 and sodium chloride (NaCl) NW 58.5. Atomic weight of Na = 23. The content of Na in the diluted sample was determined to be 0.3210 mg/100 ml. Determine the % of stated content of Na in the sample.
Oral rehydration salts are stated to contain the following components: Sodium Chloride 3.5g Potassium Chloride 1.5g Sodium Citrate 2.9g Anhydrous Glucose 20.0g 8.342 g of oral rehydration salts are dissolved in 500 ml of water. 5 ml of the solution is diluted to 100 ml and then 5 ml is taken from the diluted sample and is diluted to 100 ml. The sodium content of the sample is then determined by flame photometry. The sodium salts used to prepare the mixture were: Trisodium citrate hydrate (C6H5Na3O7, 2H2O) MW 294.1 and sodium chloride (NaCl) NW 58.5. Atomic weight of Na = 23. The content of Na in the diluted sample was determined to be 0.3210 mg/100 ml. Determine the % of stated content of Na in the sample. The stated should be 104.5, how??
A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.
write a chemical reaction scheme for the synthesis of salicylic acid from wintergreen based on the information provided below. Include the balanced chemical equation for the reaction being studied or conducted (reactants to products). indicate actual chemical structures that pertain to the experiment and indicate conditions as well as solvents over and under the reaction arrow.
Heat of Reaction, Mole Fraction 1. A group of students perform a series of experiments mixing HCI with an unknown base of the formula M(OH)n. For each trial the total volume of acid and base was 50.0 mL. The concentration of the acid and base solutions were 0.6000 M. The data is plotted in the graph provided. The density of the aqueous solution is assumed to be 1.00 g/mL and the specific heat of water is 4.18 J/g °C in joules 1600 1400 1200 1000 800 600 400 200 0 0.0000 0.6000 M HCI 0 2000 0.6000 M(OH)x 0 4000 0 6000 Mole Fraction of Acid 0 8000 10000 a) What is the limiting reagent at a mole fraction of 0.6 of acid? b) Write a balanced equation for the reaction of M(OH), with HCI. (You must determine "n") c) For one trial, the students measured a temperature change of + 2.9 °C. Calculate q. d) The students calculated a value of q of 1.5 x 10³ J for one of their trials. For this trial 0.015 mol of HCI and 0.015 mol of M(OH), were used. Calculate heat per mole for this reaction.
If one mixes 50cm³ of EtOH and 50cm³ of H2O at room temperature; will the total volume of the solution be 100.0 cm³? Justify answer with appropriate calculations and explanations