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Q: Complete the table. Element Moles Mass Cr 0.00442 Fe 73.5 mg Ti 1.009 x 10-3 Hg 1.78 kg
A: Mole is represented by the symbol mol. It is unit of measurement of substance. Mass is defined as…
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A: Given :- Mass of Fe = 89.4 g Mass of C = 2.50 g Mass of Cr = 1.47 g To calculate :- Percent by…
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A: Given: Mass of carbon in the sample = 10.0 g Mass of hydrogen in the sample = 2.5 g Mass of oxygen…
Q: Please help Element Moles Mass Cr 0.00450 _____ Fe _____ 84.0mg Ti 1.075×10-3 _____ Hg _____ 1.50…
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A: Mole= mass of Mg / molar mass of Mg Given - 1) mass of Mg =76.9 2) Molar mass of Mg=…
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A: Given :- Molecular mass of compound = 164.12 g/mol composition of C, H, & O are 58.54%, 2.46%,…
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A: Mass of oxygen added = 35.1556 - 35.0079 g Mass of Oxygen = 0.1477 g Moles of oxygen = mass / molar…
Q: 1. A sample containing only CaCO3 (100.0869) and MgCO3 (84.3139) was ignited and carbonates…
A: Molar mass of CaCO3 = 100.0869 g/mol Molar mass of MgCO3 = 84.3139 g/mol Molar mass of CaO = 56.0774…
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- A 0.7336-g sample of an alloy that contains copper and zinc is dissolved in 8 M HCl and diluted to 100 mL in a volumetric flask. In one analysis, the zinc (At. Mass = 65.38 g/mol) in a 25.00-mL portion of the solution is precipitated as ZnNH4PO4, and isolated as Zn2P2O7 (FM = 304.70g/mol), yielding 0.1163 g. The copper (At. Mass = 63.55 g/mol) in a separate 25.00-mL portion of the solution is treated to precipitate CuSCN (121.63 g/mol), yielding 0.2383 g. Calculate the %w/w Zn and the %w/w Cu in the sample.A 0.4740-g pesticide sample was decomposed by wet ashing and then diluted to 200.0 mL in a volumetric flask. The analysis was completed by treating aliquots of this solution as indicated. Calculate the percentage of copper in the sample.Pls give with reason, the type and name of the reaction.
- A. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgOGive typed full explanation A stock solution of lithium phosphate (Li3PO4, MM= 115.794361 g/mol) is prepared by dissolving 295.8 g Li3PO4 in deionized water to a final total volume of 1.000 L. Suppose a 1.000-mL aliquot is taken from this stock solution and transferred to a new container to which deionized water is added until the total volume is 50.00 mL. A new 1.000-mL aliquot is taken from this 50.00 mL solution and transferred to a third container to which deionized water is added until the total volume is 25.00 mL. Calculate the number of individual lithium ions (Li+) in the final 25.00-mL solution. Note that lithium phosphate is a strong electrolyte that completely dissociates in water (note that (aq) means the species is a solute in an aqueous solution): Li3PO4 (aq) 3 Li+ (aq) + PO43– (aq) Report your answer to two significant figures. Use scientific notation. Example: 1.0*10^23 (this notation means 1.0 1023)Done < HIIL Attempts done: 0/2 O Zn²+ O Zn O Zn²- O Zn+ What is the most common oxidation state for zinc? > AA A practice.flatworld kn Read the related chapter ? View available hints Report an error
- Give only typed answer Give all subparts answers otherwise leave itA 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.A 0.6599-g sample of impure magnesite, MgCO3 (MW = 84 g/mole), was decomposed with HCl; the liberated CO2 (MW = 44 g/mole) was collected on absorbent and found to weigh 0.1673-g. Calculate the percentage of magnesium (MW = 24 g/mole) in the sample. MgCO3 (s) + 2 HCl (aq) →MgCl2 (aq) + CO2 (g) + H2O(l) Weight of pure magnesium in the sample is a. 0.1825 g b. 0.0913 g c. 0.3194 g d. 0.0456 g Percentage of magnesium carbonate in the sample is a. 24.20% b. 27.66% c. 48.40% d. 96.80%
- matter eith constant composition in its structure is classified as?For the gravimetric determination of manganese, 1.8762 g of sample containing Mn was dissolved in acid solution and made up to 100 mL in a calibrated volumetric flask. A 25.00 mL aliquot of this solution was transferred to a beaker. The solution was heated to boiling and chemical substances required were added till precipitating MnNH4PO4. After filtering, rinsing, and igniting, 0.5365 g of Mn2P2O7 was obtained. Calculate the % manganese in the sample (Mn: 55, P: 31, O: 16 g/mol).Why is the highest oxidation state observed for CrCl4 onlythe +4 oxidation state, in contrast to the +6 stateobserved in CrF6?