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 1.00 g sample of limonite iron ore, 2Fe203 · 3H20, is dissolved, reduced to Fe2+ and titrated with 20.00 mL of 0.20 M cerium (IV). Calculate the percentage of 2FE203 · 3H20, (FM: 373.38 g/mol) in the sample. Titration reaction: Fe2+ + Ce*+ → Fe3+ + Ce3+

A dried sample of commercial salt was prepared by a coning and quartering. A 0.911-g sample of the salt was dissolved and diluted to 250.0 mL in a volumetric flask.  Repeat 10.00-mL aliquots of this solution were titrated with a 0.054 M silver nitrate solution, requiring 9.68 mL to reach equivalence. Calculate the %(w/w) NaCl in the original sample.

A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?

Ca(OH)2​(aq)+2HCl(aq)CaCl2​(aq)+H2​O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration.   A. How many moles of base were required to react completely with the acid in this reaction?   _____mol Ca(OH)2      B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HCl

4. If the following values are used... Measure the mass of 0.400 g of cobalt(II) nitrate hexahydrate (Co(NO;)2 -6H2O), and dissolve it in 15.0 mL of distilled or deionized water using a clean beaker. Using a graduated cylinder, measure out 10.0 mL of a prepared 0.10-M sodium phosphate (NazPO4) solution. ... determine which compound, (Na3PO4 or Co(N03)2 ·6H2O) will be the limiting reagent. Then determine the theoretical yield.

A quantitative analysis for ethanol, C2H60, is accomplished by a redox back titration. Ethanol is oxidized to acetic acid, C2H402, using excess dichromate, 3+ Cr207 2-, which is reduced to Cr3*. The excess dichromate is titrated with Fe2*, giving C and Fe+ as products. In a typical analysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mL sample is taken and the ethanol is removed by distillation and collected in 50.00 mL of an 2- acidified solution of 0.0200 M K2Cr207. Titration of the unreacted Cr207 requires 21.48 mL of 0.1014 M Fe2*. Calculate the %w/v ethanol in the brandy. Which is the titrant in this problem? C2H402 Fe2+ C2H60 O Cr207 2-

25.00 mL of a solution containing KIO4 is treated with excess potassium iodide. IO4- + 8H+ + 7I- → 4I2 + 4H2O The resulting solution is titrated with 0.15 M sodium thiosulfate pentahydrate. The average titre was 21.76 mL.  I2 + 2S2O32- → 2I- + S4O62- What mass of KIO4 (in g) was dissolved in water to make the original solution?

w.com/ilrn/takeAssignment/takeCovalentActivity.do?locator3Dassignment-take [References) A solution contains 6.3 x 10-3 M Mg(NO3)2. What is the minimum concentration of KF that would cause precipitation of solid MgF, (Ksp = 6.4 x 10-9)? %3D Concentration of KF M

Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the solubility in mol/L at 20oC and at 60oC? How many milliliters (mL) of 0.045 M Na2S2O3 will be required to titrate a 10.0-mL sample of saturated Ca(IO3)2 solution collected at 20oC and 60oC, respectively?