Question 9 When a sample of the CH2CI2 layer with a volume of 5.17 mL is collected 21.11 mL of a titrant solution of S2032 with a concentration of 0.01421 the endpoint. The reaction has a 2:1 mole ratio of thiosulfate to iodine. I
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- 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?Question 22.c of 30 Submit A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 19.6 mL of HNO3 was required. Given that 0.00666 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction? mol 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. How many moles of HCl was added initially to digest the limestone sample? How many moles of CaCO₃ is present in the limestone sample? What is the purity of the limestone in terms of %w/w CaCO₃?
- Iodometric titration of Vitamin C with sodium thiosulfate How many moles of iodine (I2) react with the thiosulfate? The equation is.. 5.66 x 10-4 M of sodium thiosulfate used in titration 0.62 g in 0.01 M in 250 mL conical flask 0.00075 M of iodine in the conical flask 0.00025 M of potassium iodate 1 iodine mole : 2 sodium thiosulfate mols2.23 gr sample taken from a bleaching powder is dissolved and completed to 250 ml. Taken from here 25One ml of sample is titrated with 33.02 ml of 0.1158 N Na2S2O3 solution after the necessary procedures. Bleachingactive chlorine in powder (OClCalculate the amount and percentage. (OCl: 51.5 g / mol)7. barium hydroxide reacts with acetic acid: a. Write the balanced chemical equation: (PA6 + (po moitopo olussioM 18 1svlia + muiesngom A b. How many mL of 0.1 M Ba(OH)2 will be required to neutralize 20.0 mL of 0.25 M HC2H3O2? Horl noitabixo soitaosy tail noitub 19 j
- Question A 25.0 mL volume of 0.0400 M phosphoric acid (H3PO4, pK1 = 2.15; pK2 = 7.20; pK3 = 12.38) was titrated with 0.0500 M tetramethylammonium hydroxide. The titration reactions between the acid and the strong base are H;PO4 + OH → H,POT +H20 H,PO, +OH" + HPO-+ H20 HPO-+OH" → Po-+H20 What is the pH of the solution after 20 mL of the titrant was added? Answer 4.68A silver nitrate solution contains 7.053 of primary standard AgNO3 in 500.0 mL . What volume of this solution will be needed to react with 0.1905 g of Na2CrO4?1. Calculate the concentrations of Na+ and CO32- after mixing 1.00 L of 0.200 M Na2SO4 with 2.00 L of 0.100 M K2CO3.2. Calculate the number of moles of H2 produced when 0.500 g og Mg(s) and 500. mL of 0.200 M HCl are reacted.3. What is the concentration of all ionic species present when 100. mL of 0.200 M NH4OH and 100. mL of 0.200 M H2SO4 are mixed.4. Determine the mass of CuS formed when 100. mL of 0.100 M H2S and 50.0 mL of 0.150 M Cu(C2H3O2)2 are reacted. What is the concentration of C2H3O2- in the resulting solution?5. 18.0 g of zinc is added to 100. mL of 0.200M HBr.a) Will all of the zinc dissolve?b) What will be the concentration of Br- in the resulting solution(after any reaction takes place)?6. A 1.25 g sample of impure sodium carbonate requires 18.20 mL of 0.480 M HCl to become completely neutralized. What is the percentage of the sodium carbonate in the original sample?7. 35.0 mL of 0.325 M AgNO3 is added to 50.0 mL of 0.125 M MgCl2. Assuming all volumes are additive, what…
- 50.00 mL of a solution containing 0.15 M CH2 (CO2 H)2 and 0.020 M MnSO4 Calculate the mass in g of malonic acid required.A 1.164 g sample of impure Na2CO3 was decomposed by adding 100.00 mL of a 0.2000 M HCl solution. The liberated CO2 was collected and found to have a mass of 0.2817 g. Calculate the % (m/m) Na2CO3Nickel sulfate, NiSO 4 , reacts with sodium phosphate, Na 3 PO 4 , to give a pale yellow-greenprecipitate of nickel phosphate, Ni 3 (PO 4 ) 2 , and a solution of sodium sulfate, Na 2 SO 4.. How manymilliliters of 0.375 M N i SO 4 will react with 45.7 mL of 0.265 M Na 3 PO 4 ? . Show balanced chemicalreaction of the problem.