A 25.00-mL of 0.15 M NaCI was titrated with 0.1000-M AgNO3, (Ksp for AgCl = 1.82*10-10). What is the volume (mL) of AGNO3 needed to make pAg = pCI? Select one: a. 37.50 O b. 12.50 O c. 40.00 O d. 25.00
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- A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/molChemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.Approximately 6 mL of conc. perchloric acid ( 72% ) was transferred to a bottle and diluted with about 1 liter of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O (Fwt= 382g/mol) required 27.41 mL of the HClO4 solution to reach the methyl red end point. What is the molar concentration of the HClO4 solution? Na2B4O7.10H2O + HClO4 ------------> NaClO4 H2B4O7.10H2O
- A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.a student was titrating a solutin of acitic acid with a sodium hydroxid solution. determin the ph at the equivilance point. do this by constructing a bca table, constructing and ice table, writing the equlibrium constant expresion and find the ph. the ka for ch3cooh is 1.8e-5. a 50ml solutin of 0.3 m of ch3cooh was titrated with 0.3 m of naoh.A 0.4071-g sample of CaCO3 (MM: 100.09 g/mole) is transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL aliqout of this solution was mixed with 5 mL of a pH 10 NH3-NH4Cl buffer that contains a small amount of Mg2+--EDTA to adjust the pH to 10. After adding calmagite as an indicator, the solution is titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of EDTA in the titrant. 9.543 x 10-3 M 5.748 x 10-3 M 3.266 x 10-4 M 1.018 x 10-4 M
- Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X31ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)
- The titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? Given that the chemical reaction is 2MnO4- + 5C2O42- + 16H+ -----> 2Mn2+ + 10CO2 + 8H2O Provide a detailed solution.A solution of Na3AsO4 is added dropwise to a solution that is 0.0347 M in Cu2+ and 0.000309 M in Ag+.The Ksp of Cu3(AsO4)2 is 7.95e-36.The Ksp of Ag3AsO4 is 1.03e-22.(a) What concentration of AsO43- is necessary to begin precipitation? (Neglect volume changes.)[AsO43-] = __________ M.(b) What is the concentration of AsO43- when the second cation begins to precipitate?[AsO43-] = _______ M.It is desired to determine the concentration of chlorides in a powdered milk following the method of Volhard, for such case 1.5g of milk is weighed, it is heated in a muffle until obtaining ashes, which are treated with acid water with some drops of HNO3, the solution is filtered and the obtained filtrate is collected in an Erlenmeyer and 20 mL of AgNO3 0 is added. 1M excess silver is titrated with 0.05M potassium thiocyanate, if 8 mL of KSCN has been used up at the time of the indicator turn. Calculate the % of chloride in the milk powder.