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Q: The solubility of CaSO 4 in pure water at 0 oC is 1.09 gram(s) per liter. The value of the…
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- Acidimetric titrant can be: H,SO4 solution; KOH solution; H;PO4 solution; CH;COOH solution;2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)To an aqueous solution containing 1.6000 g sample consisting of a mixture of CaBr2•H2O and inert matter, 52.00 mL of 0.200 M AgNO3 is added. The excess Ag+ requires 4.0 mL of 0.1000 M KSCN for the precipitation of AgSCN. What is the percentages of CaBr2 •H2O and of inert matter in the sample? Please provide a complete solution.
- You prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 19.54 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?Titration of 0.1756 g primary standard Na2C2O4 required 32.04 mL of a potassium permanganate solution. Calculate the molar concentration of KMnO4 in this solution.A standardized iodine solution is used to titrate hydrazine sulfate in a sodium bicarbonate- buffered solution. The reactions that occur are I2 + 2e- = 2I N2H4 .H2SO4 → N2 + SO4 2- + 6H+ + 4e- What is the molarity of a solution of hydrazine sulfate when 27.29 mL of 0.100 N iodine is required to titrate 25.00 mL of the hydrazine sulfate to the equivalence point?
- For the titration of an aqueous nitrous acid solution, HNO,(aq), with an aqueous strontium hydroxide solution, Sr(OH)2{aq), what do you expect the pH of the solution to be at the equivalence point? O Basic (pH > 7.00) O Unable to determine the pH of the solution at the equivalence point without additional information O Acidic (pH < 7.00) O Neutral (pH = 7.00)H.W titration an impure mixture containing sodium carbonate and sodium hydroxide, using two indicators. If 1g of the sample needed 30ml of 0.2N HCI solution to reach the neutral point with respect to the p.p indicator. And 13.5ml of the same acid to reach the equivalence point with respect to the M.O. What is the composition of the mixture and what are the percentages of its components?A solution may contain any or all of the following cations: Ag+, Pb2+, Ba2+, Ni2+ in an UNKNOWN mixture. HCl is added to the solution and a precipitate forms. That precipitate is removed and NH3 (aq) is added to the supernatant until the solution is basic, no solid forms. After making the supernatant basic, K2CrO4 is then added and a precipitate forms. What cations (Ag+, Pb2+, Ba2+, Ni2+)are present in this unknown sample (This is chemistry and not a writing question)
- Calculate the pH for a solution that contains 3.0*10-3M CsOH (aq)A titration of 29.2 mL of a solution of the weak base aniline, C@HNH, ( K 4.0 x 10-10), requires 21.61 mL of 0.155 M HCl to reach the equivalence point. CH_NHz(aq) + HyO* (aq) + C,H,NH, (aq)+H,O(l) a What was the concentration of aniline in the original solution? Concentration 0115 ✔ M The equivalence point for a reaction is the point at which one reactant has been completely consumed by addition of another reactant. Thus, [C,HNH] [H₂O+] [OH-]- = 0.155 mol HC1 1.00 L 1 29.2 mL b What are the concentrations of H₂O¹, OH, and C6H5NHs at the equivalence point? M C = 0.115 M x 21.61 ml x M Correct 1 mol C, H, NH, 1 mol HCl Show HintWrite the expression for the solubility product constant for Pb(OH)2.SEE MORE QUESTIONS
