A titration analysis of a 345.0 mL aqueous HBr solution was performed and the endpoint was reached upon the addition of 191.05 mL of 2.815 M aqueous KOH solution. What is the concentration (in M) of the HBr solution? HBr(aq) + KOH(aq) ——> KBr(aq) + H2O(l)
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- In an analysis of metal carbonate M2CO3∙3H2O, 1.500g of the unknown carbonate was dissolved in enough water to make a 100.0mL solution. 20.00mL of such solution was treated with 10.00mL of 1.000M HCl solution, and the excess acid was titrated with 54.92mL of 0.1138M NaOH solution. The equations are given below: CO32-(aq) + 2 H+(aq) → H2O(l) + CO2(g) H+(aq) + OH-(aq) → H2O(l) a) the moles of NaOH used in the titration is (enter the answer in 4 sig. figs.) Answer mol b) the mole of HCl reacted with the carbonate is (enter the answer in 4 sig. figs.) Answer mol c) the molar mass of M2CO3∙3H2O is (enter the answer in 4 sig. figs.) Answer g/mol d) the identity of metal M is (enter the element symbol) AnswerA carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible.What is the MW of calcium carbonate?102 g/mol98 g/mL100 g/mL100 g/molWhat is the molar concentration of the standardized EDTA solution?0.08m0.8M0.08N0.08MHow many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?0.18250.18521.8251.1852Potassium permanganate solutions may be standardized by titrating against primary standard sodium oxalate: 2MnO4- + 5C2O42- + 16H+ → 2Mn2+ + 10CO2 + 8H2O. What is the molarity of the KMnO4 solution if 43.80 mL of the KMnO4 is required to titrate 0.2168 grams of Na2C2O4?
- For the titration of HOCl in bleach solution by Na2S2O4 the following reactions are used: HOCl-(aq) + H2O(l) + 2I- (aq) → I2(aq) + 2Cl-(aq)+ 2OH-(aq) I2(aq) + 2S2O4-2(aq) → 2I- (aq) + S4O6-2(aq) What is the molar stoichiometric ratio between analyte and titrant ? a. 1 mole analyte : 1 moles titrant b. 1 mole analyte :2 moles titrant c. 2 mole analyte : 1 moles titrant d. 3 mole analyte :2 moles titrantThe hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?0.7050-g of pure KHP (FW = 204.2) was dissolved and titrated with 35.00mL of NaOH solution. The excess NaOH was backtitrated with 5.00mL of HCl solution. In a separate titration it was found that 30.00mL of NaOH will react with 28.00mL of HCl. Find the molarity of NaOH and HCl. Show all the solutions involved and round-off final answers to two decimal places except for Molarity. (Molar concentrations should be in four decimal places)
- Zinc(s) (MW=65.38), with a mass of 0.228 g, was reacted with 20.00 mL of NaClO (MW=74.44) according to the following unbalanced ionic equation. Determine the normality of NaClO. Zn(s) + ClO- → Zn(OH)2 + Cl- (in basic medium)A Medical Technology student was given a capsule of a multivitamins and she was asked to determine the % by mass (w/w) of ascorbic acid present in the capsule. The student analyzed the 2.001 g sample using volumetric titration. The following data was generated in the analysis: KIO3 + 5KI + 6H+ → 3I2 + 6K+ + 3H2O C6H8O6 + I2 → C6H6O6 + 2I- + 2H+ Table 1. Standardization of KIO3 Molarity of Ascorbic Acid Standard Solution 0.03542 M Volume of Ascorbic Acid 25.00 mL Volume of KIO3 8.70 mL Molarity of KIO3 ______________M Table 2. Determination of Ascorbic Acid Concnetration Initial burette reading, KIO3 0.00 mL Final burette reading, KIO3 33.60 mL Volume consumed, KIO3 33.60 mL MM of Ascorbic Acid 176.12 g/mole choices 7.30% 30.1% 33.6% 32.5%A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS
- A 11.00 gram sample of Vodka was analysed for its alcohol content. The sample was placed in a300 mL volumetric flask and made to the mark with distilled water. A 20.0 mL aliquot of the dilutedVodka was taken from the volumetric flask and placed in a conical flask containing some distilled water from a previous washing.The 20.0 mL aliquots were titrated against a 0.1302 M Cr2O72-solution and an average titre of13.25 mL was obtained.The reaction between the alcohol and the dichromate solution is given below2Cr2O72–(aq) + 3CH3CH2OH(aq) + 16H+(aq) 4Cr3+(aq) + 3CH3COOH(aq) + 11H2O(l)a) Calculate the amount in mol of Cr2O72– in the average titre. b) Calculate the percentage, by mass, of ethanol in the vodka.A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?A sample of CaCO3 (molar mass=100.1) weighing 0.4856 g is dissolved in HCl and the solution diluted to 500.0 mL in a volumetric flask. A 25.00-mL aliquot requires 21.37 mL of an EDTA solution for titration. How many grams of Na2H2Y.2H2O (molar mass=372.2) are required to prepare 500.0 mL of this solution.