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- Distinguish between the terms slightly soluble and weak. electrolyte.Chemistry A 2.139 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.57 mL of a 0.752 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3: ? WT% KHCO3: ? WT%.4pts) 2.80g of a mixture of Barium Nitrate, Ba(NO3)2 (MM = 261.35 g/mol) and Potassium Bromide, KBr (MM-119.01 g/mol) was dissolved in 200 mL of hot H₂0. Enough Ammonium Phosphate, (NH4)3PO4 (MM = 149.12 g/mol), was added to the solution to precipitate ALL the Barium as Barium Phosphate, Ba3(PO4)2 (s) (MM = 601.93 g/mol). The precipitate was filtered, dried, and weighed to a constant mass of 1.83 g. Determine the percentage by mass of Potassium Bromide, KBr in the original mixture.
- 1 gram of AgCl (s) is added to flask containing 98.741mL of an unknown NaCl solution. The concentration of Ag + after being added is 3.28487x10 -10 and the final mass of AgCl (s) is 1 gram. Determine the molarity of the unknown NaCl solution. Then determine the mass of NaCl dissovled in the unknown NaCl solution.A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.A 2.190 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.74 mL of a 0.778 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3: ? wt% KHCO3: ? wt%
- A 0.1824-g sample that contains both NaCl (MW= 58.442) and NaBr (MW= 102.89) is titrated with 0.1052 M AgNO, requiring 26.48 mL. Calculate the percentages of NaCl and NaBr in the sample. (Answer: 75.13% NaCI, 24.87% NaBr)A 2.187 g sample of a solid mixture containing only potassium carbonate (MM = 138.2058 g/mol) and potassium bicarbonate ( MM 100.1154 g/mol) is dissolved in distilled water. A volume of 33.47 mL of a 0.749 M HCI standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K₂CO₂: KHCO,: wt% wt%1. A sample of pure sodium oxalate, Na2C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C , requiring 45.12 mL of a KMNO4 solution. The end point is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C20,2 + + 2MN2+ 2 Mn04 + 10H* → 10CO2 + 8H20
- Solution X 100 mL of 0.10 M NaOH(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Y 100 mL of 0.10 M NaBr(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Z 100 mL of 0.10 M HC,H,O,(aq) is mixed with 100 mL of 0.10 M NaC,H3O,(aq) 6. A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below. Species Ka HBr(aq) >>I (very large) HC,H;O,(aq) 1.8 x 10-5 a. Using the information above, write the letters of the solutions in the boxes below to rank the solutions in order of increasing pH. Explain your reasoning for the ranking Lowest pH Highest pH b. Does the pH of solution Y increase, decrease, or remain the same when 100 mL of water is added? Justify your answer. c. The student adds 0.0010 mol of NaOH(s) to solution Y, and adds 0.0010 mol of NaOH(s) to solution Z. Assume that the volume of each solution does not change when the NaOH(s) is added. The pH of solution Y changes…A 0.411 g sample of potassium hydrogen phthalate, KHC8H4O4 (molar mass = 204.22g/mol), is dissolved with 50.0 mL of deionized water in a 125mL Erlenmeyer flask. The sample is titrated to the phenolphthalein endpoint with 15.17 mL of a sodium hydroxide solution. What is the molar concentration of the NaOH solution? Express the molar concentration of NaOH to the correct number of significant figures.1. Determine the mass of CaCl2·2H2O (MW 147.02 g/mole) to weigh out using a four- place analytical balance to prepare 100 mL of a 0.1005 M solution of Ca2+. 2. Determine the mass of KCI to weigh out using a four-place analytical balance to prepare 100 mL of a 1 M solution of KCI (MW 74.5513 g/mole). 3. Record the solubility of calcium carbonate in water (mg/L) in your notebook. 4. Calculate the amount of calcium carbonate (mg) not in solution if a tablet is dissolved in 250 mL of water and the tablet's label claim is 600 mg calcium / tablet.