A sodium hydroxide solution is to be standardized using KHP (99.5% purity, MW = 204.22). A 1.500-g KHP dissolved in water required 14.84 ml of NaOH solution for the phenolphthalein endpoint. Calculate the molarity of the NaOH solution.
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- A sodium hydroxide solution is to be standardized using KHP (99.5% purity, FW=204.22). A 1.500 g KHP dissolved in water required 14.84 mL of NaOH solution for the phenolphthalein endpoint. Calculate the molarity of the NaOH solution.A 0.1530 g of pure KIO3 was dissolved in 50 mL distilled water. This was then added with KI and 6N H₂SO4. After allowing the said solution to stand in the dark for 3 minutes, this was then titrated to end point with 31.35 mL sodium thiosulfate solution, with starch as the indicator. What is the normality of the sodium thiosulfate solution? Atomic weights: K = 39.1 1= 126.9 O= 16.0A 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%
- Transfer 0.5 mL phenolphthalein to a flask 25 mL KHP. Then transfer 13.2mL NaOH in the KHP that make it be pink. As the picture shows. Now, show a complete calculation for the concentration of the sodium hydroxide solution.Suka-tuba is a vinegar variety derived by fermenting the sap of a coconut tree. You are tasked to analyze its acetic acid Describe the preparation of 5.0 M NaOH stock solution from analytical grade NaOH pellets. Describe the preparation of 0.10 M NaOH solution from the stock solution. How much KHP was used per trial. (purity KHP: 99.0%).Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is a consumption of 8 mL, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) Solubility of benzoic acid at 27 ° C .................................................; b) solubility of benzoic acid at different temperature ................................................; c) second test temperature ....................................................... (M (benzoic acid): 122.12 g / mol) Note: enter only required numerical values and units in the spaces in the question.
- Q1. Dissolved 0.273 grams of pure sodium oxalate (Na2C0.) In distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMnO, solution and has exceeded end point limits by using 1.46 ml of oxalic acid (H , C, 0.) With 0.1024 N. Calculate the normlity of KMnO .. Note that the molecular weight of sodium oxalate (Na, C, 0.) = 134 and its equivalent weight = 67A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate: the molar analytical concentration of K3Fe(CN)6. the weight/volume percentage of K3Fe(CN)6. ppm Fe(CN)6Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is 8 mL consumption, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) What is the solubility of benzoic acid at 27 ° C? b) What is the solubility of benzoic acid at different temperatures? c) What is the second test temperature? (M (benzoic acid): 122.12 g / mol)
- To determine the Kgp of barium oxalate at 12°C, a 100.0 mL saturated solution was prepared by adding the solid in distilled water maintained at 12°C until it no longer dissolves. The solution was filtered and from this, a 10.0 mL aliquot of the filtrate was drawn. It was found out that 10.70 mL of 5.60 x 104 M HCI was used to reach the endpoint. Given that two moles of HCl react for every mole of dissolved oxalate during the titration, determine the amount of dissolved oxalate in the titration flask (in mol/L). Do not include the unit in your answer below. For those who will be using scientific notation, please follow the format below: Example: 0.00487 -> 4.87E-3 58000 -> 5.8E+4Step 1 :4.9668 g of Na2S03 was dissolved in 30ml distilled water by heating. Step 2 : Then 6.0895g of CuCl,. H,0 was dissolved in 20ml distilled water by stirring with a glass rod. The colour observed here was a deep blue/green Step 3 : The solution from step 1 was added to step 2 solution. Colour turned Light green. Step 4 : 20ml 0.001M H2SO4 was then added to the solution in Step 3 Step 5 : The solution was then funnelled using a buchner funnel, then washed three times with H,SO4 and washed three times with ethanol. The end product was solid white crystals, which weighed 2.4972 grams. What is the yield of the end product? Show all calculationsthe solubility of Ba(IO3)2 in a solution prepared by mixing 300 mL of 0.010 M Ba(NO3)2 with 200 mL of 0.10 M NaIO3 .(K.S.P=1.57X 10-9) is