A 0.1510 g KHP (Mw = 204.22 g/mol) sample required a volume of 57.04 mL of NaOH solution to reach a phenolphthalein end point. Calculate the molarity of NaOH titrant. (A) 0.01012 M B 0.02593 M 0.01296 M 0.006481 M
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- 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.Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be the normality of the iodine in order that each ml of titrant represents 1/2% As2O3 in the sample (Answer: 0.0809 N show full solution please)n a titration of 25.00 mL of X solution, 32.55 mL of 0.6896 M Y solution are required to reach the end-point. What is the concentration of the 25.00 mL of X?
- 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the presence of phenolphthalein indicator, the acid consumption is 15 mL. Then, the titration is continued by adding bromocresol green indicator, and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; NazCO3: 106 g / mol)Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of a 0.5972 g sample of powdered limestone was measured by suspending the powder in water, adding 25.00 mL of 0.508 molar hydrochloric acid, and heating to dissolve the solid and dispel carbon dioxide gas. The excess acid required 36.29 mL of 0.1064 molar sodium hydroxide for complete titration to a phenolphthalein end point. What is the weight percent of calcite in the limestone?A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2(ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 what is the pH at the equivalent point?
- Neutralization Titration In the standardization of HCI solution using 10.00 ml of 0.02 Na,co, according to the equation M of Na,CO, 2 HCI 2NaCl + H₂O+CO, 15.0 ml of HCI is required to reach the end point using Bromocresol green indicator the molarity of HCI (mol/L) would be al 0.032 b) 0.027 20.013 d) 0.008 e) 0.064Need solution urgently 125mL of an alkaline water sample containing 128 ppm carbonate and 40ppm hydroxide in terms of CaCO_(3) equivalent its titrated against 0.20NHCl using methyl orange as the indicator.What will be the titre value (in ml unit)?Directions: Solve the problem with a complete step-by-step solution. 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? The chemical reaction is 2MnO4- + 5C2O42- + 16H+ + ----> 2Mn2+ + 10CO2 + 8H2O
- d) please see attached question concentration KOH=20.8325mL pH solution=2.9 beginning of the titration, Vbase = 0.00 mLCalculate the grams of Acetic Acid ( M. W. 60.05g/ mole) in a unknown sample. A sample of Acetic Acid was titrated to the end point using 23.76M NaOH solution. The initial buret reading was 0.6559mL and the final reading was 0.02435mL.A 250.0-mg sample of an organic weak acid is dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight.