(=2 7. A solution of potassium permanganate was used to titrate a 15.00 mL aliquot of 0.1942 M H₂O2, and the endpoint was determined to be at 42.37 mL. What is the molarity of the potassium permanganate solution?
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- Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of commercial bleaching solution titrated ?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Moles of OCl– in the diluted bleach titrated. ?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Mass of NaOCl in the diluted bleach titrated. ?
- Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of NaOCl in commercial bleach titrated. ?KHP (aq)+NaOH (aq)-->NaKHP (aq)+H2O(l) Trial Vi (mL) Vf (mL) 1 36.19 48.56 2 3 A student masses out 1.096 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NaOH, as shown in the equation above. Calculate the molarity of the NaOH solution.o/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remaining
- 0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M'pure water, 2 M H2SO4 added, heating process and 8.4 mL titrant as a result of titration it's spin out. Calculate the actual concentration of potassium permanganate accordinglyA 0.1036-g sample containing only BaCl2 and NaCl is dissolved in 50 mL of distilled water. Titrating with 0.07916 M AgNO3 requires 19.46 mL to reach the Fajans endpoint. Report the % (w/w) BaCl2 in the sample. [Ans. 29.86 % (w /w)]UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
- A solution of HCl was titrated against sodium carbonate. What is the normality of acid for Trial 3 in the given data? T1 T2 0.3562 0.3479 0.3042 Weight (g) Initial V (mL) 0.80 1.60 0.40 Final V (mL) 35.20 36.70 39.80 Vol HCI used (ml) 35.10 39.40 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)A 22.41 mL of NaOH solution is required to reach the phenolphthalein endpoint in the standardization with 0.276 g of solid, monoprotic primary standard acid (MW 128.33) in a 25.00 mL solution. 12.34 mLof the same NaOH solution was added to titrate 5 mL of vinegar solution to the endpoint. Calculate the mass of acetic acid in this vinegar solution (d = 1.005 g/mL).Aspirin powder = 0.8110g MW of Aspirin = 180g.mol-1 Volume of 0.5N HCl consumed in back titration = 23.50mL Volume of 0.5N HCl consumed in blank titration = 44.50mL Percent purity (USP/NF) = Aspirin tablets contain NLT 90.0% and NMT 110.0% of the labeled amount of aspirin (C9H8O4) What is the calculated weight (in grams) of pure aspirin?..