select the correct answer Experiments home Titration homeLog outNext, determine theamount of Fe2+, inMnO4-(aq) + 5Fe2+(aq) + 8H*(aq) → Mn2+(aq) + 5FE3+(aq) + 4H20(1)moles, that reactedAmount of Mno, (mol):3.70 x 10-5 (Mno+)during the titrationexperiment.lonMn04Fe2+Fill in the correctMolar ratio fromnumbers from theequationbalanced equation toAmount of Fe2+ (mol) in25 cm' sample:Actual amount ofsubstance (mol)get the molar ratio ofMnO, and Fe2+ ions.3.70 x 10-53.70 x 10-5Select0.74 x 103.70 x 10-Then using the amountof MnO4", in moles, andMass of Fe+ (g) in 25cm sample:0.74 x 10-4the molar ratio, select1.85 x 10-4the correct value for theamount of Fe?+ ions, inmoles.Mass of Fe+ (g) per irontablet:Compare titrationresults with iron contenton product label:Check

The given reaction, MnO4- (aq) + 5Fe2+(aq) + 8H+(aq) -----------> Mn2+(aq) + 5Fe3+(aq) + 4H2O(l)…

Answered: Next, determine th MnO4-(aq) +…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

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A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?
Given the equation and following values, what is the concentration of the acid? (With solution) (10*Vb)/Ma Where, Vb = final - Va Va = 10+phenolphValues: Initial Volume of Analyte: 10.150 mL Initial Volume of Titrant: 50.000 mL Final Volume of Analyte: 11.620 mL Final Volume of Titrant: 48.530 mL
Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate) 2 Fe is sought(Analyte), 1Fe2O3 is weighed (Precipitate)
common-ion effect: Mg(OH)2 is a sparingly soluble compound, in this case a base, with a solubility product, Ksp of 5.61×10−11 Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.140M NaOH?
Data Table 2: Complexometric Titration of Tap Water photo shows equation to find water hardness 6 ml of water used (5 ml of tap water 1ml of buffer) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 2ml 2ml 2ml Final Syringe Reading (mL) .61ml .69ml .58ml Volume of EDTA Consumed (mL) 139ml 131ml 142ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):
2,5 ml volume has taken from an “hypothetic” solution which includes (3+) Sb and (3+) Fe and at the titration with 0.1004 N KMnO4, the wasted amount has found as 16,4 mL. The other 2,5 mL that has taken, has reduced with Zn after that, this 2,5 mL solution has titrates with the same KMnO4 solution solution and the wasted amount is 26,5mL. With these datas find the %concentrations of the ions at the solution.
A buffer was made by mixing 0.1886 moles of CH3CH2CO2H with 0.1517 moles of KCH3CH2CO2 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2441 M HBr to 50.00 mL of the buffer? Ka(CH3CH2CO2H) = 1.300e-5. Note: only a portion of the original buffer is used in the second part of the problem. Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. Addition of either a strong acid or a strong base will cause a small shift in pH to a lower or higher pH, respectively.Strategy: Determine the moles of HA and A− the buffer prior to addition of either a strong acid or base by multiplying by the molarity and volume (50 mL) → determine mole of strong acidadded to the buffer. Adjust the moles to account for loss of conjugate base and formation of conjugate acid with addition of a strong acid or loss of conjugate acid and formation of conjugate base with addition of a strong base → use Henderson-Hasselbach equation to…
Data Table 1: Complexometric Titration of Hard Water 6ml of water used (5ml of hard water and 1ml of buffer) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 0.55ml .50ml .33ml Volume of EDTA Consumed (mL) 0.45ml .50ml .77ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L): photo shows equation that needs to be used to solve
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Data Table 3: Complexometric Titration of Soft Water 6ml of water used (1ml of buffer and 5ml of soft water) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):
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