An excess of potassium iodide is added to a solution of potassium dichromate, and the liberated iodine is titrated with 48.80ml of 0.1000M sodium thiosulfate solution. How many grams of K2Cr2O7 did the dichromate solution contain?

Q: When 10.00 mL of a 0.09804 M solution of potassium hydrogen phthalate (KHP) is titrated with aqueous…

A: Volume of KHP = 10.00 mL Molarity of KHP = 0.09804 M Moles of KHP = 0.09804 × 10/1000 =      Moles…

Q: A student in conducting molecular weight determination of an uninown diprotic acid. He first…

A: KHP dissociates completely to form K+ and HP-. HP- then acts as weak acid. KHP and NaOH are…

Q: The molarity of an EDTA solution is 0.0114 M.  A 25.0 mL sample of water with unknown Ca+2…

A: Molarity is number of moles of solute present in 1 liter of solution. Mass of substance = molar mass…

Q: The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret…

A: Given, The Volume of HCl = 10.0 mL. The molarity of HCl = x. The Volume of NaOH = 31.1 mL. The…

Q: 6.A 16.6 mL aliquot of 0.2 M aqueous hydrochloric acid is titrated with 0.6 M NaOH (ac). What volume…

A: Given that: volume of HCl = 16.6 mL molarity of HCl = 0.2 M molarity of NaOH = 0.6 M  To find, the…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Calculation of no. of mol of HNO3 at the end point: n=Molarity×Volume=0.340 mol/L×16.5 ×10-3…

Q: Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If…

A:

Q: A 25.00 mL sample of a solution of citric acid, H3C6H5O7, required 22.40mL of 0.1230M NaOH to…

A:

Q: A 20.00 ml sample of 0.520 M oxalic acid is titrated with 26.50 ml of an unknown KmnO4 solution. a).…

A: a.The number of moles of oxalic acid present in titration is calculated as,

Q: What volume of 0.130 M  KMnO4 would be required to titrate 0.36 g  of  K2[Cu(C2O4)2]⋅2H2O

A: We should equal equivalent of both KMnO4 and compund ion to get volume of KMnO4 Equivalent =…

Q: During the titration, 25.0 mL of the 0.0233 M saturated calcium hydroxide solution was titrated with…

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Q: A solution of sulfuric acid (25.00 mL) was titrated to the second equivalence point with 36.55mL of…

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Q: For the adjustment of 0.1 M HCl standard solution, 0.1345 g Na2CO3 in primary standard purity was…

A:

Q: A Ba(OH)2 solution is standardized against potassium hydrogen phthalate (KHP). The titration of…

A: Given: Mass of KHP used = 0.5781 g. Volume of Ba(OH)2 required = 30.50 mL = 0.03050 L…

Q: Given the following data during the potentiometric titration of 75.00 mL unknown NaCl solution by…

A: Given Data:

Q: If 0.626 g of an unknown monoprotic acid was used to prepare a 25.00 mL weak acid solution and this…

A:

Q: A solution of malonic acid (H₂CH₂O) with a known concentration of 0.500 M H₂CH₂O is titrated with a…

A: At each equivalence point ,  Volume of malonic acid × strength of the malonic acid = volume of KOH ×…

Q: During the titration of an HClO4 solution with 0.10320 M NaOH, a student, Lovely became distracted…

A: Conc of NaOH =0.10320M Original sample volume= 25mL Volume of NaOH added=28.060ML Extra HCl…

Q: Consider the following acid base titration between H2C3H5O3 (aq) with KOH (aq).    A)Write a…

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Q: how do i calculate the molarity of KMnO4. in the titration the buret was filled with 0.0815 M of…

A: Given: Molar mass of FeCl2 sample = 126.75 g/mol Mass of FeCl2 sample = 2.0178 g 8H+ + 5Fe2+ +…

Q: You have been provided with a 2.13 x 10-2 L  sample of lithium hydroxide (LiOH) of unknown…

A:

Q: Calculate the grams of Acetic Acid ( M. W. 60.05g/ mole) in a unknown sample.  A sample of Acetic…

A: Molarity of a solution is used to express the concentration of the solution. It can be calculated by…

Q: Consider the titration of 40 ml of 0.151 M base, 8, with 0.163 M HO. The analyte, B, has a pke 4824…

A: At the equivalence point: Moles of acid, HCl = Moles of base Molarity × Volume (HCl) = Molarity ×…

Q: D. Acid-Base Titrations A 0.1558 g of primary-standard-grade benzoic acid, CsHsCOOH, was used to…

A: Hello. Since multiple questions have been posted, the first question shall only be solved in this…

Q: A 1.000 liter sample of sea water was evaporated to a small volume and treated with an excess of…

A: One ppm is equivalent to the absolute fractional amount multiplied by one million.

Q: What is the concentration of CN- (M) in the 50.0 mL sample?

A: Given, The 10 mL initial aliquot has been diluted to 25 mL. The final concentration of CN- in this…

Q: 35.0 mL sample of 0.225 M HBr was titration with 42.3 mL of KOH. What is the concentration of the…

A: First we write the balanced equation between HBr and KOH. This is given as; KOH (aq) + HBr (aq) →…

Q: The titration of 80.0 mL of an unknown concentration H 3PO 4 solution requires 126 mL of 0.218 M KOH…

A: Given :-  Molarity of KOH solution = 0.218 M  Volume of KOH solution = 126 mL  Volume of H3PO4…

Q: percentage of NaCN

A:

Q: What volume of 0.370 M  KMnO4 would be required to titrate 0.41 g  of  K2[Cu(C2O4)2]⋅2H2O = ?mL

A: The ionic equation for the reaction is

Q: How many moles of sodium thiosulfate pentahydrate are used in the titration? (use average volume of…

A: Titration (also known as titrimetry and volumetric analysis) is a common laboratory method of…

Q: A solution of oxalic acid dihydrate (H₂C₂O₄･2H₂O) with a known concentration of 0.400 M H₂C₂O₄･2H₂O…

A: At equivalent point mole to stoichiometry is equal of both reactants

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Ca(OH)2 reacts with HNO3. The balanced chemical equation for the reaction is given by:

Q: In one experiment, an 80.0-mL sample of hydrocyanic cid (HCN) was titrated with 20.0 mL of triiodide…

A: H3AsO3 (aq) +  I3- (aq) + H2O (l) → H3AsO4 (aq) + 3I- (aq) + 2H+ (aq)   Calculation for…

Q: Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of…

A:

Q: A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach…

A: To write the balanced chemical reaction.

Q: 25.00 mL of a sample containing Hg2²+ was titrated with 0.05789 M of KIO3, requiring 35.69 mL to…

A: In this question we have to calculate the concentration of Hg22+ in the sample.

Q: Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If…

A: Given information: Volume of NaOH = 19.45 mL Gram of KHP = 0.397 g

Q: Suppose 0.442 grams of a solid monoprotic acid are titrated with 15.54 mL of 0.098 M NaOH.  What is…

A: The balanced equation corresponding to the neutralization reaction between a monoprotic acid (HA)…

Q: it took 32.47 mL of 0.123M NaOH to reach the endpoint when titrating a sample containg 0.2372g of…

A: Since the acid is given as triprotic  hence the moles of NaOH required to reach the endpoint = moles…

Q: Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000552 mol…

A:

Q: Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titrations. If…

A: We have to apply simple mathematics

Q: The tetraethyl lead [Pb(C2H5 )4 ] in a 25.00-mL sample of aviation gasoline was shaken with 15.00mL…

A:

Q: The titration of 0.314 g of potassium hydrogen phthalate (KHP) requires 13.16 mL of a NaOH solution.…

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Q: What are the advantages of potentiometric titrations over conventional titrations?

A: Introduction:  Titration : Titration is a method to determine to determine the concentration of the…

Q: A 500.00 ml sample of HCl of unknown concentration is titrated with 35.23 mL of 0.05212 M Ba(OH)2 to…

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Q: A 25 ml of an HCIO4 solution was titrated with 0.1032 M NaOH solution, 28.06 ml was added in excess,…

A: When the concentration of the hydrogen ion (H+) is increased in an aqueous solution by a substance,…

Q: In an experiment to determine the molar mass of an unknown monoprotic acid, a 8.642x10-2 g sample of…

A: Given unknown acid  is monoprotic and reaction with KOH is as follows  HA + KOH ----> KA + H2O…

Q: Potassium hydrogen phthalate (KHPKHP) is often used as a primary standard in acid–base titrations.…

A: