Determination of sodium carbonate by acidimetric titration involves: Direct titration by acid solution with usage as indicator either methyl orange or phenolphthalein; heating of analyte till 70° C; Direct titration by acid solution with sequential usage of 2 indicators: methyl orange and phenolphthalein; Back titration by acid solution with usage as indicator phenolphthalein;
Q: Which of the following statements is important when assessing a gravimetric analysis? the desired…
A: Precipitation of gravimetric method : The analyte is separated from a solution of the sample as a…
Q: 1. 3M KOH is added to the precipitate and the tube is heated again. The solution is then centrifuged…
A: Group II cations in systematic analysis are precipitated as sulphides. These sulfides are…
Q: A solution containing a mixture of metal cations was treated with dilute HCl and a precipitate…
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Q: Molarity of Sodium Hydroxide Solution 0.1M Weight of Solid Containing KHP 1.4 g Final Buret Reading…
A: Mole is the amount of the substance that contains the same number of particles or atoms or…
Q: As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content…
A: Given data, Mass of soil sample = 5.045g Volume of solution = 0.500L Mass of precipitate using 125mL…
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Q: Use the following experimental titration data to calculate the concentration of the acid being…
A: The neutralisation reaction taking place can be written as, => HC2H3O2 + NaOH ------->…
Q: When treated with a solution of ammonium sulfate an unknown solution produced heavy white…
A: The above procedure is carried out to identify unknown solutions.
Q: 3. The colour changes corresponding to the pH intervals for the three indicators are given in the…
A: So according to the given data and the indicator we have the following conclusion. :
Q: Calculate the masses of (i) Ca(NO3)2 and, separately, (ii) NaCl to add to a 0.150 mol kg−1 solution…
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Q: 1. Calculate the sodium content, in terms of mEq, of 1 g of ampicillin sodium (C6H18N3NaO4S).
A: Note - Since you have asked multiple questions, we are bound to solve only the first question for…
Q: A student performed a titration to determine the exact concentration of NaOH(aq). The titration was…
A: Average titre value = 25.06 + 25.15 + 25.02 + 25.17 + 25.075 = 25.09
Q: In complexometric titration ‘the reaction with analyte should be rapid and complete’ give reason…
A: Complexometric titrations are those titrations in which chelates or soluble complexes, usually…
Q: Consider the following list of indicators. Indicator pK, Methyl red Chlorophenol red Ethyl orange…
A: When choosing the indicator for the acid base titration choose an indicator whose pH range falls…
Q: Outline the change in composition of a solution of the salt of a triprotic acid as the pH is changed…
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Q: what is the purpose of preparing of a standard sodium hydroxide solution in determination of purity…
A: We prepare a standard sodium hydroxide solution in determination of purity on impure KHP. Because we…
Q: A NAOH solution with an approximate concentration of 0.1 mol / L was produced in the laboratory. In…
A: This is a titration between a strong base and weak acid,phenolphthalein is used as the indicator.…
Q: a. What is the molarity of the titrant? The chemist obtained a 3.150 g sample and dissolved it in…
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Q: Explain the difference between 'stoichiometric (equivalence) point' and 'end point' in the context…
A: Titration is used Redox reaction and Acid-Base reaction. There are 2 important stages of the…
Q: Explain why buffer potential is maximised at the pH that matches the pka of the weak acid of the…
A: Solutions- Buffer solution-A buffer solution (also known as a pH buffer or hydrogen ion buffer) is…
Q: Treatment of ammonia with phenol in the presence of hypochlorite yields indophenol, a blue product…
A: Spectrophotometry is a technique used in quantitative analysis to determine the concentration of the…
Q: As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content…
A: · A 5.095 g soil sample was dissolved to give 0.500 L of solution.· And a 150.0 mL aliquot was…
Q: Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed…
A: Gravimetric factor is expressed as the ratio of the formula weight of the substance sought to the…
Q: Step 1 :4.9668 g of Na2SO3 was dissolved in 30ml distilled water by heating. Step 2 : Then 6.0895g…
A: After seeing the reaction and all the components added in steps we see.
Q: A generic version for Drug X is applying registration to the FDA. For the generic drug to be…
A: The Van Slyke equation for the calculation of buffer capacity can be expressed as:…
Q: How much (in g) of Calcium hydroxide is required to increase the pH of a 100mL solution containing…
A: Buffer solution is a solution of acid and it's conjugate base or salt. This solution has constant pH…
Q: Discuss whether the indicator method applied for determination of alkalinity is satisfactory, is…
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Q: The arsenic in a 1.010 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The…
A: molarity is defined as the moles of solute upon the volume of sample molarity =molesvolume
Q: Calculate the masses of (a) Ca(NO3)2 and, separately, (b) NaCI to add to a 0.150 mol kg-1 solution…
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Q: using phenolphthalein as indicator. The titration was repeated several times and the mean titre was…
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Q: 10p in recent years, technology has developed considerably in analytical devices as in many areas…
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Q: Indicator Measurement Colour of Indicator phenol red pOH = 6.8 Indicator Measurement Colour of…
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Q: Water sample from different river water was subjected to a qualitative alkaline analysis by…
A: To determine the solutes present in the given water samples and the molar concentration of the…
Q: dentify the buffer capacity of the solution by titration using 0.250 M NaOH. Calculate the buffer…
A: Buffer is a solution that resists the change in pH when one mol of acid or base is added to it. It…
Q: How do you choose the most suitable precipitate for gravimetric purposes if given many choices?
A: A precipitate is formed when an insoluble compound is dissolved in a solution when a precipitating…
Q: titration an impure mixture containing sodium carbonate and sodium hydroxide, using two indicators.…
A: An impure mixture containing sodium carbonate and sodium hydroxide will titrate together using…
Q: For titration for determination of Chloride, 0.05 AgNO3 and NaCl with a 5% (w/v) K2CrO4 indicator,…
A: In the determination of chloride ion concentration by Mohr's method, NaCl is used as the primary…
Q: The concentration of Cl– in a 100.0-mL sample of water drawn from a fresh water acquifer suffering…
A: Given data, Volume of sample = 100mL = 0.1L Molarity of Hg(NO3)2 = 0.0516 M Volume of Hg(NO3)2 =…
Q: State the limits to the generality of the expression for estimating the pH of an amphiprotic salt…
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Q: Chitinase is a protein that breaks down chitin, a primary component of the cell wall in fungi,…
A: Given: Chitinase is a type of protein that breaks down the primary component of cell wall in fungi…
Q: A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00…
A: •Standard solution which contain known concentration of any substance. •These standard solutions…
Q: You are preparing a 100.0 mL standard solution needed for titration analysis. The NaOH (40 g/mol)…
A: ff
Q: When treated with a solution of ammonium sulfate an unknown solution produced heavy white…
A: The ions present in the unknown solution has to be given,
Q: 00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of…
A: Given: Volume of diprotic acid = 10.mL Concentration of Diprotic acid = 0.1431 M To Calculate: The…
Q: a mixture of compounds was dissolved in organic solvent and extracted with NaOh. The NaOH extract…
A: Phenols and carboxylic acid react with NaOH forms corresponding salts. These salts are soluble in…
Q: The acid-base indicator "Thymol Blue" has two transition ranges as listed below (with the…
A: The pKa values of the forms of thymol blue can be calculated as: pKa=-log Ka
Q: Treatment of ammonia with phenol in the presence of hypochlorite yields indophenol, a blue product…
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Q: Mr. Clean recently bought a laboratory-grade sodium carbonate from a chemical company known as Brand…
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- A substance contains 0.5 g of magnesium hydroxide as the only basic ingredient . The sunstamce is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion substaces dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-3A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedAn alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C, treated with 2 drops of phenolphthalein indicator and titrated with 1.058 N H2SO4 requiring 6.8 mL to render the solution colorless. Upon adding 2 drops of methyl orange and continuing the titration 16.5 mL more of the acid was needed to complete analysis. What is the quantitative composition of the sample?
- The active ingredient in a certain toilet cleaner that claims to 'remove lime scale and rust' is hydrochloric acid of approximate concentration 10.9 mol/L. To analyze this toilet cleaner, a quality control chemist first delivered a 10-mL aliquot of the toilet cleaner into a 250-mL volumetric flask, then made up the diluted solution. She then titrated a 25 mL aliquot of this diluted solution against standard sodium hydroxide solution of concentration 0.46 mol/L. The expected titre (or volume of the titrant in mL) would be approximately:Water sample from different river water was subjected to a qualitative alkaline analysis by titrating against 0.1250 MHC1 and using phenolphthalein and bromocresol green end point. The table below shows the volumes of acid needed to titrate 25.00-mL portions of each sample and their corresponding end point, separately. Use this information to deduce the composition of the solutions. Calculate the molar concentration of each solute. Volume (mL) Phenolphthalein end Bromocresol green Solute identity concentration end point Volume (mL) Molar Sample point 22.40 of solute/s 1 22.41 2 0.00 33.40 3 15.67 42.13 4 29.64 36.42A NazCO3 standard solution is prepared by transferring 2.4817 grams of primary standard-grade sodium carbonate to a 250.0 mL volumetric flask, dissolving the sample in -100 ml of distilled deionized water, and diluted to the mark. A 25.00 mL aliquot is taken and titrated with 42.65 mL of HCI solution to the bromocresol green endpoint. Calculate the concentration of the HCI solution. (A 0.1598 M B 0.1098 M c) 0.3196 M (D) 0.05490 M
- 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 Volume of bleach titrated. 1ml Mass of NaOCl in commercial 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. ?Condition of permanganatometric titration of sodium oxalate includes: pH = 1 and heating of analyte solution till 70° C; pH : = 7 and heating of analyte solution till 70° C; pH = 10 and heating of analyte solution till 70° C; = 1 under room temperature; pHTo determine the concentration of glucose in the packaged juice industry, 50 mL of sample is analyzed. Analysis of it (and other reducing sugars) was carried out there using triiodide back titration. An excess volume of 75.00 mL of 0.338 M triiodide standard solution in alkaline medium was added to the glucose solution. The resulting solution was acidified and the excess triiodide was titrated with 18.37 mL of standard 0.526 M thiosulfate solution. Calculate is the concentration in ppm in the sample. In alkaline medium: Glucose (C6H12O6) / Gluconate (C6H11O7-), Triiodide (I3- ) / Iodide (I-) In acid medium: Thiosulfate (S2O32-) / Tetrathionate (S4O62-), Triiodide (I3- ) / Iodide (I-)