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- A student was asked to determine the concentration of ammonia, a volatile substance, in a commercially available cloudy ammonia solution used for cleaning. First the student pipetted 25.00 mL of the cloudy ammonia solution into a 250.0 mL conical flask. 50.00 mL of 0.100 mol L-¹ HCl(aq) was immed added to the conical flask which reactedwith the ammonia in solution. The excess (unreacted) HC1 was then titrated with 21.50 mL 0. 050 M Na2CO3 (aq). Calculate the concentration of the ammonia in the cloudy ammonia solution.A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M KOH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data. Answer with correct units and significant figures.A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M KOH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data. Answer with correct units and significant figures. Upload Choose a File Next► « Previous Not saved Submit Quiz
- Phenobarbital was introduced in 1912 for the treatment of epilepsy. It is an anti-convulsant and sedative-hypnotic drug and used to control seizures. The measurement of phenobarbital is by fluorescence method. A 5.00 mL aliquots of an unknown containing phenobarbital were delivered to 50.00 mL volumetric flasks. The following volumes of a standard solution of phenobarbital, 2.00ug/mL, were then introduced to the volumetric flasks before diluting to volume with the corresponding signals on a fluorometer equipment. Find the concentration of phenobarbital in the original unknown sample.A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M ROH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data. O 12.7 mL O 19.8 mL O48.5 mL 39.5 mLplease help me The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
- (a) A student carries out a titration to find the concentration of some sulfuric acid. The student finds that 25.00 cm of 0.0880 mol dm aqueous sodium hydroxide, NaOH, is neutralised by 17.60 cm of dilute sulfuric acid, H2SO4. -3 H2SO4(aq) + 2NaOH(aq) → Na2SO,(aq) + 2H2O(1) (i) Calculate the amount, in moles, of NaOH used. answer = mol (ii) Determine the amount, in moles, of H2SO4 used. answer mol (ii) Calculate the concentration, in mol dm3, of the sulfuric acid. answer = mol dm3 (b) After carrying out the titration in (a), the student left the resulting solution to crystallise. White crystals were formed, with a formula of Na2SO4•x H2O and a molar mass of 322.1 g mol. What term is given to the x H2O' part of the formula? Using the molar mass of the crystals, calculate the value of x. answer =A student determined the chloride content of a commercial salt by using the Mohr method. A 0.7725 -g sample of the salt was dissolved in distilled water and diluted to a final volume of 250. mL. A 25.-mL aliquot of the analyte solution was then titrated against a standard 0.0347 M AgNO3(aq) solution to the chromate end-point. A blank-corrected volume of 25.96 mL was recorded. Calculate the percent chloride in the sample. Provide your answer to two decimal places and without units.A student determined the chloride content of a commercial salt by using the Mohr method. A 0.7725 -g sample of the salt was dissolved in distilled water and diluted to a final volume of 250. mL. A 25.-mL aliquot of the analyte solution was then titrated against a standard 0.0347 M AgNO3(aq) solution to the chromate end-point. A blank-corrected volume of 25.96 mL was recorded. Calculate the percent chloride in the sample.
- Someone is attempting to measure the H3PO4(aq) content of an unknown solution by both titration with NaOH(aq) and calorimetry. The person measures 100 mL of stock NaOH(aq) solution into a buret but forgets to write down its concentration. They then measure out 50.0 mL of unknown H3PO4(aq) solution (which has an indicator) and places this solution in a constant-pressure calorimeter for the titration experiment. The initial temperature of all the solutions is 22.9 Celsius. The student adds 46.84 mL of NaOH(aq) from the buret to the H3PO4(aq) solution in the calorimeter to reach the equivalence point (color change for indicator). The final solution temperature is 33.5 Celsius. Assume density and specific heat of all solutions are the same as that of pure water and that volumes are additive. a) what is the balanced molecular equation for the acid-base reaction that takes place in the calorimeter? b) Calculate delta HRXN (enthralpy) for the above acid-base reaction c) what is the…A 1.407 g sample of canned tuna was analyzed by the Kjeldahl method. The liberated NH3 required 26.45 mL of 0.1180 M HCl. Calculate the percentage nitrogen and protein in the sample. Assume that the protein factor is 6.25, i.e. % protein = % N x 6.25.A volume of 125.0 mL of 0.565 M KOH (aq) is diluted with 425.0 mL of pure water. What is the final concentration (in molarity) of KOH? Report to three significant figures.
