Q3: In a titration of sulfuric acid against sodium hydroxide, 32.20mL of 0.250MNAOH is required to neutralize 26.60mL of H2SO4 . Calculate the molarity of the sulfuric acid using stoichiometry solutions method and give the type of this reaction . NaOH+H,SO, Na,SO,+H,O
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- A 50.00 mL sample of a locally made white wine required 34.50 mL of 0.0450 M NaOH to reach the end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6)3.) In the assay of NaHCO3, 3.0g of the solid is dissolved in 25mL water. What is the normality? How many mL of 1N H2SO4 will be required to neutralize this solution? From this volume of acid, compute the percent purity of NaHCO3.Calculate the volume in milliliters of 0.362 M KOH necessary to titrate 28.38 mL of 0.279 M diprotic sulfuric acid, H2SO4, to a phenolphthalein end-point. Report the answer to a precision of 2 decimal places.
- To analyze an aspirin sample, 0.3470 g of crushed tablets are weighed and treated with 50.00 mL 0.1155 M sodium hydroxide, boiling for 10 minutes. Under these conditions the acid acetylsalicylic (MW, 180) reacts according to: CH3COO-C6H4-COOH + 2 OH- → OH-C6H4-COO- + CH3COO- The excess NaOH is then titrated with 11.5 mL of 0.2100 M HCl. What is the purity of said show ?.Calculate the volume of a 1.420MNaOH solution required to titrate 23.50mL of a 1.500MH3PO4 solution. Round your answer to 4 significant digits.Consider the reaction of 66.5 mL of 0.310 M NaC₇H₅O₂ with 50.0 mL of 0.245 M HBr. (Ka of HC₇H₅O₂ = 6.3 x 10⁻⁵) a)Write the net ionic equation for the reaction that takes place. (In terms of C, H2O, H3O+, O, H, H+, OH-) b) How many moles of C7H5O2- would be present before the reaction takes place? c) How many moles of H+ would be present before the reaction takes place? d)What species would be left in the beaker after the reaction goes to completion? e) How many moles of C7H5O2- would be left in the beaker after the reaction goes to completion? f) How many moles of HC7H5O2 would have been produced after the reaction goes to completion? g) What would be the pH of this soultion after the reaction goes to completion?
- What volume of 2.25-M H2SO4 should be diluted with water to form a 1.25 liters of 1.5 molar of the same acid solution?What volume in millimeters of 0.0200M Ca(OH)2 is required neutralize 75.0ml of 0.0300 m HCl ?Lemon juice contains citric acid which is tribasic(H3Y). 25cm^3 of lemon juice was diluted to 250cm^3. 25cm^3 of the solution was neutralized by 15cm^3 of 0.1M sodium hydroxide. a) Calculate; i) concentration of the diluted solution of lemon juice ii) concentration of the original lemon juice. iii) percentage by mass of citric acid in lemon juice.
- A HNO3 solution has a sp.gr. of 1.42 and is 70.0 % (w/w) HNO3 . How many ml of this solution is needed to prepare 250. mL of 1.00 M HNO3?During the titration of an HClO4solution with 0.10320M NaOH, a CHEM 3A student,Juan becamedistracted and overshot the endpoint. A fellow student Pedrosuggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000mL, the volume of NaOH added was 28.060mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH andcalculate the molar concentration of the original HClO4solution.What is the pH of the solution after mixing 0.171 g of Mg(OH)2 (MW=58.321 g/mol) with 68.9 mL of 0.0569 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.