Tartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of wine. Jose was tasked to find out the acid content in a 100.0 mL wine sample by titrating it with a standardized solution of NaOH. He was able to establish the working concentration of the NaOH solution by using 35.21 mL of it to titrate a primary standard of KHP that weighed 3.001 g. The grams and %w/w of Tartaric acid present in the 100.0 mL wine sample were then determined by titrating a 25.00 mL aliquot using 43.56 mL of the standardized NaOH solution.   H2C4H4O6 (aq) + 2NaOH (aq) ↔  Na2C4H4O6 (aq) + 2H2O (l)   Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol

25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction:                                K2S(aq)  + 2HNO3(aq)   →  2KNO3(aq)  + H2S(g) The concentration of sulphide ion in the final solution is

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 316.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 93.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.

0.3456 g of a solid acid is dissolved in 50 mL of water in a flask  and a few drops of phenolphthalein are added to the solution.  A buret containing 0.2545 M NaOH is prepared with an initial volume of 10.50 mL.  The acid is accidentally titrated with the base beyond the end point, so 1.52 mL of 0.187 M HCl are added to the flask. The titration with the base is continued to a final volume reading of  40.55 mL.  Calculate the molar mass of the solid acid.

6 a b U d [Tutorial: Titration stoichiometry] This question will walk you through the steps of calculating the volume of titrant required to reach the endpoint based on the volume and concentration of analyte. Consider the standardization of NaOH by titration with C,H,O, according to the following chemical reaction: 3 NaOH(aq) + C,H,O,(aq) = Na,C,H,O,(aq) + 3 H₂O(l) Step 1: Evaluate the question. How many moles of aqueous sodium hydroxide (NaOH) will react to completely neutralize one mole of aqueous citric acid (C,H,O,)? Which equation will be most helpful for solving this problem? Calculate the volume in mL of a 0.200 M NaOH solution needed to neutralize 345 mL of 0.033 MC,H,O, standard solution. Based on the fact that NaOH is a strong base and C,H,O, is a weak acid, how would you describe the pH of the solution at the endpoint, where moles of base = 3 times the moles of acid?

Walter White requires a sulfuric acid (Strong acid) solution to use in a very important synthetic reaction.  He finds a bottle labeled H2SO4, but by some strange turn of events, he cannot remember the concentration.  He decides to perform a titration to determine the concentration of the H2SO4.  He pours 22.20 mL of his unknown sulfuric acid solution into a flask and finds that it requires 29.50 mL of 0.57 M KOH (strong base) to reach the endpoint.  What is the concentration of Walter White's sulfuric acid solution? (Enter your numeric answer only, do not use scientific notation, enter 2 decimal places with your answer) For reference: KOH = 56.106g/mol H2SO4= 98.079g/mol Avagadro's number 6.022x1023

A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 79. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 23.0 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 17. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 16.4 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. Submit Ass Continue O 2021 McGraw Hill LLC. Al Rights Reserved. Terms of Use I Privacy Center LL

A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 150. mg of oxalic acid (H₂C₂O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 77.1 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits. x10 M X 5 ?

A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M NaOH to reach the phenolphthalein endpoint. Which is the correct equation between the analyte and titrant reaction?       CH3COOH + NaOH → NaCH3COO + H2O     2CH3COOH + NaOH → NaCH3COO + H2O     C20H14O4 + NaOH → NaC20H14O4  + H2O     CH3COOH + 2NaOH → NaCH3COO + H2O