IIIO Chemical ReactionsDetermining the volume of base needed to titrate a given mass of acid1/5A chemistry student weighs out 0.0885 g of citric acid (H3CH,O), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilledwater. He plans to titrate the acid with 0.1700 M NaOH solution.Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits.mLXG

To calculate the volume of NaOH solution needed to reach the equivalence point, we first need to…

Answered: III O Chemical Reactions Determining…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Titration is a common laboratory method of quantitative chemical analysis. In an acid- base titration, 65.0 mL of Ba(OH)2 was neutralized by 58.0 mL of 0.350 mol/L HCl. Calculate the concentration of Ba(OH)
A 50.25 g sample of Ca(OH)2 is dissolved in some water. Determine how many mL of 0.525 M HClO4 will be required to titrate the Ca(OH)2
A strong acid-strong base titration was performed as follows: 10.00 mL of 0.10M HCl were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to HCl. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.20 ml of 0.100M NaOH? Select one:a. 9.80b. 10.26c. 9.90d. 11.08
In the lab, you are asked to titrate a 50.0 mL solution of hydrobromic acid, HBr, or unknown concentration using 0.125 M calcium hydroxide, Ca(OH)2. If the equivalence point is reached after adding 37.2 mL of calcium hydroxide, what is the concentration of the original hydrobromic acid solution? Answer Should Be: 0.107 M
CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) 25.00 mL of a solution of phosphoric acid, H3PO4, was titrated with 0.500 M NaOH. a) Write the balanced chemical equation for this reaction.b) If 35.92 mL of NaOH solution were needed to reach the end point in the titration, what is the molarity of the H3PO4 solution?c) How many grams of H3PO4 were present?
An analytical chemist weighs out 0.026 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 3.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol
One of the main acidic components of acid rain is sulfuric acid, H2 SO4. Assuming sulfuric acid is the only acid in the acid rain, what volume (in mL) of 0.000855 M KOH would be required to titrate a 50.00 mL sample of acid rain with an H2 SO4 concentration of 1.310 × 10-4 M? Volume mL
The molarity of an aqueous solution of sodium hydroxide, NaOH, is determined by titration against a 0.190 M nitric acid, HN3 , solution. HNO3 + NaOH→ NANO3 + H2o If 28.0 mL of the base are required to neutralize 22.4 mL of nitric acid, what is the molarity of the sodium hydroxide solution? Molarity = M Submit Answer Retry Entire Group 4 more group attempts remaining
An analytical chemist weighs out 0.185 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.2000 M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 9.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol
You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?
Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
A chemistry student weighs out 0.379 g of citric acid (H,C,H,O,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits.

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