A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain

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?

Calculate the molar mass of the unknown acid from the information below.

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

An analytical chemist weighs out 0.318 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 82.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol x10 x 3

An analytical chemist weighs out 0.203 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 18.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol Explanation Check 0.9 X 4 S MacBook Air © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center I

Consider the titration of 25.00 mL of Sprite with 0.050 M NaOH. Using the following data, determine the citric acid concentration in Sprite (g/L). Take the molar mass of citric acid to be 192.124 g/mol. Give your answer to one decimal place. initial volume (mL) final volume (mL) Buret reading (mL) 1.75 14.32

what is the volume of a NaOH solution added during a titration experiment is the initial buret reading was 12.50 mL and the final buret reading was 37.25 mL?

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1886 M0.1886 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.42 mL12.42 mL of the standard solution. What is the concentration of the original sulfuric acid solution?

An analytical chemist weighs out 0.050 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 9.6 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol