In a titration experiment using a buret, would you expect to use much less than  a 10 ml volume in each titration

During a certain titration, it took 62.2 mL of 0.626 M strontium hydroxide to exactly neutralize 38.16 mL of perchloric acid. Determine the molarity of the acid. need reaction and mole ratio, use significant figures.

A 22.47 mL sample of dilute HBr requires 31.92 mL of 0.117 M KOH for neutralization.  Determine the molar concentration of HBr in the sample

QUESTION 5 Consider the titration of 17.7 mL of 0.211 M HNO3 with 0.130 M NaOH solution. What volume (in L) of NaOH is required to reach the equivalence point in the titration? Give your answer in numerical form (NOT exponential notation) using the correct number of significant figures. Lavide jon.

2. Why is it necessary to rinse the burette with a few mililitres of the sodium hydroxide solution used in the titration before filling it with this solution? It is necessary to rinse the burette with a few militres of the sodium hydroxide solution used in the titration before filling it with this solution becuase any tiny amounts of liquid remaining are the same as the solution used to fill the burette, so they will not change the concentration of the solution in any way. Moreover this process helps to prevent contamination from the remaining traces of water. 4. When using phenolpthalein indicator in a titration, why is it necessary to have the sodium hydroxide solution in the burette, rather than in the Erlenmeyer flask? When using phenolpthalein indicator in a titration, It is necessary to have the sodium hydroxide solution in the burette, rather than in the erlenmeyer flask becuase it is easy to observe the color change from colorless to pink. On the other hand, if HCI is taken in…

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The titration demonstrated used 21.5 mL of sodium hydroxide to neutralize 25.0 mL of 1.013 M hydrochloric acid. Determine the Molarity of the sodium hydroxide solution.

Answer both questions regarding Acids and Bases. After adding 50 mL of NaOH solution, the sample in the flask still had not turned pink. What error did the student make? and then, compare your percentage of HCI to the manufacturer’s percentage for the toilet bowl cleaner. We’re your results close? What might account for any differences? (Use the second photo for reference)

If 17.1 mL of 0 M NaOH are used, how many moles are in this sample? Suppose 0.371 grams of a solid monoprotic acid are titrated with 16.45 mL of 0.117 M NaOH.  What is the molar mass of the solid acid?

A student performed a titration on a commercial acid certified to be 0.500 M.   Using her data from the titration, the student determined her sample to be 0.487 M.   Assuming the certified value was the true value, what was the percent error of her measurement?