Question

A student followed the procedure in Part I to determine the mass of an unknown acid...

A student followed the procedure in Part I to determine the mass of an unknown acid that would require 30.00 mL of 0.123 M sodium hydroxide. The student found that 8.761 mL sodium hydroxide solution was needed to titrate a 0.0526 g sample of acid to the equivalence point. Calculate the mass (in grams) of unknown required for a 30.00 mL titration.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A student performs a titration of a solution of unknown concentration of propanoic acid (Ka =...
A student performs a titration of a solution of unknown concentration of propanoic acid (Ka = 1.3 x 10-5) using 0.165 M sodium hydroxide solution. If 30.8 mL of the sodium hydroxide solution are required to titrate 36 mL of the propanoic acid solution to the equivalence point, what is the pH of the original propanoic acid solution?
In standardizing a potassium hydroxide solution, a student finds that 42.63 mL of the base solution...
In standardizing a potassium hydroxide solution, a student finds that 42.63 mL of the base solution is needed to titrate 0.5245 gram of KHP to a phenolphthalein end point. In another titration, 26.63 mL of this same base solution is needed to titrate 0.2777 grams of an unknown solid monoproctic acid A) determine the molarity B) determine the molar mass of the unknown solid monoproctic acid
A solution of a theoretical triprotic acid was prepared by dissolving 4.037 g of solid in...
A solution of a theoretical triprotic acid was prepared by dissolving 4.037 g of solid in enough DI water to make 500.0 mL of solution.   10.11 mL of a 0.592 M solution was required to titrate 20.00 mL of this acid's solution. Part A What is the concentration of the acid solution? Part B What is the molar mass of the acid? Hint: You need to calculate the total moles in the 500.0 mL solution (the full 500.0 mL was...
in an acid base titration, a sample of unknown concentration phosphoric acid is analyzed by titration...
in an acid base titration, a sample of unknown concentration phosphoric acid is analyzed by titration with a solution of sodium hydroxide solution. In this analysis just enough sodium hydroxide solution of known molar concentration is added to just react with all of the phosphoric acid. When this condition has been met, the endpoint of the titration has been reached. suppose that 26.38 mL of a 0.100 M sodium hydroxide solution is added to a 30.00 mL sample of the...
A. A 11.3 g sample of an aqueous solution of hydrobromic acid contains an unknown amount...
A. A 11.3 g sample of an aqueous solution of hydrobromic acid contains an unknown amount of the acid. If 12.8 mL of 0.122 M barium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass ofhydrobromic acid in the mixture? = % by mass B. A 10.4 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 25.9 mL of 0.403 M barium hydroxide are required to neutralize...
An unknown diprotic acid was fully titrated with 0.1599 M sodium hydroxide solution to determine the...
An unknown diprotic acid was fully titrated with 0.1599 M sodium hydroxide solution to determine the molar mass of the unknown. If it took 34.98 mL of sodium hydroxide solution to fully react with 0.2518 g of unknown acid, determine the molar mass of the acid (in g/mol). Molar mass of diprotic acid: g/mol
In titrating an acid of unknown concentration, a 20.00 mL sample of the acid was titrated...
In titrating an acid of unknown concentration, a 20.00 mL sample of the acid was titrated using standardized sodium hydroxide. The NaOH had a concentration of 0.1105 M. The titration required 35.45 mL of the base to reach the end-point in the titration. a) How many moles of H+ was in the 20.00 mL sample of acid? b) The solution of acid was prepared by adding 9.605 grams of the acid to 1.000 liter of water. What was the molecular...
What is the molarity if a sodium hydroxide solution if 0.555 g KHP is titrated with...
What is the molarity if a sodium hydroxide solution if 0.555 g KHP is titrated with 23.71 mL NaOH?This NaOH solution is then used to titrate with an unknown acid. If 21.77 mL of NaOH is needed to titrate 0.310 g unknown, what is the molar mass of the unknown acid? Please answer the second part of this.
A 0.872 gram sample of an unknown monoprotic acid is dissolved in 50.0 mL of water...
A 0.872 gram sample of an unknown monoprotic acid is dissolved in 50.0 mL of water and titrated with a a 0.424 M aqueous sodium hydroxide solution. It is observed that after 9.40 milliliters of sodium hydroxide have been added, the pH is 3.350 and that an additional 5.50 mL of the sodium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for...
A student followed the procedure of this experiment to determine the percent NaOCl in a commercial...
A student followed the procedure of this experiment to determine the percent NaOCl in a commercial bleaching solution that was found in the basement of an abandoned house. The student diluted 50.00mL of commercial bleaching solution to 250mL in a volumetric flask, and titrated a 20-mL aliquot of the diluted bleaching solution. The titration required 35.46mL of 0.1052M Na2S2O3 solution. A faded price label on the gallon bottle read $0.79. The density of the bleaching solution was 1.10g/mL. Calculate the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT