Question

If 38.17 mL of 0.1072 M NaOH is required to titrate a 15.00 mL sample of...

If 38.17 mL of 0.1072 M NaOH is required to titrate a 15.00 mL sample of sulfuric acid, what is the molarity of the acid?

Homework Answers

Answer #1

The balanced equation is

2NaOH + H2SO4 ----- > Na2SO4 + 2H2O

Number of moles of NaOH = molarity * volume of solution in L

Number of moles of NaOH = 0.1072 * 0.03817 = 0.00409 mole

From the balanced equation we can say that

2 mole of NaOH requires 1 mole of H2SO4 so

0.00409 mole of NaOH will require 0.00205 mole of H2SO4

molarity of H2SO4 = number of moles of H2SO4 / volume of solution in L

molarity of H2SO4 = 0.00205 / 0.015 = 0.137 M

Therefore, the molarity is 0.137 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
If   14.99 mL of NaOH are required to titrate 15.00 mL of a   0.46 M oxalic acid solution,...
If   14.99 mL of NaOH are required to titrate 15.00 mL of a   0.46 M oxalic acid solution, what is the concentration of the NaOH? A solution of a theoretical triprotic acid was prepared by dissolving 4.980 g of solid in enough DI water to make 500.0 mL of solution.   10.10 mL of a 0.448 M solution was required to titrate 20.00 mL of this acid's solution. 1. What is the concentration of the acid solution? 2. What is the molar mass...
What volume of 0.100 M HCl is required to titrate 25.0 mL of 0.050 M NaOH?
What volume of 0.100 M HCl is required to titrate 25.0 mL of 0.050 M NaOH?
A student required 26.42 mL of 0.1013 M NaOH solution to titrate 0.154 grams of a...
A student required 26.42 mL of 0.1013 M NaOH solution to titrate 0.154 grams of a solid triprotic acid to the phenolphthalein end point. Assuming she did her calcilations correctly, what did she report as the molar mass of her acid? (Please show all work as clear as possible) (refer to the balanced molecular equation)
A student required 26.42 mL of 0.1013 M NaOH solution to titrate 0.154 grams of a...
A student required 26.42 mL of 0.1013 M NaOH solution to titrate 0.154 grams of a solid triprotic acid to the phenolphthalein end point. Assuming she did her calcilations correctly, what did she report as the molar mass of her acid Assuming you have the answer to this^ , please answer this Q: The student later realized that she had read her buret incorrectly. The volume of the NaOH solution was actually 23.58 mL that she used. What kind of...
if 14.00 ml of 0.4 M NaOH is used to titrate the acid in an aliquot...
if 14.00 ml of 0.4 M NaOH is used to titrate the acid in an aliquot of acetic acid-butanol mixture, how many moles of acetic acid is present
1) A 21.30 mL volume of 0.0975 M NaOH was used to titrate 25.0 mL of...
1) A 21.30 mL volume of 0.0975 M NaOH was used to titrate 25.0 mL of a weak monoprotic acid solution to the stoichiometric point. Determine the molar concentration of the weak acid solution. 2.08 M 0.114 M 0.0831 M 0.00390 M 2.44 M 2) For a weak acid (CH3COOH) that is titrated with a strong base (NaOH), what species (ions/molecules) are present in the solution at the stoichiometric point? CH3COO- H2O Na+ NaCl HCl
1. 20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. ______ 1 mL...
1. 20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. ______ 1 mL of H2SO4 are needed to reach the end point. 2.  If 35.00 mL of 0.0200 M aqueous HCl is required to titrate 30.00 mL of an aqueous solution of NaOH to the equivalence point, the molarity of the NaOH solution is ________ 1 M.
How many mL of 7.73 M NaOH are needed to prepare 324 mL of 0.146 M...
How many mL of 7.73 M NaOH are needed to prepare 324 mL of 0.146 M NaOH? Your Answer: Question 5 options: Answer units What is the molarity of a NaOH solution if 27.1 mL are needed to titrate a 0.6119 g sample of KHP? Your Answer: Question 6 options: Answer units
A NaOH solution is standardized using KHP and the molarity of the NaOH solution is determined...
A NaOH solution is standardized using KHP and the molarity of the NaOH solution is determined to be 0.4150 M. Since the acid in vinegar is the monoprotic acid, acetic acid, the concentration of the acetic acid can easily be determined by titration. If 90.72 mL of this solution is required to titrate 10.32 mL of vinegar to the Phenolphthalein endpoint, what is the concentration of acetic acid in the vinegar? _______________ M 95.71 mL of NaOH solution is required...
1. Aspirin is a monoprotic acid. Calculate the volume of 0.493 M NaOH required to titrate...
1. Aspirin is a monoprotic acid. Calculate the volume of 0.493 M NaOH required to titrate a 0.1527-g sample of aspirin. (Pay attention to significant figures in your answer.) 2. A student reached the end point of the titration in the previous question 0.34 mL before expected based on the volume calculated in question 1. What is the purity of the sample? 3. A student required more titrant than predicted as necessary in question 1. Explain why this might occur.