Question

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 mass of the acid?

c) Which of the common strong acids is this likely to be? c) (10 points) What was the molar concentration of the acid?

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 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the concentration of formic acid in the original solution? What is the pH of the formic acid solution before the titration begins (before the addition of any NaOH)?
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 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the pH of the solution after the addition of 10.00 mL of NaOH solution? What is the pH at the midpoint of the titration? What is the pH at the equivalence point?
A student titrated a 25.00 mL sample of a solution containing an unknown weak, diprotic acid...
A student titrated a 25.00 mL sample of a solution containing an unknown weak, diprotic acid (H2A) with NaOH. If the titration required 17.73 mL of .1036 M NaOH to completely neutralize the acid, calculate the concentration (in M) of the weak acid in the sample.
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...
Background info: Vinegar contains acetic acid, CH3COOH. You can determine the mass of acetic acid in...
Background info: Vinegar contains acetic acid, CH3COOH. You can determine the mass of acetic acid in a vinegar sample by titrating with sodium hydroxide of known concentration. The reaction: CH3OOH(AQ) +NaOH(aq)=> CH3COONa(aq)+H2O(l). I have determined the grams of acetic acid to be 60. There are 25 ml sample of vinegar requiring 41.33 mL of a .953 M solution of NaOH by titrating sodium hydroxide of known concentration. ** THE QUESTION IS: What is the molar concentration of the acetic acid...
You are titrating 50mL of diprotic acid H2X with standardized 0.01M NaOH solution. It takes 25...
You are titrating 50mL of diprotic acid H2X with standardized 0.01M NaOH solution. It takes 25 mL of NaOH to reach the first equivalence point. a. Write down the balanced equation for each of the titration reactions b. What is the volume of base needed to reach the second equivalence point c. Calculate the concentration (M) of the unknown acid solution, H2X
A 21.1 mL sample of a 0.485 M aqueous hypochlorous acid solution is titrated with a...
A 21.1 mL sample of a 0.485 M aqueous hypochlorous acid solution is titrated with a 0.347 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? 12- A 24.0 mL sample of 0.323 M ethylamine, C2H5NH2, is titrated with 0.284 M nitric acid. At the titration midpoint, the pH is :________________.
A 0.3012 g sample of an unknown monoprotic acid requires 24.13 mL of 0.0944 M NaOH...
A 0.3012 g sample of an unknown monoprotic acid requires 24.13 mL of 0.0944 M NaOH for neutralization to a phenolphthalein end point. There are 0.32 mL of 0.0997 M HCl used for back-titration. How many moles of OH- are used? How many moles of H+ from HCl? How many moles of H+ are there in the solid acid? (Use Eq. 5.) moles H+ in solid iacid =moles OH- in NaOH soln. - moles H+ in HCl soln. What is...
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT