Question

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 error (positive or negative) did this cause in her reported molar mass? Please explain.

Homework Answers

Answer #1

1 mol triprotic acid = 3 mol naOH

no of mol of NaOH reacted = 26.42*0.1013/1000 = 0.00268 mol

no of mol of triprotic acid = 0.00268/3 = 0.000893 mol

molarmass of triprotic acid = w/n = 0.154/0.000893 = 172.45 g/mol

if The volume of the NaOH solution was actually 23.58 mL that she used.

no of mol of NaOH reacted = 23.58*0.1013/1000 = 0.00239 mol

no of mol of triprotic acid = 0.00239/3 = 0.000797 mol

molarmass of triprotic acid = w/n = 0.154/0.000797 = 193.224 g/mol

so that, correct value is higher than first calculated,that results -ve error.

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
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)
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...
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
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
A student from lab obtained 0.723 grams of potassium hydrogenphthalate (KHP, molar mass of 204.2 g/mol)....
A student from lab obtained 0.723 grams of potassium hydrogenphthalate (KHP, molar mass of 204.2 g/mol). The KHP was added to a 150 mL erlenmeyer flask along with 50 mL of DI water and a few drops of phenolphthalein indicator. The solution was stirred until all KHP was dissolved. The student obtained what was marked as - 0.1M NaOH solution and filled their buret until the meniscus was sitting on 0.50 mL line. The student proceeded to add the sodium...
Bob Cat is attempting to determine the molarity of an unknown solution of acetic acid. He...
Bob Cat is attempting to determine the molarity of an unknown solution of acetic acid. He began by mixing an aqueous NaOH solution and standardizing it by titration of KHP with phenolphthalein indicator. He then titrated the acetic acid solution with his standardized NaOH. The data from one of Bob’s trials is below, but he still needs to complete his calculations. The molar mass of KHP is 204.2 g. Titration of KHP Titration of Acetic Acid mass of KHP (g)...
Suppose that 14.56 ml of a 0.115 M solution NaOH (aq) was required to neutralize 0.0822g...
Suppose that 14.56 ml of a 0.115 M solution NaOH (aq) was required to neutralize 0.0822g of an unknown triprotic acid, H3X. What is the molecular weight (g/mol) of the unknown acid? What I have so far: H3X + 3NaOH -> Na3X + 3H2O 0.0822/[0.115M (mol/L) NaOH × 0.01456L × (1molH3X/3molNaOH)] = 147g/mol H3X What is the mass percent of protons of the unknown acid? <- This question please. Thanks. ?
A 0.1000 M NaOH solution was employed to titrate a 25.00-mL solution that contains 0.1000 M...
A 0.1000 M NaOH solution was employed to titrate a 25.00-mL solution that contains 0.1000 M HCl and 0.0500 M HOAc. Please determine the pH of the solution after 27.00 mL of NaOH is added. Ka, HOAc = 1.75*10-5 . Answer. 4.04 Just want to see how they got that.
How many mL of a 0.100 M NaOH solution would be needed to titrate 0.156 g...
How many mL of a 0.100 M NaOH solution would be needed to titrate 0.156 g of butanoic acid to a neutral pH endpoint?
Using the above sodium hydroxide solution, 27.21 mL of the NaOH solution is required to neutralize...
Using the above sodium hydroxide solution, 27.21 mL of the NaOH solution is required to neutralize a volume of 31.86 mL of an acidic solution having an unknown concentration to a phenolphthalein end point. Determine the concentration of the acidic solution, assuming that the acid is diprotic, such as sulfuric acid. Start with a balanced equation. 0.02086 0.001329 0.04172 0.4384 0.01256 0.05024
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT