Question

After standardizing your NaOH solution, you have determined that the concentration is actually 0.1125 M. What...

After standardizing your NaOH solution, you have determined that the concentration is actually 0.1125 M. What is the weight percent concentration of KHP (MW=204.23) in your unknown sample of mass 1.625 g if it takes 38.40 mL of titrant to reach the equivalence point?

A student weighs out 1.7500 grams of dried potassium hydrogen phthalate standard (MW=204.23) and finds that it takes 39.05 mL to reach the endpoint of the titration with the solution of NaOH. What is the molarity of the NaOH titrant?

After standardizing your NaOH solution, you have determined that the concentration is actually 0.1125 M. If your unknown contains a 35.60 weight percent concentration of KHP (MW=204.23) in your unknown sample of mass 1.500 g how many milliliters of titrant will be needed to reach the equivalence point of the titration?

Homework Answers

Answer #1

KHP + NaOH ----> salt + H2O

No of mol of NaOH = 38.4/1000*0.1125 = 0.00432 mol

No of mol of KHP reacted = 0.00432 mol

mass of kHP reacted = 0.00432*204.23 = 0.88 grams

mass percentage =   0.88 / 1.625*100 = 54.15%


No of mol of KHP reacted = 1.75/204.23 = 0.00857 mol

Molarity of NaOH = 0.00857/39.05*1000 = 0.22 M


No of mol of KHP = 1.5*(35.6/100)*(1/204.23) = 0.0026 mol

No of mol of NaOh = 0.0026 mol

volume of NaOH needed = 0.0026 / 0.1125 = 23.11 ml

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. A student dissolves 1.1007 grams of their KHP unknown in 50.0 mL of water. The...
a. A student dissolves 1.1007 grams of their KHP unknown in 50.0 mL of water. The molarity of the student’s NaOH titrant is 0.0999 M. If it takes 40.25 mL of the sodium hydroxide titrant to reach the equivalence point, what is the wt% KHP (MW=204.23) in the unknown? b. If the student uses 55.0 mL of water instead of 50.0 mL to dissolve the unknown, what affect, if any, does this have on the calculated weight % of the...
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...
In analytical chemistry, bases used for titrations must often be standardized; that is, their concentration must...
In analytical chemistry, bases used for titrations must often be standardized; that is, their concentration must be precisely determined. Standardization of sodium hydroxide solutions can be accomplished by titrating potassium hydrogen phthalate (KHC8H4O4), also know as KHP, with the NaOH solution to be standardized. The titration of 0.5727 g of KHP required 24.70 mL of an NaOH solution to reach the equivalence point. What is the concentration of the NaOH solution?
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
To standardize a solution of NaOH, one uses a primary standard called potassium hydrogen phthalate. It...
To standardize a solution of NaOH, one uses a primary standard called potassium hydrogen phthalate. It is a monoproctic acid that can be obtained extremely pure and dried to a constant weight. It has a molar mass of 204.33 g/mol. suppose you weigh out 0.556 g of KHP and dissolve it in water. It requires 14.48 mL of NaOH solution to reach the endpoint. What is the concentration of the NaOH solution? The NaOH solution from above is used to...
An approximately 0.1 M NaOH solution is prepared by adding 2.0 g of solid NaOH to...
An approximately 0.1 M NaOH solution is prepared by adding 2.0 g of solid NaOH to 500 mL of water. The precise concentration of the solution is determined by titrating the NaOH against weighed portions of a weak acid, pot assium hydrogen phthalate (KHP), obtained from the National Institute of Standards and Technology (NIST) and certified as being 99.99% pure. The KHP samples are weighed by difference on an analytical balance. Following its standardization, the NaOH solut ion is used...
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of...
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of 0.1 M H3PO4? Question options: a) V = 12 mL b) V = 6 mL c) V = 18 mL d) V = 30 mL he pH at the equivalence point when a 0.20 M weak base (Ka = 9.1 x 10-7) is titrated with a 0.20 M strong acid is: Question options: a) pH = 2.9 b) pH = 1.7 c) pH =...
You are given a sulfuric acid solution of unknown concentration. You dispense 10.00 mL of the...
You are given a sulfuric acid solution of unknown concentration. You dispense 10.00 mL of the unknown solution into an Erlenmeyer flask and add 12.20 mL of distilled water and a drop of phenopthalein to the flask. You fill your buret with 0.103 M NaOH (aq) solution and begin the titration. During the titration you rinse the tip and the sides of the Erlenmeyer flask with 3.52 mL of distilled water. It requires 10.38 mL of your NaOH (aq) solution...
a) If your titration solution is 0.409 M in NaOH, and the endpoint occues at 13.00...
a) If your titration solution is 0.409 M in NaOH, and the endpoint occues at 13.00 mL of titrant, how many mmol of NaOH are required to reach the endpoint? ____ mmol NaOH b) How many mmol of acetic acid (HC2H3O2) are required to react with the NaOH? ____ mmol HC2H3O2 c) How many grams of acetic acid is this? ____ grams HC2H3O2 d) If the mass of analyte is 10.15 grams, what is the mass % of acetic acid...
(a) If your titration solution is 0.410 M in NaOH, and the endpoint occurs at 13.50...
(a) If your titration solution is 0.410 M in NaOH, and the endpoint occurs at 13.50 mL of titrant, how many mmol of NaOH are required to reach the endpoint? __?__mmol NaOH (b) How many mmol of acetic acid (HC2H3O2) are required to react with the NaOH? __?__ mmol HC2H3O2 (c) How many grams of acetic acid is this? __?__ grams HC2H3O2 (d) If the mass of analyte is 10.05 grams, what is the mass % of acetic acid in...