Question

0.1532-g of an unknown diprotic acid requires 32.41 mL of 0.1050M sodium hydroxide to completely neutralize...

0.1532-g of an unknown diprotic acid requires 32.41 mL of 0.1050M sodium hydroxide to completely neutralize the acid. The acid elemental composition is 26.68% C, 71.08% O, and 2.24% H. What is the molecular formula of this acid?

Homework Answers

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
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
The following questions involve the reaction of sodium hydroxide and succinic acid. Succinic acid is diprotic:...
The following questions involve the reaction of sodium hydroxide and succinic acid. Succinic acid is diprotic: the acid (H2C4H4O4) reacts with two of its hydrogens to give C4H4O42-. The balanced "molecular" equation for the reaction has coefficients of 2 for NaOH and 1 for succinic acid: 2 NaOH (aq) + H2C4O4 (aq) --> Na2C4H4O4 (aq) + 2 H2O (l) A student weights 1.700 g of succinic acid and dissolves it in water in a 250.0 mL volumetric flask. A 25.00...
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
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
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 student dissolves 153 milligrams of a diprotic acid in water and titrates the solution with...
A student dissolves 153 milligrams of a diprotic acid in water and titrates the solution with a 0.150 M solution of sodium hydroxide. It takes 27.15 mL of sodium hydroxide to neutralize the acid. What is the molar mass (in g/mol) of the acid?
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...
1. A student is asked to standardize a solution of sodium hydroxide. He weighs out 0.939...
1. A student is asked to standardize a solution of sodium hydroxide. He weighs out 0.939 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 27.5 mL of sodium hydroxide to reach the endpoint. A. What is the molarity of the sodium hydroxide solution? ______M This sodium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid. B. If 14.7 mL of the sodium hydroxide solution is required to neutralize 23.4 mL ofhydrobromic...
A solution contains 11.45 g of unknown compound dissolved in 50.0 mL of water. (Assume a...
A solution contains 11.45 g of unknown compound dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -4.73 ∘C. The mass percent composition of the compound is 53.31% C, 11.19% H, and the rest is O. What is the molecular formula of the compound? Express your answer as a molecular formula.
A 11.9 g sample of an aqueous solution of perchloric acid contains an unknown amount of...
A 11.9 g sample of an aqueous solution of perchloric acid contains an unknown amount of the acid. If 19.2 mL of 2.80 M potassium hydroxide are required to neutralize the perchloric acid, what is the percent by mass of perchloric acid in the mixture? A 10.7 g sample of an aqueous solution of hydroiodic acid contains an unknown amount of the acid. If 17.4 mL of 1.66 M sodium hydroxide are required to neutralize the hydroiodic acid, what is...