A 50.67 g sample of an unknown acid requires 25.1 ml of a 0.29 M sodium...

A 50.67 g sample of an unknown acid requires 25.1 ml of a 0.29 M sodium hydroxide solution to reach the point of equal moles. Assuming the acid is monoprotic, what would be the molar mass?

what if the acid were diprotic?

FIND: molar mass (mono)

the molar mass of the unknown acid if monoprotic

FIND: molar mass(di)

the molar mass of the unknown acid if diprotic

Solutions

Expert Solution

Thank you ! !

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A 22.26-mL sample of hydrochloric acid solution requires 35.00 mL of 0.115 M sodium hydroxide for...

A 22.26-mL sample of hydrochloric acid solution requires 35.00 mL of 0.115 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?

A) When a 25.1 mL sample of a 0.434 M aqueous acetic acid solution is titrated...

A) When a 25.1 mL sample of a 0.434 M aqueous acetic acid solution is titrated with a 0.320 M aqueous sodium hydroxide solution, what is the pH after 51.1 mL of sodium hydroxide have been added? pH = B) When a 17.5 mL sample of a 0.492 M aqueous nitrous acid solution is titrated with a 0.451 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration? pH =

A 0.1276 g sample of an unknown monoprotic acid was dissolved in 25.0 mL of water...

A 0.1276 g sample of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0633 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 18.4 mL. (a) Calculate the molar mass of the acid. (b) After 10.0 mL of base had been added during the titration, the pH was determined to be 5.87. What is the Ka of the unknown acid? (10 points)

A. A 25.00 mL sample of nitric acid requires 27.75 mL of 0.088 M NaOH to...

A. A 25.00 mL sample of nitric acid requires 27.75 mL of 0.088 M NaOH to reach the end point of the titration. What is the molarity of the nitric acid solution? B. 0.5106 grams of KHP were added to 100.0mL of water. What is the molarity of the KHP solution? (Do not type units with your answer.)

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH after 400.0 mL of acid has been added. 2. A 1.0-L buffer solution contains 0.100 mol HCN and 0.100 mol LiCN. The value of Ka for HCN is 4.9 x 10-10. Because the initial amounts of acid and conjugate base are equal, the pH of the buffer is equal to pKa = -log (4.9 x 10-10) = 9.31. Calculate the new...

1) A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....

1) A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH after 600.0 mL of the acid has been added. 2) A 100.0-mL sample of 0.100 M HCHO2 is titrated with 0.200 M NaOH. Calculate the pH after adding 30.00 mL of the base.

A buffer is created using 100.0 mL of 0.1000 M acetic acid and 1.36 g sodium...

A buffer is created using 100.0 mL of 0.1000 M acetic acid and 1.36 g sodium acetate trihydrate. 1. Calculate the buffer composition from the volume and molarity of the acetic acid and moles of sodium acetate that were added. 2. Calculate the theoretical pH of the buffer using the HH equation and the known pKa for acetic acid (4.74).

1. It requires 10.9 mL of 0.50 M NaOH to neutralize 15.0 mL of an unknown...

1. It requires 10.9 mL of 0.50 M NaOH to neutralize 15.0 mL of an unknown H3PO4 solution. a. Balance the reaction equation. H3PO4 + NaOH Na3PO4 + H2O b. Calculate the initial H3PO4 concentration. 2. It requires 28.1 mL of 16.0 mM H2SO4 to neutralize 11.0 mL of an unknown Ca(OH)2 solution. a. Balance the reaction equation. H2SO4 + Ca(OH)2 ⇋ CaSO4 + H2O b. Calculate the initial Ca(OH)2 concentration.

1.567 g of an unknown Mohr’s salt was dissolved in 80 mL of the sulfuric acid...

1.567 g of an unknown Mohr’s salt was dissolved in 80 mL of the sulfuric acid / phosphoric acid mixture solution. This iron solution was then titrated with a potassium permanganate solution (0.02M), what will be the volume at the equivalence point for the titration? Show all your calculations including formulas.

In a titration of 44.50 mL of 0.3082 M nitrous acid with 0.3082 M aqueous sodium...

In a titration of 44.50 mL of 0.3082 M nitrous acid with 0.3082 M aqueous sodium hydroxide, what is the pH of the solution when 44.50 mL of the base have been added?

Subjects