Calculate the concentration of phosphoric acid in a solution if 25.0 mL of that solution required...

Question

Question

Calculate the concentration of phosphoric acid in a solution if 25.0 mL of that solution required 35.2 mL of 0.189 M KOH for neutralization

science chemistry

Answer 1

Similar Homework Help Questions

If a 25.0 mL sample of phosphoric acid, H3PO4, is completely neutralized by 137 mL of...

If a 25.0 mL sample of phosphoric acid, H3PO4, is completely neutralized by 137 mL of 0.100 M KOH, what is the molarity of the phosphoric acid? Given: H3PO4 + 3 KOH → 3 H2O + K3PO4
a) Calculate the final concentration when 25.0 mL of an 18.0 M HCl solution is diluted...

a) Calculate the final concentration when 25.0 mL of an 18.0 M HCl solution is diluted to 0.500 L. b) Calculate the volume required when an 8.50 M KOH solution is diluted to form 95.0 mL of a 0.500 M KOH solution
If a 25.0 mL solution of acetic acid of unknown concentration required 30.0 mL of 0.100M...

If a 25.0 mL solution of acetic acid of unknown concentration required 30.0 mL of 0.100M NaOH solution to be neutralized, what is the concentration of the unknown substance.

A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution....

A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
Acid-base titration questions. Please help! Thanks. 2. Given that 20.00 mL of phosphoric acid solution required...

Acid-base titration questions. Please help! Thanks. 2. Given that 20.00 mL of phosphoric acid solution required 15.50 mL of 0.200M NaOH for the first equivalent point. What is the molarity of the phosphoric acid? 3. A student titrated 25.00 mL of cola and it required 18.27 mL of 0.0100 M NaOH to reach the 1'equivalence point. Calculate the molar concentration of phosphoric acid in this brand of cola. 4. If the density of the "Cola" drink is 1.00 g/mL. What...
1.5 g of solid phosphoric acid was dissolved in 250.00 mL volumetric flask. 25.0 mL of this solution neutralize 24.60 mL...

1.5 g of solid phosphoric acid was dissolved in 250.00 mL volumetric flask. 25.0 mL of this solution neutralize 24.60 mL of LiOH solution. Calculate the molarity of LiOH

a. A 25.0 mL of a solution of acetic acid (HA) of unknown concentration is titrated with...

a. A 25.0 mL of a solution of acetic acid (HA) of unknown concentration is titrated with 0.0919 M NaOH and the equivalence point volume was determined by graphical means to be 25.91 mL. What is the concentration of the acetic acid? concentration of HA = ___ M b. Calculate the pKa of a weak monoprotic acid if the pH of a 0.162 M solution is 2.52. pKa = ___
An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH....

An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH. What is the concentration of the acid? H3PO4 (aq) + 3 KOH(aq) - K3PO4 (aq) + 3 H2O) Initial volume of KOH solution 1.03 mL Final volume of KOH solution 15.02 mL Original volume of H3PO4 solution 24.68 mL O 0.001260M 0.05104 M 0.1531 M 0.4593M
An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH....

An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH. What is the concentration of the acid? H3PO4 (aq) + 3 KOH(aq) – K3PO4 (aq) + 3 H200) Initial volume of KOH solution 1.03 mL Final volume of KOH solution 15.02 ml Original volume of H3PO, solution 24.68 ml O 0.001260M 0.4593 M 0.05104 M 0.1531M

What is the concentration of a solution of HNO3 if 25.0 mL of the acid requires...

What is the concentration of a solution of HNO3 if 25.0 mL of the acid requires 13.5 mL of 0.200 M NaOH?