### Titration Problem: Determining Concentration of H₃PO₄**Problem Statement:**A 4.50 mL sample of an H₃PO₄ solution of unknown concentration is titrated with a 1.050×10⁻² M NaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point.You may want to refer to (Pages 494 - 497) Section 14.6 while completing this problem.**Part A:**What is the concentration of the unknown H₃PO₄ solution?Express your answer with the appropriate units.[Input Fields]- Value - Units---This problem requires performing a titration calculation to determine the concentration of H₃PO₄ in the given sample. Using the volume and molarity of the NaOH solution, along with the volume of the H₃PO₄ solution, you can calculate the concentration using stoichiometry.

Balanced chemical equation for the neutralization: 3NaOH + H3PO4 -----> Na3PO4 + 3H2O…

Answered: A 4.50 mL sample of an H3 PO4 solution…

A 4.50 mL sample of an H3 PO4 solution of unknown concentration is titrated with a 1.050x10-2 M NaOH solution. A volume of 7.32 mL of the NAOH solution was required to reach the equivalence point.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: If you find that a 69.8 mL sample of vinegar requires 120.31 mL of a 0.504 M solution of NaOH for…

A: To calculate the amount of acetic acid in the vinegar sample, we can use the following balanced…

Q: In an acid-base titration, 27.27 mL of H2SO4 were used to neutralize 35.89 mL of 0.303 M NaOH. What…

Q: An analytical chemist weighs out 0.054 g of an unknown monoprotic acid into a 250 mL volumetric…

Q: A 0.75 L sample of aqueous Ca(OH)2 is titrated with a 0.384 M HCl solution and 0.89 L are required…

A: The chemical reaction taking place during titration is shown below, Observing the balanced reaction…

Q: The antacid "Brand X" was titrated using 0.3 M HCl. The buret reading was initially 0.68 mL. After…

A: Volume of HCl = Final buret reading - initial reading

Q: 30 mL of an unknown concentration of phosphoric acid (triprotic) was titrated with 10 mL 0.05 M…

A: We have to predict the concentration of the acid

Q: Exactly 41.00 mL of 0.100 M NaOH is used to titrate a 25.00 mL sample of HNO3 . What is the…

A: Volume of NaOH = 41.00 mL Concentration of NaOH = 0.100 M Volume of HNO3 = 25.00 mL

Q: A student is asked to standardize a solution of calcium hydroxide. He weighs out 0.952 g potassium…

Q: A sample of 5.00 mL of the HCI received from a tanker is diluted to 250 mL in a volumetric flask. A…

A: 5ml is taken from the tanker and diluted to 250ml. 30.18ml of 2.012M NaOH solution is needed to…

Q: An aqueous sample of 25.0 mL H2SO4 is neutralized by the addition of 28.9 mL of 0.203 M KOH. What…

A: The neutralisation reaction taking place will be 2 KOH + H2SO4 ------> K2SO4 + 2 H2O

Q: Imagine your instructor gave you a solution of carbonic acid (H2CO3) and asked you to determine the…

A: The number of the moles of solute to the volume of solution in liters is known as molarity.

Q: An analytical chemist weighs out 0.127 g of an unknown triprotic acid into a 250 mL volumetric flask…

Q: A 25.0 mL solution of HNO₃ is neutralized with 20.4 mL of 0.250 M Ba(OH)₂. What is the concentration…

A: Given : volume of HNO3 = 25.0 mL Volume of Ba(OH)2 = 20.4 mL…

Q: 34.6°C 78.3°C 100°C 800 760 Normal boiling point Diethyl ether 600 Ethyl alcohol (ethanol) Water 400…

A: The given graph is plotted between vapor pressure (torr) v/s temperature (oC).

Q: A 0.8159 sample of HCl was placed into a 50mL volumetric flask and the sample was thoroughly…

A: In the titration process of an acid and a base which are in a ratio of 1:1, the below given equation…

Q: A titration required 22.30 mL of 2.567 M Sr(OH)2 to neutralize 6.50 g of an unknown diprotic acid.…

A: For Sr(OH)2 solution,Concentration of Sr(OH)2 solution = 2.567 M = 2.567 mol/LVolume of Sr(OH)2…

Q: A 25.0 mL solution of HNO₃ is neutralized with 44.5 mL of 0.250 M Ba(OH)₂. What is the concentration…

A: We know the relation , V1S1 = V2S2 (V1 is the volume of acid ,S1 is strength of acid ,V2 is the…

Q: A student titrates a weak acid with 0.100 M NaOH, adding 31.65 mL before a dark pink color is seen.…

A: The mole of H+ ion the weak acid is equal to the mole of NaOH used in the titration. The molarity…

Q: You conduct a titration experiment to determine the concentration of a H3PO4 solution. Your…

Q: A 5.00 mL sample of 0.25 M HBr solution is titrated with 0.35 M NaOH. What volume of NaOH is…

A: We should equal equivalent of both acid and NaOH ion to volume of NaOH Equivalent =…

Q: A 1.146 g sample of weak acid is dissolved in 164.2 mL of water and titrated with 0.248 M NaOH to…

A: Given, mass of weak acid = 1.146 g Volume of weak acid = 164.2 mL Concentration of NaOH = 0.248 M…

Q: In a titration, it takes.125 L of a 0.50 M NAOH solution to neutralize 235 Lof HCI solution. What is…

A: Given : molarity of NaOH solution = 0.50 M volume of NaOH solution = .125 L volume of HCl solution =…

Q: The molar concentration of an unknown acid solution with general formula H3A is to be determined by…

A: Given Molarity of KOH=0.72 M Volume of KOH=33.33 ml Volume of H3A =17.363ml To determine the…

Q: In an acid-base titration, 27.27 mL of H2SO4 were used to neutralize 35.89 mL of 0.303 M NaOH. What…

A: Given Volume of H2SO4 (V1) = 27.27 mL Volume of NaOH (V2) = 35.89 mL Molarity of H2SO4 = M1…

Q: An aqueous solution containing 12.9 mmol of HCl requires addition of what volume of aqueous 0.200 M…

Q: A 15.00 mL sample of a NaOH solution was titrated with a 0.1053M H2SO4 solution. If 17.88 ml of…

A: Sulfuric acid reacts with sodium hydroxide to form sodium sulfate and water. The equation for the…

Q: A student titrates a weak acid with 0.100 M NaOH, adding 34.84 mL before a dark pink color is seen.…

A: Calculation of no. of mol of NaOH: No. of mol=Molarity×Volume=0.100 mol/L×34.84×10-3 L=3.484 ×10-3…

Q: A 10.00 mL sample of a Ca(OH)2 solution is diluted to 250.0 mL total volume. A 25.0 mL sample of the…

A: The balanced equation isCa(OH)2 + 2 HCl ----> CaCl2 + 2 H2OGiven thatvolume of Ca(OH)2 sample =…

Q: The antacid "Brand X" was titrated using 0.3 M HC. The buret reading was initially 1,71 mL. After…

A: The sample here was titrated using 0.3M HCl. Initial and final burette readings are also given.…

Q: A 25.0 mL solution of HNO₃ is neutralized with 25.6 mL of 0.250 M Ba(OH)₂. What is the concentration…

A: At complete neutralization, no of moles of acid is equal to the no of moles of base

Q: A 25.0 mL solution of HNO is neutralized with 31.6 mL of 0.250 M Ba(OH)₂. What is the concentration…

A: The question is based on the concept of solutions. we are carrying out reaction of base with acid.…

Q: The antacid "TUMS" was titrated using 0.3 M HCl. The buret reading was initially 2.94 mL. After…

A: Given: Initial Burette reading = 2.94 mL Final Burette reading = 21.81 mL To Find: The volume of HCl…

Q: A 15.00 mL sample of aqueous carbonic acid solution of unknown concentration requires titration with…

A: Number of moles = concentration x volume n- factor =2 for carbonic acid. n- factor=1 for sodium…

Q: A 0.4574 g sample containing only NaCN and KCN requires 41.65 ml of 0.1056 M AgNO3 for titration.…

Q: a 0.8159g sample of HCL was placed into a 50mL volumetric flask and the sample was thoroughly…

A: Balanced chemical equation: HCl (aq) + NaOH (aq) ------> NaCl (aq) + H2O (l) This suggest…

Q: take a 25.00 mL sample of 0.150 M hypochlorus acid and to it add 10 mL of 0.130 M NaOH. What is the…

Q: You have a solution of NaOH of unknown concentration. A 15.98 mL sample of the NaOH solution was…

A: Concentration of NaOH = To be determined Volume of NaOH = 15.98 mLMolarity of HNO3 = 0.377 MVolume…

Q: A 0.050 solution of Ba(OH)2 is neutralized by 0,072 L of a 0.55 M HNO3 solution. What is the…

A: Given: The volume of HNO3 = 0.072 L The concentration of HNO3 = 0.55 M The volume of Ba(OH)2…

Q: When titrating a 0.4444 g sample of KHP (molar mass = 204.2 g/mol), it took 18.54 mL of sodium…

Q: 13.07 ml of an Unknown Acid titrated with 24.03 ml of a Base standardized to 0.10000M. What is the…

Q: A 0.307-g sample of an unknown triprotic acid is titrated completely using 35.2 mL of 0.106 M NaOH.…

Q: A 0.261 g sample of NaHC2O4 (one acidic proton) required 17.5 mL of sodium hydroxide solution for…

A: A chemical reaction between NaHC2O4 and NaOH can be written in the form of an equation as shown…

Q: Calculate the molarity of dilute Ca(OH)2 solution if the titration of 30.00 mL of 0.05231 M HCl…

A: We need to calculate the Molarity of dilute Ca(OH)2 solution. It is given that, 30.00 ml of 0.05231…

Q: solution

A: Dear student I have given answer to your question in the image format.

Q: A 50.25 g sample of Ca(OH)2 is dissolved in some water. Determine how many mL of 0.525 M HClO4 will…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

### Titration Problem: Determining Concentration of H₃PO₄

**Problem Statement:**

A 4.50 mL sample of an H₃PO₄ solution of unknown concentration is titrated with a 1.050×10⁻² M NaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point.

You may want to refer to (Pages 494 - 497) Section 14.6 while completing this problem.

**Part A:**

What is the concentration of the unknown H₃PO₄ solution?

Express your answer with the appropriate units.

[Input Fields]
- Value
- Units

---

This problem requires performing a titration calculation to determine the concentration of H₃PO₄ in the given sample. Using the volume and molarity of the NaOH solution, along with the volume of the H₃PO₄ solution, you can calculate the concentration using stoichiometry.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A solution of H2C2O4 is used to titrate a 18.42 mL sample of a 0.2079 M KOH solution. If the titration requires 13.51 mL of the H2C2O4 solution, what is its molarity? I need the work to understand it
0.2 mL of 0.10M NaOH is needed to titrate an unknown acid with a volume of 10.15mL. What is the final concentration of the resulting titrated sample?
A 31.5 mL sample of a 0.489 M aqueous nitrous acid solution is titrated with a 0.425 M aqueous solution of barium hydroxide. How many milliliters of barium hydroxide must be added to reach a pH of 3.158? mL
Acid 3- Fluro benzoic NO2 NO2 Nitro ben zene 1,3- Dinitro benzene HO. Fina! (3- Fluoro kenzayamine) NH2 3- Fluoro ben zamide
Chaya the chemistry student carries out a titration by adding an aqueous solution of NaOH to an aqueous solution of the weak acid HY. The images below represent the solutions formed at various points during this titration. (Na+ and H₂O are omitted for clarity.) HY OY &H30+ О ОН A B C Select the image corresponding to each of the following points in Chaya's titration. Before adding any NaOH : -- + Partway to the equivalence point: -- At the equivalence point : -- After the equivalence point: [ → D E y selecting h menu.
The antacid "Brand X" was titrated using 0.3 M HCl. The buret reading was initially 1.34 mL. After reaching the endpoint, the final volume reading was 12.67 mL. What volume of HCl was used in this titration? Include a unit in your answer.
A 4.80 mL sample of an H3PO4 solution of unknown concentration is titrated with a 1.100×10−2 M NaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4 solution? Express your answer with the appropriate units.
An aqueous solution of Ca(OH)2with a concentration of 0.188 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid?
O SIMPLE REACTIONS Determining the molar mass of an acid by titration Jacque An analytical chemist weighs out 0.279 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 33.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol fo Exnation Check |Privecy 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use MacBook Air
A 10.00 mL sample of H2SO4 acid solution requires 22.53 mL of 0.1000 M NaOH for titration. What is the molarity of the acid solution?
A sample of oxalic acid (a diprotic acid of the formula H2C2O4) is dissolved in enough water to make 1.00 L of solution. A 100.0 mL sample of this solution is titrated with a solution of sodium hydroxide (NaOH) of concentration 0.750 M and requires 20.0 mL of sodium hydroxide to reach the end point. Calculate the mass of the original oxalic acid sample. H2C2O4 + 2NaOH → Na2(C2O4)+ 2H2O
what is the molarity of a solution of phosphoric acid (a tricrotic acid) if 10.00 mL of the phosphoric acid solution requires 38.11 mL of 0.2412 M NaOH solution to titrate it?