A titration of 65.0 mL of a sulfuric acid (H,SO) solution of unknown concentration with a standardized 1.55 M Ba(OH), solution requires 23.0 mL to reach the second equivalence point. What is the concentration of the H,SO, solution?

A titration of 65.0 mL of a sulfuric acid (H,SO) solution of unknown concentration with a standardized 1.55 M Ba(OH), solution requires 23.0 mL to reach the second equivalence point. What is the concentration of the H,SO, solution?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.93QE

See similar textbooks

Related questions

Q: What volume (in mLmL) of 0.200 M NaOHM NaOH do we need to titrate 36.00 mLmL of 0.140 M HBrM HBr…

Q: In a titration 40.0 mL of HCl is put in a flask with a few drops of phenolphthalein. A solution of…

A: Given: Volume of HCl V1= 40 mL Volume of NaOH V2= 20 mL Concentration of NaOH M2= 0.200M To find:…

Q: What is the pH at the equivalence point in the titration of a 23.6 mL sample of a 0.479 M aqueous…

Q: What is the pH at the equivalence point in the titration of a 16.3 mL sample of a 0.497 M aqueous…

Q: A 25.00-mL sample of an HI solution is titrated to the equivalence point using 0.639 M KOH. If the…

A: The equation used to calculate the unknown values is, M1V1=M2V2 where M is the molarity and V is the…

Q: A 0.4574 g sample containing only NaCN and KCN requires 41.65 ml of 0.1056 M AGNO3 for titration.…

A: Given: mass of NaCN + KCN = 0.4574 g Volume of AgNO3 = 41.65 mL Concentration of AgNO3 = 0.1056 M…

Q: A 40.00 solution of 0.1430 M chloroacetic acid (pKa = 2.865) is titrated with a 0.1500 M solution of…

A: Given, Volume Of the Solution = 40ml Concentration Of Chloroacetic acid = 0.1430 M Concentration…

Q: A student performs a titration of 35.0 mL of a phosphoric acid (H,PO,) solution of unknown…

A: The question is based on the concept of titrations. it involves titration of a weak acid phosphoric…

Q: A 25.00 mL sample of aqueous carbonic acid solution of unknown concentration requires titration with…

A: Given, A 25.00 mL sample of aqueous carbonic acid solution of unknown concentration requires…

Q: 78.48 mL of a solution of the acid HNO3 is titrated, and 66.50 mL of 0.7900-M NaOH is required to…

A: The volume of HNO3, V1=78.48 mL The volume of NaOH, V2= 66.50 mL The concentration of NaOH,…

Q: How many milliliters of 0.105 M HCl are needed to titrate eachof the following solutions to the…

A: Normality equation : Let , S1 (N) normal and V1 mL acid is completely neutralized by S2 (N) normal…

Q: 6.A 16.6 mL aliquot of 0.2 M aqueous hydrochloric acid is titrated with 0.6 M NaOH (ac). What volume…

A: Given that: volume of HCl = 16.6 mL molarity of HCl = 0.2 M molarity of NaOH = 0.6 M To find, the…

Q: A 15.5 mL sample of a solution Sr(OH)2 is titrated to the equivalence point with 65.2 mL of 0.7807 M…

A: Acids and bases neutralize each other. Strontium hydroxide will neutralize hydrochloric acid to…

Q: When a 28.4 mL sample of a 0.467 M aqueous hydrofluoric acid solution is titrated with a 0.446 M…

A: Answer: In this question we have to calculate the pH of two types of solution those are forming at…

Q: Molarity of the standard solution of sodium hydroxide = 0.1110 mol/L Volumes of NaOH (aq): Rough…

A: Titrimetric analysis:

Q: The pKa of hypochlorous acid is 7.530. A 56.0 mL solution of 0.126 M sodium hypochlorite (NaOCl) is…

Q: A 10.00 mL sample of a solution of hydrofluoric acid, HF, is diluted to 500.00 mL. Of this, 20.00 mL…

A: The chemical reaction is, Calculate the diluted morality of HF, HF=13.51×10-3 L NaOH20 ×10-3…

Q: A 35.00 mL volume of formic acid is titrated with 0.1428 M potassium hydroxide (KOH). If 24.39 mL…

A: Given: The concentration of potassium hydroxide (KOH)=0.1428 M The volume of potassium hydroxide…

Q: A hydrochloric acid solution is standardized by titrating 0.2329 g of primary standard sodium…

A: Interpretation- Molarity of HCl. Concept information- Molarity - ratio of number of moles of solute…

Q: What is the pH at the equivalence point in the titration of a 20.4 mL sample of a 0.444 M aqueous…

Q: If 0.626 g of an unknown monoprotic acid was used to prepare a 25.00 mL weak acid solution and this…

Q: How many mL of 0.13 M NaOH have to be added to reach the equivalence point when 15.00 mL of 0.14 M…

A: Here 3H+ neutralizing with 1OH- thus the formula is:- 3M1V1(NaOH)= M2V2(H3PO4)

Q: What is the pH at the equivalence point in the titration of a 15.0 mL sample of a 0.315 M aqueous…

A: Answer:- Firstly from the given data, concentration of the conjugate base of hypochlorous acid is…

Q: The following acid solutions were titrated to the equivalence point with the base listed. Use the…

A: Neutralization formula for acid-base titration is, M1V1n1=M2V2n2 where, M1 = Molarity of acid V1 =…

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

Q: When a 22.9 ml. sample of a 0.347 M aqueous nitrous acid solution is titrated with a 0.309 M aqueous…

A: The volume of the sample = 22.9 mL The molarity of the sample = 0.347 M The molarity of Ba(OH)2…

Q: When a 24.3 mL sample of a 0.359 M aqueous hydrofluoric acid solution is titrated with a 0.382 M…

A: 1.) We would use the fact that at half equivalance point , pH = pKa of weak acid. 2.) To…

Q: Image attached

A: Given, Salt = NaCN acid = HCl Molarity of NaCN = 0.10 M Volume of NaCN = 25.0 mL Molarity of HCl…

Q: A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated…

A: The volume of 0.01252 M HCl used for titration is 17.94 mL. The volume of solution titrated against…

Q: 15.00 mL of an ammonia sample (D = 0.980 g/mL) is titrated to endpoint with 31.25 mL of a 0.500M HCI…

Q: A student performs a titration of 53.0 mL of a phosphoric acid (H3PO:) solution of unknown…

A: We know, V1S1 = V2S2 Where, S1 =Concentration of NaOH V1 =Volume of NaOH solution V2 =volume of…

Q: A solution containing 2.09 g of a diprotic acid H,C3H,O4 (malonic acid) was titrated with 45.5 mL of…

Q: When 10.23 ml of an unknown weak acid was titrated, it required 12.08 mL of 0.423M NaOH to reach the…

A: Given that : Volume of NaOH (V1) = 12.08 mL Molarity of NaOH (M1) = 0.423 M Volumes of weak acid…

Q: 6.) A 25.00-mL sample of HCI is titrated with 0.1001 M NaOH, 49.90 ml of base is required to reach…

Q: A titration of 3.36 g of an acid requires 43.72mL of 0.100M NaOH to reach the equivalence point.…

Q: What volume of base is required to reach the equivalence point in a titration of 20.00 mL of 0.11 M…

Q: The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret…

A: In this problem, the volume of sodium hydroxide can be calculated only when the initial…

Q: 30.23 mL of a solution of the acid H2SO4 is titrated, and 47.20 mL of 0.8600-M NaOH is required to…

A: H2SO4 is a dibasic acid, so it will give 2 H+ ions on dissociation (Basicity =2) NaOH is a…

Q: Caitlin titrated 25.00 mL of 0.40 M formic acid with 0.25 M LIOH. What volume of lithium hydroxide…

A: Equivalence point: it can be define as the point where moles of the titrant are equal to the moles…

Q: HCN is a weak acid with a Ka = 4.90 x 1010 A 50.00 mL sample of this HCN solution %3D (0.250 M) is…

A: Given: Ka = 4.90 × 10-10 Concentration of sample = 50 mL Molarity of HCN = 0.250 M Molarity of NaOH…

Q: What volume of 0.05 M NAOH must be added to reach the final equivalence point in the titration of…

Q: In the titration of a 25.00 mL sample of the hypothetical monoprotic acid, CHEM, it took 20.41 mL of…

Q: 17.A 16.6 mL aliquot of 0.2 M aqueous hydrochloric acid is titrated with 0.6 M NaOH (ac). What…

Q: You are titrating 21.00ml of a 0.850 M solution of NH3(ammonia) with a strong acid. If you add…

A: A basic buffer is acquired on mixing weak bases with their conjugate salts in a definite ratio. They…

Q: 5. The diagram below shows the titration curves for weak and strong base using 0.100 M as titraot I…

A: Given: Volume of base solution = 25.0 mL Concentration of HCl = 0.100 M And the titration curve…

Q: A student titrates 25.0 ml. of an unknown acid with 0.1 M KOH, The student determines that it takes…

A: The given information is: Volume of unknown acid = 25.0 ml Molarity of KOH = 0.1 M Volume of KOH…

Q: How many mL of 0.21 M NaOH have to be added to reach the equivalence point when 15.00 mL of 0.29 M…

Q: Compare the two quantities based on the given condition: X: Titration of 25 mL 0.10 M HX (weak acid)…

A: Given:

Q: A titration of 79.0 mL of a tartaric acid (H,C HO.) solution of unknown concentration with 0.805 M…

Q: A titration of 65.0 mL of a tartaric acid (H,C,HO.) solution of unknown concentration with 0.805 M…

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

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

What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
Morphine, C17H19O3N, is a weak base (K b =7.4107). Consider its titration with hydrochloric acid. In the titration, 50.0 mL of a 0.1500 M solution of morphine is titrated with 0.1045 M HCl. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of hydrochloric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HCl is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?
A titration of 40.0 mL of a sulfuric acid (H₂SO₄) solution of unknown concentration with a standardized 1.55 M Ba(OH)₂ solution requires 23.0 mL to reach the second equivalence point. What is the concentration of the H₂SO₄ solution?
What volume of 0.2045 M NaOH is necessary to titrate 50.00 mL of 0.1177 M acetic acid, CH3COOH ?
For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, what is the% base amount in CaCO3? (CaCO3: 100,087 g / mol)
For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, which of the following is the% base amount in CaCO3? (CaCO3: 100,087 g / mol)
What is the normality of 50.0 ml Ba(OH)2 solution when titrated with 23.50 mL of 0.250 N HCl?
You are given solutions of HCl and NaOH and must deter-mine their concentrations. You use 27.5 mL of NaOH to titrate100. mL of HCl and 18.4 mL of NaOH to titrate 50.0 mL of 0.0782 M H₂SO₄. Find the unknown concentrations
2. Calculate the molarity of a solution of potassium hydroxide, KOH. If 33 mL of this base were titrated with a 1.5 M HNO3 standard and 20 mL were consumed. KOH + HNO3 KNO3 + H2O
The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.180 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
Assume the equivalent weight of an acid is 51.0.51.0. Calculate the number of mL of 0.233 M0.233 M NaOHNaOH that would be needed to titrate 0.466 g0.466 g of the acid.
If 14.45 ml of H2SO4 is required to reach the end point when titrated with 25.00 ml of 0.9298 M NaOH, what is the concentration of the acid?