By titration, it is found that 70.1 mL of 0.161 M NAOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate theconcentration of the HCl solution.[HCI] =MQuestion Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books

Answered: Image /qna-images/answer/a12d316e-c9cb-439b-bfc3-98a9d5c4afa1.jpg

Answered: By titration, it is found that 70.1 mL…

By titration, it is found that 70.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of HCI(aq). Calculate the concentration of the HCl solution. [HC1] = M

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 2ASA: In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a...

See similar textbooks

Related questions

Q: An aqueous solution of perchloric acid is standardized by titration with a 0.198 M solution of…

A: Given- Concentration of calcium hydroxide =0.198M Volume of calcium hydroxide =19.0 mL Volume…

Q: The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide…

Q: An aqueous solution of sodium hydroxide is standardized by titration with a 0.142 M solution of…

Q: Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811 M NaOH to reach the end point.…

A: The neutralisation reaction taking place between NaOH and H2SO4 is given by NaOH + H2SO4…

Q: What volume of 0.812 M HCl, in milliliters, is required to titrate 1.45 g of NaOH to the equivalence…

Q: Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:…

Q: The acidic substance in vinegar is acetic acid, HC2H302. When 6.05 g of a certain vinegar sample was…

Q: Solid iron(III) hydroxide is added to 633 mL of 0.270 M HCl. The resulting solution is acidic and…

Q: Calculate the molarity of an acetic acid solution, HC2H3O2(aq), if a 50.0 mL sample requires 45.6 mL…

A: molarity is concerned with the moles of a solute in relation to the volume of a solution.…

Q: The following chemical reaction takes place in aqueous solution: AgF(aq)+KBr(aq) →A£B1(s)+KF(aq)…

Q: A solution of malonic acid, H2C3H2O4, was standardized by titration with 0.1000 M NaOH solution. If…

Q: A student prepares a solution of hydrochloric acid that is approximately 0.1 M and wishes to…

A: 3 (a) Given :- molarity of NaOH solution = 0.07575 M volume of NaOH solution = 38.92 mL volume…

Q: A 0.9600 M NaOH solution was diluted with a factor of 4. Then the diluted solution of NaOH was…

A: Th dilution factor is simply the ration between final volume of the diluted solution to the initial…

Q: 1. When H2SO4(aq) was reacted with NaOH(aq) in the titration, why was a precipitate not formed? 2.…

A: 1. On the reaction of NaOH with H2SO4, we get Na2SO4 and water. The sodium sulfate Na2SO4 is a…

Q: The molarity of an aqueous solution of hydrochloric acid, HCl, is determined by titration with a…

A: Given: Titration of HCl with KOH.

Q: What volume (in mL) of 0.197 mol/L sodium hydroxide, NaOH (aq), is needed to completely neutralize…

A: Given: Concentration of NaOH = 0.197 M Concentration of HCl = 0.298 M And volume of HCl solution to…

Q: The end point in a titration of a 50.00-mL sample of aqueous HCl was reached by addition of 35.23 mL…

A: Given reaction: HCl(aq) + NaOH(aq) ⟶ NaCl(aq) + H2 O(l)

Q: The following chemical reaction takes place in aqueous solution: AgNO,(aq)+NH,Cl(aq)…

A: Ionic equation: It is a chemical reaction where molecules dissolved in water are written in ions…

Q: By titration it is found that 114.3 mL of 0.562 M NaOH is needed to titrate 48.0 mL of HCl. What is…

A: Here given, Volume of NaOH (V1) = 114.3 mL Strength of NaOH (S1) = 0.562 M Volume of HCl (V2) = 48…

Q: Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811MNaOH to reach the end point. If…

A: As per the question, assuming that the acidity of the rain is due to the presence of sulfuric acid…

Q: An aqueous solution of barium hydroxide is standardized by titration with a 0.180 M solution of…

A: Barium hydroxide reacts with perchloric acid as follows: The stoichiometry of the balanced chemical…

Q: A titration of a 25.00 mL sample of a hydrochloric acid solution of unknown molarity reaches the…

A: The equivalence point in acid base solution is Moles of acid = Moles of base

Q: What volume of 0.923 M HCl , in milliliters, is required to titrate 1.10 g of NaOH to the…

A: The number of moles for a given compound can be called as the ratio of the mass to that of molecular…

Q: A student conducted a titration by adding 12.0 mL of NaOH(aq) of unknown concentration to 16.0 mL of…

A: An acid reacts with a base to form salt and water. The given acid is HCl and base is NaOH. HCl…

Q: An aqueous solution of hydroiodic acid is standardized by titration with a 0.137 M solution of…

A: The hydrochloric acid reacts with calcium hydroxide to form calcium chloride and water. The equation…

Q: The following chemical reaction takes place in aqueous solution: MgCl,(aq)+2 KOH(aq) →Mg (OH),(s)+2…

Q: A student titrates a 10.00-mL sample of an HCI solution, using a 0.365 M solution of NaOH. She finds…

Q: Suppose you have a solution that might contain one or more of the following cations: lead (II) ion,…

A: All the chloride salts are soluble except Lead(II)chloride, silver(I)chloride, and HgCl2. All the…

Q: The following chemical reaction takes place in aqueous solution: MnCl,(aq)+2 KOH(aq) →Mn(OH),(s)+2…

A: The given molecular equation is : MnCl2 (aq) + 2KOH (aq) --------> Mn(OH)2 (s) + 2KCl (aq)

Q: By titration it is found that 28.7 milliliters of 0.155 M NaOH(aq) are required to neutralize 25.0…

Q: 1Ing the Volume of base needed to titrate a given mass... A chemistry student weighs out 0.196 g of…

A: The question involves concept of titration. It involves reaction of citric acid with Sodium…

Q: The concentration of SO42–(aq) in a sample of river water can be determined using a precipitation…

A: Given,Volume = 6.0 mlConcentration of Ba2+ = 0.00100 M

Q: The amount of I7(aq) in a solution can be determined by titration with a solution containing a known…

A: The given net ionic equation is : The volume of Na2S2O3 = 29.3 mL The molarity of Na2S2O3 = 0.310 M…

Q: The molarity of an aqueous solution of sodium hydroxide, NaOH, is determined by titration against a…

A: In the given question we have to calculate the molarity of sodium hydroxide (NaOH) Solution by…

Q: The molarity of an aqueous solution of potassium hydroxide, KOH, is determined by titration against…

A: Balanced chemical equation: HBr + KOH ----> KBr + H2O Number of mmole of KOH = number of…

Q: The molarity of an aqueous solution of perchloric acid, HC104, is determined by titration with a…

A: The balanced reaction taking place is given as, => 2 HClO4 + Ba(OH)2 -------> Ba(ClO4)2 + 2…

Q: An aqueous solution of sodium hydroxide is standardized by titration with a 0.109 M solution of…

Q: Assume that the red spheres in the buret represent H3O+ ions, the blue spheres in the flask…

A: Applying formula M1V1= M2V2

Q: Suppose you had titrated with barium hydroxide instead of sodium hydroxide: What volume (in mL) of…

A: Data given Volume of Ba(OH)2(V1) = ? Molarity of Ba (OH)2 (M1) =0.586M Volume of sample vinegar (V2)…

Q: The data ( Concentration HCl =0.35 M, Volume HCl=24.35 mL, Volume NaOH=36.44 mL) refers to a…

A: Given Concentration HCl =0.35 M Volume HCl=24.35 mL Volume NaOH=36.44 mL

Q: The amount of (aq) in a solution can be determined by titration with a solution containing a known…

A: 1) As the balanced chemical equation shows, 2 moles of requires 1 mole of ions. Thus, 1 mole of…

Q: A solution is prepared by dissolving 0.400 g of an unknown monoprotic acid in 50.0 mL of solution.…

Q: Complete and balance the following neutralization reaction, name the products, and write the net…

Q: The following chemical reaction takes place in aqueous solution: FeSO,(aq)+2 NAOH(aq)…

A: Given The given ionic compounds are NaOH and FeSO4.

Q: 2. The end point in a titration of a 50.00 mL sample of HCl solution was reached by the addition of…

A: Given data: The volume of HCl sample VHCl=50.00 mL. The volume of NaOH VNaOH=35.23 mL. The molarity…

Q: The following chemical reaction takes place in aqueous solution: MgCl,(aq)+2 KOH(aq)→Mg(OH),(s)+2…

A: Ans Molecular chemical equation for MgCl2aq + 2KOHaq ---------> Mg(OH)2s + 2KClaq Total ionic…

Q: A student titrates 22.00 mL of an unknown HCI solution with 27.00 mL of a 0.5090 M Ca(OH)2 solution.…

A: Neutralization :- The reaction of an acid with base to form salt and water is known as…

Q: A student titrates 0.6769 grams of an unknown acid to the equivalence point with 23.70 mL of 0.1034…

A: Assuming the acid given is mono-protic hence the moles of acid present = moles of NaOH required…

Q: If you used no antacid tablet in your titration, you would be titrating 25.00 mL of 0.500 M HCl with…

A: For neutralize mole of acid = mole of base

Question

By titration, it is found that 70.1 mL of 0.161 M NAOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
concentration of the HCl solution.
[HCI] =
M
Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books

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 with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
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.
A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.150 M NaOH. What was the pH of the solution when the equivalence point was reached?
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.