MaVa=MbVb A 15.0 mL sample of HCI (acid) required 28.0 mL of 0.25 M NaOH (base) toreach the equivalence point. What is the concentration (molarity) of the HcIa

Given, volume of HCl (acid) (Va) = 15.0 mL. Volume of NaOH (base) (Vb) = 28.0 mL. Concentration of…

Answered: A 15.0 mL sample of HCI (acid) required…

A 15.0 mL sample of HCI (acid) required 28.0 mL of 0.25 M NaOH (base) to reach the egyiyalence point. What is the concentration (molarity) of the HCI

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 38QRT: It took 12.4 mL of 0.205-M H2SO4 solution to titrate 20.0 mL of a sodium hydroxide solution to the...

See similar textbooks

Related questions

Q: A 0.350 g sample of a diprotic acid is dissolved in water and titrated with 0.320 M NaOH. What is…

A: Solution : Titration is a method for the determination of the equivalence point. At the…

Q: 4. The titration of 10.00 mL of a diprotic acid solution of unknown concentration requires 21.37 mL…

A: Acid-base titration: Titration is a method to determine the concentration of unknown acid by using…

Q: By titration, it is found that 24.7 mL of 0.184 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: The reaction of HCl with NaOH is a neutralization reaction that forms NaCl and water as the…

Q: A 25 ml solution of 0.5 M NaOH is titrated until neutralized into a 50 ml sample of HCI. What was…

A: Given volume of NaOH is 25 mL and strength is 0.5 M. Given volume of HCl is 50 mL. Recall the…

Q: If 10.0 mL of hydrochloric acid is titrated by 16.4 mL of NaOH that has a concentration of 1.7 M,…

Q: How many milliliters of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of…

A: Concentration of NaOH = 0.100 M Concentration of acetic acid = 0.150 M Volume of acetic…

Q: By titration, it is found that 51.5 mL of 0.183 M NaOH(aq) is needed to neutralize 25.0 mL of…

Q: What volume, in mL, of 1.78 M LiOH(aq) is needed to COMPLETELY NEUTRALIZE 125. mL of 1.38M H2C2O4…

Q: By titration, it is found that 73.9 mL of 0.190 M NAOH(aq) is needed to neutralize 25.0 mL of…

A: Given :- concentration of NaOH = 0.190 M Volume of NaOH solution = 73.9 mL…

Q: Which one of the following can be classified as a weak electrolyte? A) HBr B) CaF, C) OBr, D) HF E)…

A: The explanation is given below-

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: By titration, it is found that 13.5 mL of 0.112 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Since the reaction taking place is given by NaOH + HCl ----> NaCl + H2O Hence we can say that 1…

Q: A 0.548 g sample of a diprotic acid is dissolved in water and titrated with 0.320 M NaOH. What is…

Q: A 0.347 g sample of a diprotic acid is dissolved in water and titrated with 0.170 M NaOH. What is…

A: Given, Molarity of NaOH solution = 0.170 M = 0.170 mol/L Note: 1000 mL = 1 L Volume of NaOH solution…

Q: 6) If 11.3 ml of 0.110 M HCI is required to neutralize 25.00 mL of a barium hydroxide solution, what…

Q: The titration of 25.00 mL of a sulphuric acid solution of an unknown concentration requires 31.22 mL…

A: The reaction in which an acid and a base react to produce salt and water is called as…

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

A: The complete balanced Chemical Reaction is - NaHC2O4 + NaOH ----> Na3C2O4 + H2O Thus, one mole of…

Q: By titration, it is found that 63.7 mL of 0.184 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Given, 63.7 mL of 0.184 M NaOH 25.0 mL of HCl

Q: Calculate the concentration of all ions present in 56.5 mg NH4B in 500.0 mL of solution. MNH4 MBr…

A: Given that 56.5 mg of NH4Br is present in 500.0 mL of a solution. We have to find the concentration…

Q: 25.0 mL of 0.212 M NaOH is neutralized by 26.7 mL of an HCl solution. The molarity of the HCl…

A: Given -> Volume of NaOH(V1) = 25.0 ml = 0.025 L Molarity of NaOH(M1) = 0.212 M Volume of HCl (V2)…

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

A: Acid reacts with base to form salt and water. This reaction is known as neutralization reaction.

Q: A 50.0ml sample of HCl required 25.81 mL of 0.1250 M KOH for neutralization. what is the molarity of…

A: The balanced reaction of HCl and KOH is as follows: Calculation of no. of mol of KOH:

Q: Calculate the molar concentration of the acid if 35.18mL of hydrochloride acid was required to…

A: Given: Mass of lithium hydroxide i.e. LiOH used = 0.376 g. And volume of HCl acid required = 35.18 m…

Q: Determination Of The Acid Conent In Vinegar -How would the concentration of the vinegar solution…

A: Please find your solution below : The acid content in vinegar can be easily determined by titrating…

Q: A 50 mL solution of NaOH was titrated with 39.7 mL of 0.9781 M HCl. What is the concentration of the…

Q: A 45.15 mL sample of phosphoric acid required 215mL of 1.000 M sodium hydroxide to reach the…

A: A balanced molecular equation is one in which the ionic reactions are represented as neutral…

Q: What is the purpose of a titration? How is it performed (in general)?

Q: A 0.760 g sample of a diprotic acid is dissolved in water and titrated with M NaOH.0.260 M NaOH.…

A: Assuming the diprotic acid has formula H2A hence the reaction will be H2A + 2 NaOH ----> 2 NaA +…

Q: By titration, it is found that 55.5 mL of 0.116 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: HCl(aq) + NaOH (aq) ------> NaCl (aq) + H2O (l) Number of moles of HCl = Number of…

Q: . If 0.2500 g sample of an unknown triprotic acid is neutralized by 14.2 mL of 0.187 M strontium…

A: To neutralize a substance, the number of moles of acid should be equal to number of moles of base.…

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

Q: How many mL of the standard AgNO3 solution were used in the titration?

A: Solution: We have filled standard AgNO3 solution in burette and used for titration. In the given…

Q: A 0.229 g sample of impure NaOH requires 16.0 mL of 0.2050 M HCl for neutralization. What is the…

Q: Determining the % Citric Acid (H3C6H5O7) in Lemon Juice Balanced neutralization reaction:…

A: The density of lemon juice can be determined as follows: Density of lemon juice = Mass of lemon…

Q: By titration, it is found that 63.5 mL of 0.104 M NaOH(aq) is needed to neutralize 25.0 mL of…

Q: What volume (L) of water would need to be added to 50.00 mL of 6.25 x 10-2 M aluminum hydroxide…

A: We have to calculate the volume of water as well as mass of aluminium hydroxide .

Q: By titration, it is found that 39.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Balanced chemical equation: NaOH + HCl -----> NaCl + H2O Number of mmoles of NaOH = Number…

Q: A 50.00-mL sample of a citrus drink requires 17.62 mL of 0.04166 M NaOH to reach the phenolphthalein…

Q: What volume (in mL) of the following acid would be required for complete neutralization of 50.00mL…

A: The volume (in mL) of the following acid that would be required for complete neutralization of…

Q: 1. In a titration, a 20 ml sample of 0.3 N HCI is neutralized with 55 ml of NaOH. a) Write the…

A: "Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: In an experiment, 20.11 mL of 0.102 M LIOH is required to complete neutralize a 12.36 mL of…

A: To solve this problem we first calculate the number of mile of LiOH from its molarity and volume…

Q: 25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl…

Q: A 0.658 g sample of a diprotic acid is dissolved in water and titrated with 0.130 M NaOH. What is…

A: First find number of moles of NaOH. Then with the help of balanced equation find the number of moles…

Q: By titration, it is found that 96.5 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Given information:Volume of NaOH (V1)= 96.5 mLVolume of HCl (V2)= 25.0 mLMolarity of NaOH (M1)=…

Q: What volume (in mL) of the following acid would be required for complete neutralization of 50.00mL…

A: The neutralization reaction is given below.

Q: What volume of 0.150M HNO3 solution is needed to exactly neutralize 35.0mL of 0.150M NaOH solution?…

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

Q: give an example of neutralisation reaction.

A: Neutralization reaction is a reaction of an acid with a base to produce a salt and…

Q: By titration, it is found that 37.3 mL of 0.182 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Neutralisation Reaction : When an acid and a base reacts together to form salt and water as…

Q: By titration it is found that 76.7 mL of .151 M NaOH(aq) is needed to neutralize 25.0mL. Calculate…

A: Given information: The volume of HCl is 25.0mL The concentration of NaOH is 0.151 M The volume of…

Q: In a titration, 25.0 mL of NaOH is completely neutralized by 15.0 mL of 0.500 M HCl. What is the…

A: We should know the balanced reaction for titration for predicting equivalence point. We have given…

Concept explainers

Micelles and Biological Membrane

Micelles are the type of lipid molecules that organize themselves in spherical shape in aqueous solutions. The production of the micelle is a reply to the amphipathic behavior of fatty acids. It means that they consist of both hydrophobic regions and hydrophilic regions. In micelles, polar head groups (hydrophilic groups) produce an outer layer associated with water whereas nonpolar tails (hydrophobic groups) are organized in the interior.

Question

MaVa=MbVb

A 15.0 mL sample of HCI (acid) required 28.0 mL of 0.25 M NaOH (base) to
reach the equivalence point. What is the concentration (molarity) of the HcIa

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

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

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.
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
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 solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
It took 12.4 mL of 0.205-M H2SO4 solution to titrate 20.0 mL of a sodium hydroxide solution to the equivalence point. Calculate the molarity of the original NaOH solution.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
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?
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
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?
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 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.