By titration, it is found that 14.7 mL of 0.190 M NAOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate theconcentration of the HCl solution.[HCI] =Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books

Answered: By titration, it is found that 14.7 mL…

By titration, it is found that 14.7 mL of 0.190 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] M

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: > Calculate the percent of acetic acid in a 20 mL vinegar sample. Titration was used, and it took…

A: Given data is Volume of the vinegar sample = 20 mL Volume of NaOH used in the titration= 35.19 mL…

Q: Question 1 what is the formation of the keytone compound Answer HO. R OH R H₂0 und? Is the answer…

Q: You dissolve 1.029 grams of an unknown triprotic acid in water. This solution is exactly neutralized…

A: Given, Molarity = 0.435 M Volume of Solution = 17.53 mL = 0.01753 L Mass of unknown acid = 1.029 g…

Q: An analytical chemist weighs out 0.203 g of an unknown diprotic acid into a 250 mL volumetric flask…

A: The point that appears in the titration curve, where the number of moles of an acid and the number…

Q: What volume in mL of 0.025 M HBr solution is to be required to titrations 125mL of a 0.049 M NaOH…

A: As per the reaction, NaOH(aq) + HBr(aq) -> NaBr(aq)+H2O(I) we can see that 1 mole of HBr is…

Q: A chemistry student weighs out 0.146 g of citric acid (H,C,H,O,), a triprotic acid, into a 250. mL…

Q: A 0.392 g sample of a monoprotic acid is dissolved in water and titrated with 0.120 M KOH. What is…

A: We have to calculate the molar mass of acid.

Q: A 25.0 mL volume of HCl solution of unknown concentration is titrated with a 0.154 M NaOH solution.…

Q: Calculate the molarity of a sodium hydroxide(NaOH) solution that is titrated with 0.6887 g of oxalic…

A: Given: The mass of oxalic acid taken = 0.6887 g The volume of NaOH solution required to reach the…

Q: Calculate the volume of 1 M CoCl2 needed to prepare 100 mL of 0.25 M CoCl2

A: Molarity of solution 2 (M2) = 0.25 Volume of solution 2 (V2) = 100 ml Molarity of solution 1 (M1)= 1…

Q: Solid ammonium carbonate is slowly added to 175 mL of a 0.0585 M lead nitrate solution. What is the…

Q: 0.644 g of wood bleach, which contains oxalic acid, H2C2O4, was placed in an Erlenmeyer flask. The…

A: The molar mass is the sum of the mass of each element. The molar mass of hydrogen, carbon, and…

Q: ydroiodic acid often is used to disinfect and sanitize medical tools and products. In an experiment,…

A: 1. the hydronium ion concentration of the resulting diluted solution = 0.15M 2. the pH of the…

Q: Consider the following: 50 mL of a 1.067 M solution of HCI was diluted to 250 mL. The diluted HCI…

A: 50 mL of a 1.067 M solution of HCl was diluted to 250 mL . 25.00 mL of these diluted HCl solution…

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: In a titration, suppose 20.00 mL of 0.275 M oxalic acid solution required 21.72 mL of NaOH solution…

A: H2C2O4(aq) + 2NaOH(aq) -------> Na2C2O4(aq) +2H2O(l)

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: 25 mL of acetic acid was titrated 0.1 M NaOH. The titration required approximately 20.00 mL of NaOH…

A: Given,molarity of NaOH = 0.1 MVolume of NaOH = 20.00 mLVolume of acetic acid = 25 mL

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

A: Given, Molarity of HCl = 40.0 mL Molarity of NaOH = 0.200 M Volume of NaOH=…

Q: Consider the titration of 100.0 mL of an unknown concentration of weak monoprotic acid with 0.550 M…

A: The volume of unknown weak monoprotic acid, V1 = 100.0 mLThe concentration of weak monoprotic acid,…

Q: Malonic acid, H2C3H2O4 (aq), is a diprotic acid, so 2 moles of hydroxide ions are required per mole…

A: A neutralization reaction can be described as a chemical reaction in which acid and base react…

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 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: An aqueous solution of Ca(OH)2with a concentration of 0.188 M was used to titrate 25.00 mL of…

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: Titration of a 20.00 mL sample of acid rain required 4.13 mL of 0.08424 M KOH to reach the end…

A: The given reaction is, H2SO4- + 2KOH -----> K2SO4 + 2H2O This means that 2 moles of KOH is…

Q: A 13.8 mL solution of 0.176 M phosphoric acid (aq) is to be titrated with 0.384 M sodium hydroxide…

A: The mathematical calculation can be explained using acidimetry and alkalimetry . From this principle…

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 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: A strong acid-strong base titration was performed as follows: 10.00 mL of 0.10M HCl were collected…

Q: By titration it is found that 35.7 mL of 0.101 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: The concentration of the HCl solution after neutralisation with sodium hydroxide is determined as,

Q: An analytical chemist weighs out 0.141 g of an unknown diprotic acid into a 250 mL volumetric flask…

A: Given, Mass of unknown diprotic acid = 0.141 g. Volume of flask = 250 mL Molarity of NaOH = 0.1100 M…

Q: 15. A NAOH(aq) solution and an acid-base indicator are used to determine the molarity of an HCI(ag)…

Q: If the concentration of the NaOH that was added was 1.0 M and the volume of oxalic acid being…

A: For NaOH, Molarity, M1 = 1.0 M = 1 mol L-1 Volume used, V1 = 29 mL = 29 x 10-3 L…

Q: mass of Iknowr

A: To solve the problem, we need to back calculate the moles of monoprotic acid from the titration…

Q: An analytical chemist weighs out 0.203 g of an unknown diprotic acid into a 250 mL volumetric flask…

A: l

Question

By titration, it is found that 14.7 mL of 0.190 M NAOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
concentration of the HCl solution.
[HCI] =
Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books

Expert Solution

Step 1

The neutralization reaction between NaOH and NaOH is as follows;

$NaOH + HCl \to NaCl + H_{2} O$

Consider the given information is as follows;

Volume of NaOH $(V_{1})$ = 14.7 mL

Concentration of NaOH $(M_{1})$ = 0.190 M

Volume of HCl $(V_{2})$ = 25.0 mL

Concentration of HCl $(M_{2})$ = ?

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

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
An unknown potassium hydroxide solution is titrated with a standardized solution of hydrochloric acid. It takes 37.4 mL of the base to reach the endpoint when reacting with 25.0 mL of 0.138 M HCl. What is the molarity of the KOH solution?
Constant-boiling HCI can be used as a primary standard for acid-base titrations. A 50.00 mL sample of constant-boiling HCI with a concentration of 0.1020 M was collected and titrated to an endpoint with 40.29 mL of a Ba(OH)₂ solution. What is the molarity of the Ba(OH)₂ solution? concentration: M
How many mL of 0.45 M HCl(aq) are needed to neutralize a 149 mL solution of 1 M Ba(OH)2?
A 50.0 mL solution of Mg(OH)2 of unknown concentration is titrated with 0.348 M HCI. The equivalence point (end point) is reached after 62.8 mL of HCI were dispensed into the Mg(OH)2 solution. What is the molarity concentration of the base?
An acid-base titration reaches its end point when iõð mlL of 8.2 M HCI Is ådded to 50 mL of NaOH. What is the concentration of the NaOH (M)?
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.
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
A student tries to determine experimentally the molar mass of aspirin (HAsp).She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is:HAsp(aq) + OH-(aq) ----> Asp-(aq) + H2O(l) What is the molar mass of aspirin?
presented by Macmillan Learning By titration, it is found that 37.3 mL of 0.182 M NaOH(aq) is needed to neutralize 25.0 mL of HCI(aq). Calculate the concentration of the HCl solution. [HCI] =