al ExamHide Timern 1717 ofPart AA 18.9 mL aliquot of 0.178 M H3PO,(aq) is to be titrated with 0.305 M NaOH(ag). What volume (mL) of base will it take to reach the equivalence point?

Volume of H3PO4 = 18.9mL = 18.9*10-3L Molarity of H3PO4 = 0.178M Molarity of NaOH = 0.305M H3PO4 +…

Answered: Part A A 18.9 mL aliquot of 0.178 M…

Part A A 18.9 mL aliquot of 0.178 M H,PO, (aq) is to be titrated with 0.305 M NAOH(aq). What volume (mL) of base will it take 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: 1. Consider the titration of 25.00 mL of 0.150 M acetic acid (HC2H3O2, Ka = 1.8 × 10−5 ) (aq) with…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: When a 20.3 mL sample of a 0.386 M aqueous acetic acid solution is titrated with a 0.472 M aqueous…

A: pH of the solution :- pH is the quantitative measure of the acidity or basicity of aqueous or…

Q: If 50.0 mL of 0.250 M Sn(NO3)2 is added to 100.0 mL of 0.300 M Nal What is the concentration of Sn2+…

A: We have to calculate the concentration of Sn2+ in final solution mixture.

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 student was performing this experiment with an antacid tablet which contained C a CO3 but forgot…

A: Antacid tablets are used to reduce the acidity in the stomach and are made up of alkaline…

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: What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL…

A: In the given problem, a titration between H2SO4 and Ba(OH)2 is discussed. Both H2SO4 and Ba(OH)2 are…

Q: Molarity of the standard solution of soc hydroxide Volumes of NAOH(aq): First Rough titration Second…

A: Given : Rought First Second…

Q: A 44.8 mL sample of a 0.543 M aqueous acetic acid solution is titrated with a 0.436 M aqueous barium…

Q: The end point in a titration of a (1.710x10^-2)-L sample of aqueous H₂SO4 (a diprotic acid) was…

A: mol = concentration * volume / 1000mol of NaOH = (1.3400*10^(-1) * 3.37*10^1)/1000 =0.0045158…

Q: Calculate the pH of the resulting solution if 27.0 mL of 0.270 M HCl(aq) is added to 32.0 mL of…

Q: A 250.0 mL sample of 0.328 M HOCl(aq) (Ka = 2.9 x 10−8) is titrated with 0.457 M NaOH(aq). How many…

Q: In a titration, 10.543 mL of a 1.112 M weak acid solution are placed in a 125 mL Erlenmeyer flask. A…

A: Suppose the weak acid is HA. The reaction of the titration is HA (aq) + NaOH(aq) →NaA(aq) + H2O(l)

Q: Talk about the indicator in titration involving iodine. Comment on it's chemistry, how much of it is…

A: The indicator used in titration involving Iodine is STARCH.

Q: Solid lead nitrate is slowly added to 125 mL of a 0.0323 M ammonium sulfate solution. The…

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: Calculate the pH during the titration of 20.0 mL of 0.30 M HNO3(aq) with 0.30 M KOH after 19.24 mL…

A: Given Volume of HNO3 ( V1 ) = 20 mL Molarity of HNO3 ( M1 ) = 0.30 M Molarity of KOH ( M2 )…

Q: A 32.4 mL sample of a 0.432 M aqueous hydrofluoric acid solution is titrated with a 0.399 M aqueous…

Q: A 36.6 mL sample of a 0.401 M aqueous hypochlorous acid solution is titrated with a 0.456 M aqueous…

Q: A stainless steel alloy is to be analyzed for its chromium content. A 3.50 g sample of the steel is…

A: Mass of steel alloy = 3.50 gVolume of Cr2O72- solution = 250 mLMass of BaCrO4 = 0.145 g Percent by…

Q: A 37.0 mL sample of a 0.430 M aqueous acetic acid solution is titrated with a 0.458 M aqueous…

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

Q: In an experiment on evaluation of antacid containing magnesium carbonate, a tablet weighing 2.50 g…

A: Given, mass of tablet = 2.50 g molarity of HCl = 1.00 M volume of HCl = 5.00…

Q: NH3 + H3O* → NH; + H2O A 25.0 mL sample of the 0.0220 M NH3 was placed in a flask and titrated to…

A: HBr is a monoprotic strong base and NH3 is also a monoacidic weak base. The balanced neutralization…

Q: Solid silver fluoride is slowly added to 50.0 mL of a 0.252 M sodium sulfide solution until the…

Q: A solution is made by dissolving 33.5 g of Ba(NO₂)2 in 500.0 mL of water. Does Ba²+ have any acidic…

A: The reaction for the dissolution of Ba(NO2)2 in water can be written as Ba(NO2)2 + H2O → Ba(OH)2…

Q: A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCI and 2 drops of…

Q: A 44.7 mL sample of a 0.403 M aqueous nitrous acid solution is titrated with a 0.212 M aqueous…

A: Given data :

Q: A 46.9 mL sample of a 0.347 M aqueous acetic acid solution is titrated with a 0.494 M aqueous…

Q: A 0.328 g sample of an unknown monoprotic acid, HA, is dissolved in water and titrated with a…

Q: Determine the volume in mL of 0.251 M HBr(aq) needed to reach the equivalence (stoichiometric) point…

A: Given information, Molarity of HBr = 0.251 M Volume of (CH3)2NH = 25.92 mL Molarity of (CH3)2NH =…

Q: Determine the pH at the equivalence point of a titration of 100.0 mL of 0.265 M CH₂NH₂ solution with…

A: Answer: Conjugate acid of weak base gets hydrolyzed in water and produces H3O+ ion and as CH3NH2 is…

Q: Solid sodium bromide is slowly added to 175 mL of a 0.0318 M silver acetate solution. The…

A: Given data,Molarity of CH3COOAg=0.0318MVolume of CH3COOAg=175mL

Q: 35.8 mL sample of a 0.321 M aqueous acetic acid solution is titrated with a 0.408 M aqueous…

Q: Solid potassium hydroxide is slowly added to 150 mL of a 0.0538 M iron(II) acetate solution. The…

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: A 21.3 mL sample of a 0.387 M aqueous nitrous acid solution is titrated with a 0.333 M aqueous…

A: The pH of a solution is defined as the negative logarithm to the base 10 of the value of the…

Q: A 25.0 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.105 M NaOH (aq). It took…

Q: A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown…

A: Three questions based on pH titration, which are to be accomplished.

Q: A sample of 25.0 mL of buffer solution contains 0.100 M fluoride ions and 0.126 M hydrofluoric acid.…

A: 25.0 mL of buffer solution0.100 M fluoride ions0.126 M HF4.93 mL of 0.0100 M HCl is added to the…

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

al Exam
Hide Timer
n 17
17 of
Part A
A 18.9 mL aliquot of 0.178 M H3PO,(aq) is to be titrated with 0.305 M NaOH(ag). What volume (mL) of base will it take to reach the equivalence point?

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 Given

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

A 0.434 g sample of a monoprotic acid is dissolved in water and titrated with 0.170 M KOH. What is the molar mass of the acid if 18.5 mL of the KOH solution is required to neutralize the sample? molar mass: g/mol 19 || ||| |
The molar solubility of barium phosphate in a 0.102 M barium nitrate solution is М.
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)?
Solid lead acetate is slowly added to 125 mL of a 0.0470 M ammonium bromide solution. The concentration of lead ion required to just initiate precipitation is M.
4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of potassium hydrogen phthalate (C8H5O4K, M = 204.22 g/mol). In the titration 34.67 mL of NaOH solution is required to react with 0.1082 g C8H5O4K to reach the equivalence point. a) Calculate the concentration of the sodium hydroxide solution. Potassium hydrogen Phthalate = 0-10829, Molar mass of KMP=204-22 Hales of KMP = Mass 0.10829 g/mol Mm 6.000529 mal 204229/Mal Concentration of NaOH = Males = = of volume of Naot (L) = 0-000529 mal 34-67 mе onl ها NaOH (mal) = 0.000015258 mal/L 0.015M b) This solution of sodium hydroxide is used for another titration. A sample of 10.0 mL of HCI is neutralized using 22.1 mL of sodium hydroxide solution. Calculate the concentration of the HCI solution. sodium hydroxide 222.1 ml, Nal100
A 0.396 g sample of KHPKHP will be titrated with a NaOHNaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.
1. Calculate the concentrations of the major species present in a buffer solution prepared by adding 1.40 g of NaOH to: 140 mL of 0.750M NH4Cl(aq).
Solid sodium chromate is slowly added to 150 mL of a 0.0675 M lead nitrate solution. The concentration of chromate ion required to just initiate precipitation is M.
Solid ammonium fluoride is slowly added to 175 mL of a 0.0682 M lead nitrate solution. The concentration of fluoride ion required to just initiate precipitation is M.
A 15.00 mL solution of phosphoric acid (H;PO,) is titrated with 11.20 mL of 0.155M sodium hydroxide. What is the concentration of the acid?
A student added 1.78g of Ca(OH)2(9) to 0.250 L of 0.200 molL-1 HNO3(aq)- The mixture was carefully stirred until no further reaction occurred. Assuming that the total volume of the solution remains unchanged, calculate the pH of the resulting solution.
Arsenic in a 1.22 g sample of a pesticide was converted to AsO4^3- by chemical treatment. The ion was then titrated using Ag+ to form Ag3AsO4 as a precipitate. If 25 mL of 0.102 M Ag+ were required to reach the equivalence point in this titration.Calculate the percentage by mass of arsenic in the pesticide.