21:56 1Question 21 of 30SubmitA solution of phosphoric acid (H3PO4) with a knownconcentration of 0.250M H;PO. is titrated with a 0.800M NAOH solution. How many ml of NaOH are required toreach the third equivalence point with a starting volume of72.0mL H3PO. , according to the following balancedchemical equation:НРО, +3NaOH > NaзРОд +3H20XSTARTING AMOUNTADD FACTORANSWERRESET*( )7.503222.50.25072.0167.5m10000.8000.00143.26.75 x 1040.0675Tap here or pull up for additional resources

At third equivalence point, all the H3PO4 molecule get converted to PO4-3 i.e complete…

Answered: A solution of phosphoric acid (H3PO4)…

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 16.58QE

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A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
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 buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
Th pH of blood is steady at a value of approximately 7.4 as aresult of the following equilibrium reactions:CO2(aq) 1 H2O(l) N H2CO3(aq) N HCO3–(aq) 1 H1(aq)The actual buffer system in blood is made up of H2CO3 andHCO3–. One way the body keeps the pH of blood at 7.4 is byregulating breathing. Under what blood pH conditions will thebody increase breathing and under what blood pH conditionswill the body decrease breathing? Explain.
Please complete the calculation of the pH of the equivalence point all numbers required are here Concentration of NaOH solution = 0.1 mol dm3. Mean titre (NaOH solution) = 17.95 cm³. Amount of NaOH = 0.00180 moles. Molar ratio of NaOH:aspirin = 1:1. Amount of aspirin = 0.00180 moles. Mass of aspirin (in titration) = 0.324 g. Mass of aspirin (per tablet) = 0.324 g. %3D
The pH of a Buffer containing 1.OM CH3COOH and 0.1M CH3COONA (pka of * :CH3COOH =4.74) is 3.0 4.74 3.74 5.74
How many grams of Na2HPO4*2H2O must be added to 400 mL of 0.200 M H3PO4 to give a buffer of pH 7.30?
Determine the pH during the titration of 62.0 mL of 0.342 M formic acid (K,- 1.8x104) by 0.342 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 93.0 mL of KOH

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