1. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid,H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is theconcentration of the phosphoric acid solution using the results that were obtained? KGiven: H₂PO4(aq) + 3NaOH(aq) -Na3PO4(aq) + 3H₂O(1)Initial BuretReading (mL)Final BuretReading (mL)Volume BaseAdded (mL)2 =>Na MgRb Sr2.92 MCs Ba0.55 M1.21 MBe0.97 M1.76 MCa Sc3.11 MRaLa91AMHfAcTrial 10.314.2TIZr Nb Mo Tc[81$4Cr Mn FeRe OsRf Db Sg Bh HsPeriodic Table of the ElementsTTrial 214.2ABasicD30.0Symbol1077 78224,Co Ni Cu Zn GaB14NebleGasTrial 330.043.9Ru Rh Pd Ag Cd In Sn Sb TeMс NExpe201VIASmNd PmEu GdDy Ho"Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr15VIAMHeGe As Se Br KrXePt Au HgDs Rg Cn Uut FI Uup Lv Uus UuoNe"Er Tm Yb

Answered: Image /qna-images/answer/a5d8df0b-3ab1-4fc0-a968-f127db9ec241.jpg

1. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid, H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is the concentration of the phosphoric acid solution using the results that were obtained? K Given: H₂PO4(aq) + 3NaOH(aq) - Na3PO4(aq) + 3H₂O(1)

1. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid, H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is the concentration of the phosphoric acid solution using the results that were obtained? K Given: H₂PO4(aq) + 3NaOH(aq) - Na3PO4(aq) + 3H₂O(1)

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

Similar questions

For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. A. One simple way to measure the [H+] is to measure pH. If a 10.0mL solution of “acid rain” is measured to have a pH=2.77, what is the concentration of strong acid, HNO3, formed? Hint: pH=-log[H+] and 10–pH= [H+], where [H+] is in molarity units.
A sample of acetic acid is titrated with a standardized NAOH solution. Before the end-point of the titration, which of the following must be true? HC,H3O, (aq) + NAOH (aq) → NaC,H3O2 (aq) + H2O (1) Note: [X] = molar concenctration of X %3D O [H+] > [OH-] [-HO] > [+H] O %3D [-HO] = [+H] O
If 100.0 mL of 0.250 M HBr is titrated with 0.150 M KOH answer the following questions. What is the pH of the solution before the titration begins? How many milliliters of NaOH must be added to reach the equivalence point? HBr (aq) + KOH (aq)  KBr (aq) + H2O (l) What is the pH of the solution at the equivalence point? What is the pH of the solution when 30.0 mL of KOH has been added? What is the pH of the solution when 180.0 mL of KOH has been added?
A 2.00 L solution contains 0.545 M NH3 and 0.641 M NH4A. (The Kb of NH3 is 1.86⋅10−51.86⋅10-5). What is the pH of this solution? What is the pH of this solution after 0.121 mol of HCl are added to the solution? What is the pH of this solution after 0.242 mol of HCl are added to the solution?
2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium acetate (CH3COONa) together in a beaker: a. The Ka of acetic acid is 1.8 x 105. What is the pH of the solution that you made? What is the degree of ionization? CH&COOH+ CHeCOONat lOH 4 g CH300H
11
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.14 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. During the titration the following reaction occurs HA + NaOH ⇒ NaA + H2OWhat is the concentration of A- (the conjugate base of the weak acid) at the equivalence point? ml NaOH added pH Hal-way point 18.71 3.41 Equivalence point 37.41 8.53
Can you help me answer the PH=
100.0 mL of HCI required 25.00 mL of 0.2000 M Mg(OH)2 to reach pH 7. What is the concentration of the HCI ? 2 HCI + Mg(OH)₂ MgCl₂ + 2 H₂O The neutralization equation is There is enough information to calculate the moles of Mg(OH)2 ( L Mg(OH)₂ (- concentration = Then use stoichiometry to convert moles of Mg(OH)₂ into moles of HCI mol HCI a. acid i. 0.2000 p. 0.01000 mol Mg(OH)₂ (- b. base c. HCI d. NaOH mol Mg(OH)2 We now can calculate the concentration of HCI since we have both the moles of HCI and the volume of HCI j. 1.000 k. 0.005000 q. 0.001000 1 L mol HCI LHCI r. 58.31 = mol Mg(OH)2 e. NaCl I. 100.0 f. H₂O m. 0.1000 s. 5.831 = g. 25.00 mol/L n. 0.05000 h. 0.02500 mol Mg(OH)2 o. 2.000 mol HCI
An analytical chemist is titrating 143.6 mL of a 0.7000M solution of piperidine (C,H10NH) with a 0.4000M solution of HNO3. The p K, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 267.7 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH
ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 7.00 ✕ 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M Na+ M H3O+ M OH- M C6H5CO2-
20. mL of 0.250 M NH3 is titrated with 0.500 M of HCl solution, what is the pH of the resulting solution when 0mL, 5.0 mL, 10.0 mL and 12 mL of HCl was added into the NH3solution? KB(NH3) = 1.8 x 10-5