Phosphorous acid, H,PO, (aq), is a diprotic oxyacid that is animportant compound in industry and agriculture.pKalpKa2но--P-O-1.306.70Calculate the pH for each of the points in the titration ofH.50.0 mL of 2.4 M H, PO, (aq) with 2.4 M KOH(aq).before addition ofanyКОН:after addition of 25.0 mL KOH:after addition of 50.0 mL KOH:after addition of 75.0 mL KOH:after addition of 100.0 mL KOH:

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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...

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The acid HX has a pKa of 5.00. If 25.00 mL of a 0.106 M solution of HX are titrated with 0.100 M NaOH solution, what's the pH after 11.28 mL ofbase solution is added?
The following titration curve shows the titration of triethylamine (C2H5]3N with hydrochloric acid. Which net ionic reaction explains the pH of the solution after 60 mL of titrant is added? 12 10 PH 50 mL of HCI 10 30 70 90 110 O H,O(1) --> H*(aq) + OH (aq) (C,H5)3N(aq) + H*(aq) --> (C,H5)3NH* (aq) (C,H5)3N(aq) + H3O*(aq) (C,H5)3NH*(aq) + OH (aq) (C,H5)3NH (aq) + H2O(1) (C,H5)3N(aq) + H3O*(aq) (C2H5)3N(aq) + H20(1) OH (aq) + (C2H5)3NH*(aq) O O O O O
What is the pH at 25°C of a solution that results from mixing equal volumes of a 0.0500 M solution of acetic acid and a 0.0400 M solution of sodium hydroxide? The pKa of acetic acid is 4.74.
The titration of CH3COOH (Ka = 1.76x10-4; pKa = 3.754; Kb = 5.68x10-11) with NaOH is an example of a weak acid/strong base titration. A 40 mL aliquot of a 0.060 M solution of HCOOH is titrated by 0.060 M KOH. What is the pH of the solution at each of the following points: a) initially b) after 1 mL of base has been added c) after 20 mL of base has been added d) at the equivalence point e) after 45 mL of bases has been added
Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid. The Kb for hydrazine is 3.00x10-6. H2NNH2(aq) +HNO3(aq) ⟶ [H2NNH3]+1(aq) + NO3-1(aq) 1. 4.80 2. 9.60 3. 4.70 4. 9.39 5. 3.22 6. 3.32
You need to prepare an acetate buffer of pH 5.455.45 from a 0.843 M0.843 M acetic acid solution and a 2.06 M KOH2.06 M KOH solution. If you have 630 mL630 mL of the acetic acid solution, how many milliliters of the KOHKOH solution do you need to add to make a buffer of pH 5.455.45? The p?apKa of acetic acid is 4.76.4.76. Be sure to use appropriate significant figures. mL
You have 25.00 mL of a solution containing 0.1125 M benzoic acid (pKa = 4.20) in a flask that you titrate with 0.2250 M NaOH to a Phenolphthalein endpoint. What is the pH after the following additions of NaOH: a) 12.5 mL of NaOH b) 6.25 mL NaOH c) 15 mL NaOH
Consider the following reaction:CH3COOH(aq)+OH−(aq)CH3COO−(aq)+H2O(l) pKa: 4.75 How much 5.60 M NaOH must be added to 420.0 mL of a buffer that is 0.0205 M acetic acid and 0.0260 M sodium acetate to raise the pH to 5.75?
the pKb values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.36. calculate the pH at all points in the titration of 50 mL of a .55 M B solution with 55 M HCI: before the addition of HCl, after the additon of 25 mL HCI, after addition of 50 mL HCl, after addition of 75 mL HCl, after addition of 75 mL HCl, after addition of 100 mL HCl
In the titration of 25.0 mL of 0.1 M F− (where the solution was made using NaF(aq)) with 0.1 M HCl, how is the pH calculated after 12.5 mL of titrant is added? Group of answer choices The pH is based on the concentration of protons present in the solution, which is equal to the original concentration of the acid. The pH is equal to the pKa of the conjugate acid. The pH is 7. The pH is calculated by determining the concentration of weak base present in the solution, using an ICE table to calculate the hydroxide ion concentration present after hydrolysis, subtracting pOH from 14, and taking the negative log of the result. The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is 1. The pH is 14. The pH is calculated by determining the concentration of protons left in the solution after neutralization, and taking the negative log of the result.
An analytical chemist is titrating 70.8mL of a 0.7400M solution of butanoic acid HC3H7CO2 with a 1.100M solution of KOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 55.5mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
If 26.6 mL of 0.108 M acid with a pKa 4.65 is titrated with 0.101 M NaOH solution, what is the pH of the acid solution before any base solution is added?

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