Determine the [SO, 2] in the Na₂SO, solution which you prepared. Using thatinitial concentration and the measured pH value, determine the K, value forSO, and the K, value for the HSO,. Compare your K, value to the acceptedvalue for HSO, which is 6.2 x 10" M and comment on the agreement.-1 Data Table II: HydrolysisRecord the actual mass of each of the following solutes:1-159Ammonium chloride, NH4Cl1-1.59Sodium carbonate, Na2CO3Zinc nitrate, Zn(NO3)2. 6H2OAluminum nitrate, Al(NO3)3. 9H₂OSodium sulfite, Na2SO31-1.521.2991.10 g(skip)(skip)1.43 99.Record the pH of the above solutions and the prepared ammonium acetate and sodium hydrogenphosphate solutions to the nearest 0.01 pH units:pH of Ammonium chloride, NH4Cl solutionSodium carbonate, Na2CO3Zinc nitrate, Zn(NO3)2. 6H2OAluminum nitrate, Al(NO3)3. 9H₂OSodium sulfite, Na2SO3pH of Ammonium acetate solutionpH of sodium hydrogen phosphate solution7.10 PH12.110 раPH(skip)(skip)9.00 PH5.16 PH(skip)

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Answered: Determine the [SO, 2] in the Na₂SO,…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 19QAP: . How is the strength of an acid related to the fact that a competition for protons exists in...

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. 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?
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?
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
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
you want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphidesfrom each other. What pH value must you set so that one of the twometals is precipitated quantitatively (concentration in the solution less than/equal to 10/-5 mol/l)is precipitated while the other is still in solution? Ksp (NiS): 10^-21, Kps (MnS): 10~15; Ks (H2S): 10 ~- 20,Saturation concentration of H2S in water: 0.1 mol/l
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Fr 17a.
Determine the pH during the titration of 67.0 ml of 0.375 M formic acid (K, - 1.8x10 4) by 0.375 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 17.0 ml of KOH (e) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 101 mL of KOH Submit Show Appresch Show Tutar e
E University Librarie. E UNIVERSITY POR. Student Detail Sc. Part A The table shows respective color change when a universal indicator is added to the clear solutions. Rank the samples based on increasing order of acid strength. Solutions Color change 0.001 M lactic Light red 0.01 M phenol Light yellow 0.01 M nitrous acid Light orange 0.001 M hydrogen peroxide Light green Rank the solutions by Increasing order of their acid strength. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help 0.01 Mnitrous acid 0.001 Mlactic acid 0.001 M hydrogen peroxide 0.01 Mphenol Least acidic Most acidic P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions | Contact Us | MacBook Air 80 888 DII DD F3 F4 F5 F6 F7 F8 F9 F10 F11 $ & 3 4 7 8. 9. { R Y U 一 F J K く C V B N M + I| .. .- エト
A buffer solution could be made by mixing equal amounts of citric acid and a solution containing. would resist When a small amount of strong acid or base is added, this buffer The statements above are completed by ཤ (-) (-C,H,O(C00), tay ila pH change (aq) i-C,H,O(COO), (aq) О -C,H,O(COOH),COO) О i-C,H,O(COOH),C00(a) it an equilibrium shift -a pH change -an equilibrium shift
17.
Use the References to access important values if needed for this question. A buffer solution is made that is 0.385 M in HNO, and 0.385 M in KNO,. If K, for HNO2 is 4.50 x 10, what is the pH of the buffer solution? 4. ted pH Write the net ionic equation for the reaction that occurs when 0.078 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H; O* instead of H) +.

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