6. Both CO3 and HCO3 respond to the usual carbonate ion test. Give specificprocedures by which you could distinguish between these ions in an unknown. (Hint:Consider the pH of the solution.)2-

The carbonic acid has a tendency to exist in the three forms in a solution. The equilibrium shown by…

Answered: 6. Both CO3 and HCO3 respond to the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 7P

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The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Why is (CH3)3Cl considered to be a Lewis Acid?
1. Solid NH4NO3 dissolves in water and then reacts with KOH (aq). The container releases a smell as the reaction proceeds. (a) Write the acid-base reaction products for this reaction. (b) Write the decomposition reaction that happens immediately after the acid-base reaction that is responsible for the smell observed. 2. Write the complete and balanced Bronsted- Lowry acid-base reaction for the following. Choose the correct arrows to indicate if the reaction goes 100% to completion or is a reversible reaction using equilibrium arrows. (a) H₂S(aq) + NH4OH(aq) (b) HC₂H3O2(aq) + Ca(OH)2 (aq) 3. Use dimensional analysis, proper significant figures & show units. A nicotine-like compound found in tobacco has an empirical formula of C5H7O1 and a molar mass of 160 g/mol. What is the molecular formula of this compound?
Calculate the pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present. The pKb of ammonia solution is 4.75.
When 1.40 moles of Br2 are put in a 0.960−L flask, 1.10 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.
What is the equilibrium constant value for NaC2H3O2 and how do you find its Kb?
A buffer solution is 0.402 M in NaH2PO4 and 0.318 M in Na2HPO4. If Ka for H2PO4- is 6.2 x 10 -8, what is the pH of this buffer solution?
1.) Calculate the pH of a solution that is 1.00 M HCN and 1.00 M HF. Compare the concentration (in molarity) of the CN- ion in this solution with that in a 1.00 M HCN solution. Comment on the difference. 2.) A 1.292-g sample of a metal carbonate (MCO3) is reacted with 500 mL of a 0.100 M HCl solution. The excess HCl acid is then neutralized by 32.80 mL of 0.588 M NaOH. Identify M.
Please write the balanced chemical equations on the observations of heating NaHCO3 and bubbling the gas made by decomposition through the Ca(OH)2 solution in the presence of bromothymol (blue acid base indicator solution) Please write out in chemical equation form!
Write the basic equilibrium equation for C₄H₃N₂O₃⁻. Be sure to include the proper phases for all species within the reaction.
Predict the products of each reaction, and whether the solution at equilibrium will be acidic, basic, or neutral. At equilibrium the solution is...? reaction acidic N,0,(s) + 3H,0(1) → 0 basic neutral O acidic co, (g) + H,0(1) basic neutral acidic Na, 0 (s) + H,0(1) - 0 basic neutral

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6. Both CO3 and HCO3 respond to the usual carbonate ion test. Give specific procedures by which you could distinguish between these ions in an unknown. (Hint: Consider the pH of the solution.) 2-