Tutored Practice Problem 17.3.5COUNTS TOWARDS GRADECalculate the pH and concentration of species present in a polyprotic acid solution.For a 7.46×10-2 M solution of H2S, calculate both the pH and the S²- ion concentration.H2S+ H2O H30+ + HS Kal = 1.0×10-7HS + H2OH3O++ S2- Ka2 = 1.0×10-19Check & Submit AnswerShow ApproachpH =[S²-] =M

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Answered: Tutored Practice Problem 17.3.5 COUNTS…

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 107AP

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Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
. 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?
Addition of the indicator methyl orange to an unknownsolution leads to a yellow color. The addition of bromthymolblue to the same solution also leads to a yellow color.(a) Is the solution acidic, neutral, or basic? (b) What is therange (in whole numbers) of possible pH values for the solution?(c) Is there another indicator you could use to narrowthe range of possible pH values for the solution?
A solution of acetic acid CH3COOH, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.68, what was the initial concentration of the acid? Ka=1.7x10-5 Ethanolamine, HOC2H4NH2, is a viscous liquid with an ammonia-like odour used to remove hydrogen sulphide from natural gas. A 0.15 mol dm-3 aqueous solution of ethanolamine has a pH of 11.34. What is kb for ethanolamine? What is the concentration of hydroxide ion in a 0.060 mol dm-3 aqueous solution of methylamine, CH3NH2? What is the pH? Kb=4.4x10-4
A 20.00ml aliquot of a 0.75M solution of a weak acid at {:1.00x10^(-5) at 25deg C) is titrated with 0.500M NaOH. Determine the pH at the following volumes of NaOH: Volume NaOH = 17.50mL, pH = Ans = 5.15 Volume NaOH = 30.00mL, pH = ? Volume NaOH = 35.00mL, pH = ? Please help .
The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5. What will be the pH of a 0.10 M HC2H3O2 solution which is 0.10 M in NaC2H3O2
PR: (a) Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 800. mL of solution. (10). (b) Calculate the pH after 0.050 moles of NaOH are added to the buffer solution (assume no volume change) (10). Ka (HCNO) = 2.0 × 10-4
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
How many moles of B (weak base) would need to be added to 507 mL of 0.28 M BHCl (the acidic salt) to produce a solution with a pH equal to 9.05? Report your answer to the thousandths place. The Kb of the weak base (B) is 4.7 × 10-6 Please explain each step, i want to learn how to solve it myself!
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 2.733 g KH2PO4 and 4.508 g K2HPO4 in water to give 250. mL of solution. Stepwise acid dissociation constants for phosphoric acid may be found in your textbook. (b) a solution made by mixing 35.00 mL 0.24 M C6H5NH2 with 15.00 mL 0.19 M C6H5NH3Cl. The base dissociation constant Kb is 4.00 x 10^-10 for C6H5NH2. Assume that the final volume is the sum of the volumes of the two solutions that are mixed.
Why is pH at the equivalence point larger than 7 when youtitrate a weak acid with a strong base? (a) There is excessstrong base at the equivalence point. (b) There is excess weakacid at the equivalence point. (c) The conjugate base that isformed at the equivalence point is a strong base. (d) The conjugate base that is formed at the equivalencepoint reacts with water. (e) This statement is false: the pH isalways 7 at an equivalence point in a pH titration.
Select the statement below that is correct regarding the behavior of strong acids. O A strong acid and its sodium salt can be used to form a buffer solution. OA 1.0 M solution of a monoprotic strong acid will require twice as much 1.0 M NaOH to neutralize it as a 1.0 M solution of a monoprotic weak acid. Strong acids are acids with a solution concentration of > 3 M. O Strong acids ionize completely in solution.

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