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?
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B represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an aqueous solution can be written as: B(ac) + H2O(l) <-> +BH(ac) + OH(ac) If B (ac) is yellow +BH is red. Using Le Châtelier's principle, predict the color of the indicator by adding a few drops of the indicator to an aqueous solution of HCl and an aqueous solution of NaOH. Write the corresponding chemical reactions.
You make an ideal solution of acetic acid in 945.9 g of water. The freezing point of this solution is -0.27 °C. What is the pH of the solution? The freezing point depression constant for water is 1.86 °C • kg • mol-¹ and the density of water is 0.9978 g/mL. The pKa of acetic acid is 4.76, the molar mass is 60.052 g/mol and the density is 1.05 g/mL.
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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!
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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.
Determine the pH of the resulting solution when the following two solutions are mixed: 50.0 mL of 0.500 M HNO2 and 30.0 mL of 0.200 M Ca(OH).. The value of Ka for HNO2 is 6.8 × 104. 1 3 4 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HNO:(aq) ОН (аq) H:O(1) NO: (aq) + + Before (mol) Change (mol) After (mol) 5 RESET 0.500 0.200 +x -X 0.500 + x 0.500 - x 0.200 + x 0.200 - x 0.0060 -0.0060 0.0120 -0.0120 0.0250 -0.0250 0.0190 -0.0190 0.0130 -0.0130
Which of the following is true for the reaction of BF3 + HF HBF4? BF3 is the Lewis Base BF3 is the Arrhenius base BF3 donates an electron pair HF accepts an electron pair HF is the Lewis Base Suppose you have 0.6 M solution of acid HB. Suppose further that K, <« 1 for this acid. Wsich of the following statements is true? (<) indicates much less. [H") and (8) are exactly 0.3 M [H') and (B] are <« 0.6 M (H'] and (B') are approximately 0.6 M [H'] and (B1 are < 0.6 M [H"] and (B] are exactly O M

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