Use an ICE table, including a chemical equation at thetop, to aid in the follwing calculation. A solution of thesalt (CH2OH)3CNH3CI has a concentration of 0.00458M. The Kb for (CH2OH)3CNH2 is 8.3 x 10^-9. Findthe hydronium ion concentration in the salt solution

Step 1: Tris-aminomethane hydrochloride, or (CH2OH)3CNH3Cl, is a weakly acidic salt that is a…

Answered: Use an ICE table, including a chemical…

Chemistry

9th Edition

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Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 111IP: Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of...

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of barium nitrate is added. Assuming no change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.
Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.
A scientist has synthesized a diprotic organic acid, H2A, with a molar mass of 124.0 g/mol. The acid must be neutralized (forming the potassium salt) for an important experiment. Calculate the volume of 0.221 M KOH that is needed to neutralize 24.93 g of the acid, forming K2A.
If one mole of the following compounds were each placed into separate beakers containing the same amount of water, rank the Cl(aq) concentrations from highest to lowest (some may be equivalent): KCl, AlCl3, PbCl2, NaCl, HCl, NH3, KOH, and HCN.
The composition diagram, or alpha plot, for the important acid-base system of carbonic acid, H2CO3, is illustrated. (See Study Question 1.7 for more information on such diagrams.) (a) Explain why the fraction of bicarbonate ion, HCO3, rises and then falls as the pH increases. (b) What is the composition of the solution when the pH is 6.0? When the pH is 10.0? (c) If you wanted to buffer a solution at a pH of 11.0, what should be the ratio of HCO3 to CO32?
Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture of NaHCO3 and Na2CO3 was titrated, what would be the relative sizes of V1, and V2? b. If a mixture of NaOH and Na2CO3 was titrated, what would be the relative sizes of V1 and V2? c. A sample contains a mixture of NaHCO3 and Na2CO3. When this sample was titrated with 0.100 M HCl, it took 18.9 mL to reach the first stoichiometric point and an additional 36.7 mL to reach the second stoichiometric point. What is the composition in mass percent of the sample?
A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).
4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.
What is the concentration (in molarity) of H+, HCO3−, and CO32–, in a solution that is initially prepared as a mixture of 0.0100 M H2CO3 and 0.000010 M Na2CO3? (Carbonic acid is a weak diprotic acid where Ka1 is 4.20 x 10–5 and Ka2 is 2.00 x 10–6) a) [H+] at equilibrium = ? b) [HCO3-] at equilibrium = ? c) [CO32-] at equilibrium = ?
1. 0.200 M acetic acid is added to water. What is the concentration of H3O* in solution if Kc=1.8x10-6? 2. After an all-night drinking binge, a man pukes 300.0mL of liquid into his trash can. Assuming the puke is 20% HCI and the rest does not affect the pH, what is the pH of the solution resulting from the puke being neutralized with 0.50M NH3? (Kb-1.8x105) 3. If the initial concentration of NH3 is 0.350 M and the concentration at equilibrium is 0.325 M, what is Kc for this reaction?
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Use an ICE table, including a chemical equation at the top, to aid in the follwing calculation. A solution of the salt (CH2OH)3CNH3CI has a concentration of 0.00458 M. The Kb for (CH2OH)3CNH2 is 8.3 x 10^-9. Find the hydronium ion concentration in the salt solution