Solid CO2 (0.42 mol) is reacted with CH3MGB (0.29 mol) in ether solvent. The product of the reaction is isolated in aqueous solution (assume 100% yield) and excess CO2 is removed. Subsequently, HCI (aq) (0.06 mol) is added. What is the pH of the solution that results? Notes: You will need to look up a pk, for this question and report your answer to 2 decimal places. Your Answer:

A 100.0 mL solution containing 0.973 g of maleic acid (MW 116.072 g/mol) is titrated with 0.364 M KOH. Calculate the pH of the solution after the addition of 46.0 mL of the KOH solution. Maleic acid has pK, values of 1.92 and 6.27. pH At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H, M, HM¯, and M2-, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. [M²-] = M [HM-] = M [H,M] = M

An analytical chemist is titrating 122.4 mL of a 0.2000M solution of propylamine (C,H,NH,) with a 0.07300M solution of HNO2. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 122.3 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. PH = Explaion Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Priva

A chemist titrates 90.0 mL of a 0.5350M trimethylamine ((CH3)N) solution with 0.1600M HCl solution at 25 °C. Calculate the pH at equivalence. The pK₂ of trimethylamine is 4.19. Round your answer to 2 decimal places. ? Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = ☐ X Ś olo

Incorrect Your answer is incorrect. • KC: Your answer is incorrect. • Cacl, Vour answer is incorrect. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll ind K, data in the ALEKS Data tab. Does enlubility change with pH? hiyhest solubility compound pll 5 pll 6 pll 8 yes O no yes Ba(OH), O no O yes Caci, e no

An analytical chemist is titrating 184.0 mL of a 0.5400M solution of propylamine (C,H,NH,) with a 0.8600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 60.2 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 191.3 mL of a 0.2000 M solution of propylamine (C,H,NH,) with a 0.1100 M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 416.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

You have 0.600 L of an 0.300 M acetate buffer solution (i.e. [HC;H,O2] + [C,H¿O¿¯] = 0.300 M) at pH 5.30. What will the new pH of the solution be if you add 82.0 mL of 1.000 M HCI to it. Acetic acid has a pKa of 4.74.

An analytical chemist is titrating 71.3 mL of a 1.000M solution of formic acid (H,CO,) with a 0.6600M solution of KOH. The pK, of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 119. mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH Solution added. Round your answer to 2 decimal places. pH =

An analytical chemist is titrating 75.2 mL of a 0.5800 M solution of trimethylamine ((CH3)N) with a 0.2600M solution of HNO3. The p K₂ of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 197.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X 5 4