An analytical chemist is titrating 222.2 mL of a 0.3600M solution of methylamine (CH3NH₂) with a 0.8600M solution of HNO3. The pK, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 61.0 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 = X Ś

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An analytical chemist is titrating 200.9 mL of a 0.1300M solution of piperidine (C,H, NH) with a 0.6100M solution of HNO₂. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 19.4 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-0 X

An analytical chemist is titrating 208.8mL of a 0.7500M solution of methylamine CH3NH2 with a 0.5600M solution of HNO3 . The pKb of methylamine is 3.36 . Calculate the pH of the base solution after the chemist has added 236.8mL 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.

An analytical chemist is titrating 135.0 mL of a 0.06400M solution of piperidine (CH,NH) with a 0.4700M solution of HNO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 21.3 mL of the HNO 3 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 3 solution added. Round your answer to 2 decimal places. pH = 0 ×

An analytical chemist is titrating 102.2 mL of a 0.1400 M solution of dimethylamine ((CH,) NH) with a 0.7900 M solution of HNO,. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 19.5 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 = Explanation Check 2021 McGraw-Hil Terms of Use

A chemist titrates 180.0 mL of a 0.3545M ammonia (NH3) solution with 0.7205M HBr solution at 25 °C. Calculate the pH at equivalence. The pk, of ammonia is 4.75. 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 HBr solution added. -0 pH = X

A solution which is yellow in the presence of alizarin yellow indicator and red in the presence of phenolphthalein, must have a pH which is in what range? Refer to precision of indicators in the picture    what is the lowest possible ph and the highest possible ph ?

An analytical chemist is titrating 94.2 mL of a 0.4600M solution of dimethylamine ((CH,),NH) with a 0.2300M solution of HNO,. The p K, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 121.9 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 =||

Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry and agriculture. ???1 ???2 1.30 6.70 Calculate the pH for each of the points in the titration of 50.0 mL of 2.4 M H3PO3(aq) with 2.4 M KOH(aq). 1. Before any addition of KOH 2. After addition of 25 mL of KOH 3. After addition of 50 mL KOH