A sample of water was alkaline both to phenolphthalein and methyl orange. 100 mL of this water sample required 20 mL of N/50 HCl for phenolphthalein end point and another 15 mL for complete neutralization. Elucidate the type and strength of alkalinity present in the water sample

Why is the pH of mixture D the same as the pH of mixture B? B 0.1 mol L–1 CH3COOH   Conductivity (mA)   5 PH 3 D Mixture made by mixing equal volumes of 0.2 mol L–1 HCl and 0.2 mol L–1 NaCH3COO Conductivity (mA) 80 pH 3

A chemist titrates 80.0 mL. of a 0.0754 M aniline (C6H5NH2) solution with 0.5961 M HBr solution at 25 °C. Calculate the pH at equivalence. The pKa of aniline is 4.87. 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.

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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

An analytical chemist is titrating 83.2mL of a 0.6200M solution of diethylamine C2H52NH with a 0.3300M solution of HNO3 . The pKb of diethylamine is 2.89 . Calculate the pH of the base solution after the chemist has added 28.7mL 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.

Calculate the pH of a solution prepared by mixing 1.70 g of imidazole with 1.70 g of imidazole hydrochloride and diluting to 100.0 mL. The pKa of imidazole hydrochloride is 6.993. pH = Calculate the pH of the solution if 1.50 mL of 1.07 M HCIO are added. pH = How many milliliters of 1.07 M HClO4 should be added to 1.70 g of imidazole to give a pH of 6.993? volume: mL

An analytical chemist is titrating 156.3 mL of a 0.4800M solution of propylamine (C₂H,NH2) with a 0.1500M solution of HNO3. The pK of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 79.5 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 HNO3 solution added. Round your answer to 2 decimal places. pH ☐ G

When titrating 25 mL of an approximately 0.1 M solution of a triprotic acid solution with 0.1052 M NaOH, a student calculates that the end point will be reached after the addition of approximately x mL of NaOH. However, after the addition of 2x mL of sodium hydroxide, no colour change is observed.  Which of the following errors could not account for this obervation?        using a 3 mole acid : 1 mole base ratio in the calculation      washing the sides of the flask with DI water during the titration and diluting the analyte solution      mistakenly using a 0.01000 M NaOH solution in the titration      failing to add an indicator to the analyte solution      mistakenly using a primary standard solution of > 1.0 M in the titration

The pK₂ of acetic acid, HC₂H3O2, is 4.96. A buffer solution was made using an unspecified amount of acetic acid and 0.1 moles of NaC2H3O2 in enough water to make 1.82 liters of solution. Its pH was measured as 4.04. How many moles of HC2H3O2 were used? Report your answer with 2 places past the decimal point. Do not put unit in your answer.