pka of 4.9 what is the weak acid and conjugate base pH of buffer solution is 5.90

An analytical chemist is titrating 239.3 mL of a 0.8400M solution of methylamine (CH, NH,) with a 0.3300M solution of HNO,. The p K, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 257.2 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. pH =

The fumarate ion is a dibasic base with pKb values of 9.52 and 10.98. What is the concentration of the fumarate ion (B) in a 0.100 M solution of disodium fumarate that is buffered at pH 5.21? SOLVE FOR CONCENTRATION NOT PH

The percent dissociation of veronal (diethyl barbituric acid) in a 0.010 M aqueous solution is 0.16%.  What is the pH of the solution and what is the Ka of veronal?

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

Which of the following equal molar salt solutions has the highest pH? (Nat is neutral.) NACIO Nalo NaBrO More information is needed to make a determination.

Use the following information as a guide to help answer the next three questions. Your answer MUST be in the same format. Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between .0 and 7.6 6. Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Using the method outlined above in the example of bromothymol blue, indicate what the colours of the indicators tell us about the pH approximation of the solution. Values and wording are very important, so be precise. Be sure to word your pH approximation as outlined in the example. Indicator Colour pH approximation methyl red orange Indicator Colour pH approximation phenolphthalein colourless Indicator Colour pH approximation phenol red red

Calculate the pH of a solution prepared by mixing 1.50 g of imidazole with 1.50 g of imidazole hydrochloride and diluting to 100.0 mL. The pK, of imidazole hydrochloride is 6.993. pH = pH == 6.81 Incorrect Calculate the pH of the solution if 1.70 mL of 1.03 M HCIO, are added. 6,72 Incorrect volume: How many milliliters of 1.03 M HCIO, should be added to 1.50 g of imidazole to give a pH of 6.993? 6.73 Invert Curstinn San ml.

A buffer solution contains formic acid (0.75M) and an equal molar amount the sodium salt of its conjugate base. The Ka of formic acid is 0.00018. At what approximate pH does the solution buffer?

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0158 M solution. The pH of the resulting solution is 2.30. Calculate the pKa for the acid. pKa