A pure sample of a monoprotic acid is dissolved in water. The sample is titrated with sodium hydroxide solution. At the point where 20.0 mL of the NaOH solution has been added, the pH is 4.15. The phenolphthalein endpoint of the titration is observed when 50.0 mL of NaOH have been added. What is the pKa of the acid? (A) 4.15  (B) 4.33  (C) 4.55  (D) 5.19 Correct answer is B but I can't figure out how to get that answer. Please show your work.

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.

The acid HX has a pKa of 5.00.  If 25.00 mL of a 0.106 M solution of HX are titrated with 0.100 M NaOH solution, what's the pH after 11.28 mL ofbase solution is added?

A formic acid buffer solution contains 0.20 M  HCOOHHCOOH  and 0.24 M  HCOO−HCOOX− The pKa of formic acid is 3.75. What is the pH of the buffer?

Calculating the pH of å Weak Base lilla An analytical chemist is titrating 61.7 mL of a 0.3400M solution of aniline (CH,NH, with a 0.8400M solution of HIO3. The p K, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 10.9 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. dh pH = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility 24 MacBook Air

You need to prepare an acetate buffer of pH 5.455.45 from a 0.843 M0.843 M acetic acid solution and a 2.06 M KOH2.06 M KOH solution. If you have 630 mL630 mL of the acetic acid solution, how many milliliters of the KOHKOH solution do you need to add to make a buffer of pH 5.455.45? The p?apKa of acetic acid is 4.76.4.76. Be sure to use appropriate significant figures.   mL

Calculate the ratio of conjugate base to weak acid needed to make a buffer at pH 4.75 if the pKa of the acid is 5.32.

An analytical chemist is titrating 70.8mL of a 0.7400M solution of butanoic acid HC3H7CO2 with a 1.100M solution of KOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 55.5mL 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.

What is the pH of an aqueous solution containing 75.0 mL of a 0.15M HNO2 solution and 45.0 mL of a .25M KNO2? What is the pH of this solution after 10.0 mL of a 0.20M solution of KOH is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)?

An analytical chemist is titrating 106.5 mL of a 0.1100 M solution of methylamine (CH3NH₂) with a 0.8500M solution of HNO3. The p K₁ of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 11.6 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 × S