4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid used to prepare buffers for biological samples through combination with strong bases. How many mL of 0.626 M KOH should be added to 5.00g of MOBS (pKa=7.48 and formula mass is 223.29 g/mol) to give a pH of 7.40

An analytical chemist is titrating 143.6 mL of a 0.7000M solution of piperidine (C,H10NH) with a 0.4000M solution of HNO3. The p K, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 267.7 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

An analytical chemist is titrating 64.8mL of a 0.3000M solution of ammonia NH3 with a 0.7300M solution of HNO3 . The pKb of ammonia is 4.74 . Calculate the pH of the base solution after the chemist has added 31.6mL 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 169.4 mL of a 1.000M solution of butanoic acid (HC3H,CO₂) with a 1.100M solution of KOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 183.1 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 = ☑

How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid, HBrO, to form a buffer solution of pH 8.95? The Ka of HOBr is 2.0 × 10–9. Express your answer in moles using at least three significant figures. Do not use scientific notation.

An analytical chemist is titrating 164.9 mL of a 0.4100M solution of hydrazoic acid (HN3) with a 0.9800M solution of KOH. The pK of hydrazoic acid is 4.72 Calculate the pH of the acid solution after the chemist has added 76.81 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 = M

a An analytical chemist is titrating 233.8 mL of a 0.9100M solution of hydrazoic acid (HN3) with a 1.100M solution of NaOH. The pK of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 70.25 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH 0 = X

Nitesh

Many drugs administered to patients are actually primary amine (RNH2 derivatives).  These drugs may be very hydrophobic but are made water soluble by making them as mine salts.  A synthetic chemist treats the primary amine derivative with a strong acid like hydrochloric acid to make the amine salt.  Calculate the pH at the equivalence point in the titration of 75 mL of 0.10 M Methylamine with a 0.30 M HCl solution. The Ka for methylamine (CH3NH2) is 2.3X10-11.

An analytical chemist is titrating 116.2mL  of a  0.5100M  solution of butanoic acid  HC3H7CO2  with a  0.5000M  solution of  NaOH . The  pKa  of butanoic acid is  4.82 . Calculate the pH of the acid solution after the chemist has added  139.9mL  of the  NaOH  solution to it.   Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH  solution added.   Round your answer to 2  decimal places.