TAPS is the acronym of ((tris(hydroxymethyl)methylamino)propanesulfonic acid), which is a chemical compound commonly used to make buffer solutions. A TAPS buffer solution is prepared by mixing 2 solutions. The first solution is 200.0 mL and it contains 52.661 grams of TAPS. The buffer solution is prepared by adding 51.92 mL 0.9832 M KOH solution to the first solution. Assume that the volume is additive. At 25 °C, the pKa of TAPS is 8.441. C7H₁7NO6S + KOH → C₂H₁6NO6SK + H₂O Determine the equilibrium concentration of TAPS in the buffer solution. Please provider your answer below. A. B. Determine the equilibrium concentration of C₂H₁6NO6SK in the buffer solution.. Please provider your answer below. 00 0² 0₂ C. Determine the pH of the buffer solution. pH = n A M M

A 31.8 mL sample of a 0.528 M aqueous acetic acid solution is titrated with a 0.422 M aqueous sodium hydroxide solution. What is the pH after 26.5 mL of base have been added? pH =

When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. Titration of (5.15400x10^-1) grams of monoprotic weak acid (dissolved in KCI) required (2.2540x10^1) mL of (1.979x10^-1) molar NaOH solution to reach equivalence. Based on this information, what is the molar mass of the weak acid? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10 Answer units

-2 What volume in milliliters of 9.850 x 10 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 14.0 mL sample of 0.144 M phosphoric acid? Express your answer using three significant figures.

By titration, it is found that 36.7 mL of 0.117 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.  I got 0.14862 - but is wrong.

A 35.8 mL sample of a 0.321 M aqueous acetic acid solution is titrated with a 0.408 M aqueous potassium hydroxide solution. What is the pH after 17.3 mL of base have been added?

please answer all of them especially at 50 ml. Thank you. Consider the titration of 80.0 mL of 0.100 M  Ba(OH)2 by 0.400 M HCl . Calculate the pH of the resulting solution after the following volumes of  have been added. 0.0 mL pH =  20.0 mL pH =  30.0 mL pH =  40.0 mL pH =  50.0 mL pH =

An analytical chemist weighs out 0.275 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0500M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 73.3 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol x10 X S

Solid potassium chromate is slowly added to 50.0 mL of a calcium nitrite solution until the concentration of chromate ion is 0.0247 M. The maximum amount of calcium ion remaining in solution is

A 18.8 mL sample of a 0.424 M aqueous acetic acid solution is titrated with a 0.331 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added? pH =