Why is .05 or 0.1N solution of NaOH or HCl used in titrating and 1N solution in adjusting the pH of the remaining medium?

A buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.

A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.

In developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.

Why is .05 or 0.1N solution of NaOH or HCl used in titrating while 1N solution is used in adjusting the pH of a sample?

3. A 20.0 mL sample of 0.200 M cyanic acid (HOCN, Ka-3.3 x 104) is titrated with 0.400 M NaOH. Calculate the pH and % dissociation of the cyanic acid solution before any NaOH solution has been added. (a) (b) Calculate the pH of the solution after 3.00 mL of NaOH solution has been added. Calculate the pH of the solution at the half equivalence point. (c) (d) Calculate the pH of the solution at the equivalence point. and I 11

A chemistry graduate student is given 100. mL of a 0.60M diethylamine ((C,H,) NH) solution. Diethylamine is a weak base with K, = 1.3 × 10¯. what mass of (C,H5),NH,Cl should the student dissolve in the (C,H;), NH solution to turn it into a buffer with pH = 11.30? You may assume that the volume of the solution doesn't change when the (C,H,) NH,Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

1. How many moles of sodium hydroxide would have to be added to 125 mL of a 0.339 M hypochlorous acid solution, in order to prepare a buffer with a pH of 7.530? 2.

A chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution. Diethylamine is a weak base with K,=1.3 × 10 °. What mass (HIN %3D of (C,H5), NH,Br should the student dissolve in the (C,H,) NH solution to turn it into a buffer with pH =10.79? 2. You may assume that the volume of the solution doesn't change when the (C,H) NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round 12 it to 2 significant digits. 10

A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)