A 29.9 mL sample of 0.252 M dimethylamine, (CH3)₂NH, is titrated with 0.355 M hydrochloric acid. The pH before the addition of any hydrochloric acid is

A 200.0 mL sample of 0.20 M Sr(OH)2 is titrated with 0.20 M HBr.  Determine the pH of the solution after the addition of 400.0 mL HBr. Enter the pH with only 2 sigfigs.

A chemistry graduate student is given 450. mL of a 1.10M dimethylamine (CH.) NH) solution. Dimethylamine is a weak base with K,=5.4 × 10 4. What mass of (CH,),NH,CI should the student dissolve in the (CH,), NH solution to turn it into a buffer with pH = 10.89? You may assume that the volume of the solution doesn't change when the (CH,),NH,CI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?

If 100.0 g calcium phosphate (Ksp= 1.3 x 10^-32) are placed in enough water to generate 750.0 mL of solution, calculate the molar solubility of the calcium phosphate solution and the molar solubility of the calcium ion if 30.0 mL of 0.400 M calcium nitrate solution is added to the original solution.

A buffer solution contains 0.210 M NH4Cl and 0.358 M NH3 (ammonia). Determine the pH change when 0.100 mol HBr is added to 1.00 L of the buffer.

A solution contains CO32– at a concentration of 0.0023 M and Cl– at a concentration of 0.00076 M. If AgNO3(aq) is added drop by drop to the solution, which ion, CO32– or Cl–, will precipitate first? Give the minimum concentration of Ag+ needed to precipitate each of the