Reference no: EM131430130

Calculate the pH of a solution that is 0.189 M (CH₃)₃N and 0.323 M (CH₃)₃NHCl.K_bof (CH₃)₃N is 6.5 x 10^-5? 

The pH of 0.50 M HF is 1.88. Calculate the pH difference when 0.69 g of NaF is added to 13 mL of 0.50 M HF. Ignore any changes in volume. The K_a value for HF is 3.5 x 10^-4?

Calculate the pOH of a solution that results from mixing 73 mL of 0.13 M acetic acid with 49 mL of 0.12 M sodium acetate.  The K_a value for CH₃COOH is 1.8 x 10^-5?

What is the buffer component ratio, (BrO^-)/(HBrO) of a bromate buffer that has a pH of 8.08 K_a of HBrO is 2.3 x 10^-9?

A buffer that contains 0.15 M of a base, B and 0.21 M of its conjugate acid BH⁺, has a pH of 9.59. What is the pH after 0.03 mol of NaOH are added to 0.88 L of the solution?

Calculate the pH during the titration of 35 mL of 0.2 M KOH(aq) with 0.12 M HBr after 10 mL of the acid have been added?

Calculate the pH during the titration of 20.00 mL of 0.1000 M C₆H₅OH(aq) with 0.2000 M NaOH(aq) after 4 mL of the base have been added. K_a of phenol = 1.0 x 10^-10?

Calculate the pH during the titration of 20.00 mL of 0.1000 M hydrazine, NH₂NH₂(aq), with 0.2000 M HBr(aq) after 3 mL of the acid have been added. K_b of hydrazine = 1.7 x 10^-6? 

^{Calculate the pH during the titration of 30.00 mL of 0.1000 M methylamine, CH₃NH₂(aq), with 0.1000 M HCl(aq) after 29 mL of the acid have been added. K_b of methylamine = 3.6 x 10-4?}

Determine the volume in mL of 0.13 M LiOH(aq) needed to reach the half-equivalence (stoichiometric) point in the titration of 43 mL of 0.17 M formic acid(aq).  The K_a of formic acid is 1.8 x 10-4.

Determine the pH at the equivalence (stoichiometric) point in the titration of 48 mL of 0.25 M HClO(aq) with 0.15 M NaOH(aq).  The K_a of HClO is 2.3 x 10^-9?