Determine the pH of a solution with [OH] = 1.8  10-4 M and indicate if thesolution is acidic, basic, or neutral.

Determine the pH of a solution that is 0.50 M CH3COOH and 0.30 M CH3COONa.

Calculate the PH of a solution that is 0.0011M in HCl and 0.012M in HClO2. Express your answer using three decimal places.

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0154 M solution. The pH of the resulting solution is 2.46. Calculate the Ka for the acid.

Which one of the following correctly shows the weak acid equilibrium for trichloroacetic acid, CCI,COOH? A) CCI,COOH (aq)= CC,Co (aq) + ОН (аq) в) ССІ СООН (аq) + н.о () — CC,COOH, (aq) + OH (aq) С) CI СООH (aq) + Н,О (1) CCI,CoO (aq) + H,0* (aq) D) CCI,COOH (aq) + H,O (1) = CC,CO(OH), (aq) + H* (aq)

Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215 mol/L H2NNH3Br solutionGive an answer to at least 3 decimal places. Next, calculate the pH of this same solution if 12.00 mL of 0.300 mol/L HNO3 is added.Give an answer with at least 3 decimal places.

Calculate the ph of a solution that is 0.040 M in HI.

Calculate the pH of an aqueous solution that is 0.35 M NH3 and 0.15 M NHẠNO3 given that the K of NH3 is 1.8x10-5. Express your answer in decimal notation rounded to three significant figures.

If 15.0 mL of glacial acetic acid (pure HC2H3O2) is diluted to 1.70 L with water, what is the pH of the resulting solution? The density of glacial acetic acid is 1.05 g/mLpH=?

If a solution has a concentration of hydronium ions less than 1.0 x 10-12 M would it be considered acidic or basic?