What is the pH at the equivalence point when you mix 20mL of 0.1M of some acid with 40mL of 0.05M of some base? Ka = 1.74 * 10^-4

A solution is made by mixing 185 mL of 0.100 M formic acid (Ka = 1.7 x 10-4 ) with 190. mL of 0.100 M sodium formate. What is the pH of the solution? Express your answer in decimal notation rounded to three significant figures.

What is the pH of a solution prepared by combining 0.258 mol of a newly discovered weak acid (Ka = 1.3 x 10-4) with 0.156 mol of the salt containing its conjugate base in 1.4 L of water?

A solution is prepared that is initially 0.26M in hydrofluoric acid (HF) and 0.25M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H₂O*]. You can leave out the M symbol for molarity. initial change final [HF] 0 П [F] 0 0 0 [H₂O*] 0 0 0 X

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa). (K₂ = 6.5 × 10-5 for benzoic acid) a

What is the approximate pH at the equivalence point of a weak base-strong acid titration if 50.00 mL of aqueous ammonia (NH3) requires 37.10 mL of 0.1087 mol L-1 HCI? pK₁ =4.75 for ammonia. Report your answer in 2 decimal places.

We have a titration for the titration of 50.0 mL of 0.425 M lactic acid, a monoprotic acid, (Ka = 1.38 x 10^-4) with 0.350 M NaOH.  1. Calculate the exact volume of the NaOH needed (to the correct numbers of sig figs) to reach the equivalence point.  2. Calculate the exact volume of NaOH needed (to the correct numbers of sig figs) to reach the mid point.

What is the pH of a solution containing a mixture of 0.50 M HCN and 0.040 M NaCN?  (Ka = 4.9 x 10-10 for HCN ).

What is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10-5) when 100.0 mL of a 0.0.75 M HCl solution is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ?Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.

What is the pH of an aqueous solution made by mixing 300 mL of 0.10M hydrofluoric acid (pKa= 3.18) with 200 mL of 0.10M potassium hydroxide?