What is the pH of 500ml solution conating 0.125 M fornic acid and 0.140 M sodium formate? Include chemical equation What would the pH be if 1mL of 0.5 HBr was added to solution? pka=3.744

Which of the following statements is/are true? (Select all that apply) OThe higher the concentration of OH in a solution, the lower the pH. OThe higher the concentration of OH in a solution, the lower the pOH. O An acidic solution has a pH of geater than 7. The concentration of H30* in pure water is 1.00 x 107 M. OA Bronsted acid is a proton donor in an acid-base reaction.

Calculate the pH of a solution that is 0.000846M HBr and 0.00125 M HCIO4. Answer:

The theoretical pK, of a weak acid is 3.54. Calculate the pK, experimental error of a solution composed of 10 mL of 0.23 M HA, 15 mL of 0.17 M of NaA and 20 mL of water. The measured - of C pH of this solution is 3.17. (Report only the numerical answer of the percent without the % symbol)

Which of the following are acid/base reactions? Select all that apply. 1. NaOH + FeI2  --> Fe(OH)2 + 2 NaI 2. NH3 + HCl  -->  NH4Cl 3. H2O + Cu  -->  CuO + H2 4. HNO2  + H2O -->  H3O+ + NO2- 5. None of the above

2. A solution contains 250 mL of 0.25M benzoic acid (HBen) and 0.20M sodium benzoate (NaBen). What is the pH of the solution after 25.0 mL of 0.10M HCI have been added? (Ka (HBen) = 6.5 x 10-5) (A) 4.19 (B) 4.107.9 (C) 4.28 c (D) 4.05

Calculate the pH of the solution when 10.0 mL of 0.15 M NH3 is titrated to the equivalence point with 0.15 M HClO4. Kb of NH3 is 1.8 × 10–5 at 25°C.   Correct Answer is 5.19 why

The final part asks for molNaClO

Please correct answer and don't use hend raiting

Which of the following are neutralization reactions? Select all that apply. 1. HCl  + H2O -->  H3O+ + Cl- 2. NaNO2  + H2O -->  HNO2 + NaOH 3. HClO4 + NaOH --> H2O + NaClO4 4. H+ + OH-  --> H2O 5. None of the above