Calculate the pH of a 0.100 M NaCH 3CO 2 solution. Ka for acetic acid, CH 3CO 2H, is 1.8 × 103.

What is the pH of a 0.950 M solution of Na2HPO4?

Calculate the pH at 25 °C of a 0.23 M solution of sodium hypochlorite (NaClO). Note that hypochlorous acid (HCIO) is a weak acid with a pK, of 7.50. a Round your answer to 1 decimal place. pH = 0 ?

A 450.0 mL solution contains 0.42 M KCIO. What is the pH? Ka (HCIO) = 2.90 x 10^-8. Report your answer with two decimal places.

Richard and Jessica are lab partners. They pour 40.0 mL of a 0.200 M HC2H3O2 solution into a 250 mL flask. They then set up a burette and add 0.250 M NaOH solution to the burette. They are asked to fill in the table below. The first box asks for the pH of the acetic acid without any NaOH added. The second through tenth boxes show the pH after the indicated amounts of NaOH are added to the acetic acid solution. Please show your work for the first, sixth and tenth boxes. The initial reaction is: H₂O (L) + HC2H3O2 (aq) = H₂O* (aq) + C₂H₂O₂ with Ka = 1.8 x 105 and the reaction involving NaOH is: NaOH (aq) + HC₂H₂O₂ (aq) = H₂O (L) + C₂H₂O₂ (aq). mL of NaOH added pH Box 1 work 0.00 2.72 4.00 8.00 3.46 3.99 12.00 16.00 4.37 H3O+ HCz HyOz | Hz H3 C2H3O2 20.00 24.00 28.00 32.00 36.00 Initial .200 0 PH= 2.72 change -X X X Equilibrium 200-x 1.8×10-5 = x² X X = 3.6 × 10-6 = √x²= √3.6×10-6 1 .200 Box 6 work Box 10 work [H 301 = 0.00189 pH = 100 [H3O+] =

Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Kå for HBrO₂ = 5.6 x 10-7 and K for Ca(OH)2 > 1.

What is the pH of a 0.950 M solution of Na2HPO4? H3PO4 is a weak polyprotic acid with Ka1 = 7.2×10‒3, Ka2 = 6.3×10‒8, and Ka3 = 4.2×10‒13.

A weak base has a base hydrolysis constant, Ko, of 3.1 × 106. What is the pH of a 0.11 M solution of the weak base? pH =

Estimate the calcium concentration (in ppm by mass) in a groundwater sample, which has a pH of 5.63. Assume that the groundwater at this location is saturated with CO2 at a partial pressure of 0.185 atm. The atomic weight of calcium is 40.1 g/mol.

A weak acid is added to a strong base. The base is neutralized last, giving a mole ratio to acid remaining of 2:3. If Ka is 1.0 x 10-5, what is the ph of the solution?