Calculate the pH and concentrations of H, A, HA", and A?-, at equilibrium for a 0.115 M solution of Na, A. The acid dissociation constants for H, A are K = 6.94 × 10° and K2 = 3.11 x 10-9. pH = M (A?-) =
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- The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.010 M solution of HClO isA 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?Use the References to access important values if needed for this question. The pOH of an aqueous solution of 0.580 M nitrous acid, ( Ka(HNO2) = 4.5 x 10^-4) is
- What is the pH of the solution after mixing 0.188 g of Mg(OH)2 (MW=58.321 g/mol) with 18.1 mL of 0.0173 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.calculate the pH of a solution that is 1.00 M CH3COOH (ka = 1.0 x 10^-5) and 1.00 M CH3COONaWrite both the charge balance equation (CBE) and mass balance equation (MBE) for the following solutions at equilibrium: 1. 0.12 M H2A 2. 0.40 M NH4Cl
- Calculate the pH of a 0.38 M weak acid HA solution at 25°C. Ka = 1.6 x 10-6Calculate the pH of a solution that is 0.553 M nitrous acid (HNO2) and 0.663 M of potassium nitrite (KNO2). The acid dissociation constant of HNO2 is 4.50 x 10-4.Hi, A weak acid is added to a strong base. The base is neutralized, 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? Thanks,
- For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surelywhat volume of sodium sulfate 0.1 M and how many grams of sodium hydrogen sulfate (NaHSO4 . H2O) should be added together to produce a solution with a pH of 1.9? (Ka for HSO4-=1.2*10-2)One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9